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Case Study Question 1 on Chemical Kinetics – Chapter 4 CBSE Class 12 Chemistry

• April 6, 2022
• Class 12 , Chemistry , CBSE

Case Study Question 1 on Chemical Kinetics – Chapter 4

Read the given passages and answer the questions that follow..

Question. The rate of a chemical reaction is expressed either in terms of decrease in the concentration of a reactant per unit time or increase in the concentration of a product per unit time. Rate of the reaction depends upon the nature of reactants, concentration of reactants, temperature, presence of catalyst, surface area of the reactants and presence of light. Rate of reaction is directly related to the concentration of reactant. Rate law states that the rate of reaction depends upon the concentration terms on which the rate of reaction actually depends, as observed experimentally. The sum of powers of the concentration of the reactants in the rate law expression is called order of reaction while the number of reacting species taking part in an elementary reaction which must collide simultaneously in order to bring about a chemical reaction is called molecularity of the reaction.

1. Express the rate of the following reaction in terms of different reactants and products.

4NH 3 (g) + 5O 2 (g) —–> 4NO 2 (g) + 6H 2 O(g)

2. Why do pieces of wood burn faster than a log of wood of the same mass?

Ans. Pieces of wood have larger surface area than the log of wood of the same mass. Greater the surface area, faster is the reaction.

3. Why does the rate of any reaction generally decrease during the course of the reaction?

Ans. The rate of reaction depends on the concentration of reactants. As the reaction progresses, reactants start getting converted to products so the concentration of reactants decreases hence the rate of reaction decreases.

4. Why is molecularity applicable only for elementary reactions and order is applicable for elementary as well as complex reactions?

Ans. A complex reaction proceeds through several elementary reactions. Number of molecules involved in each elementary reaction may be different, i.e., the molecularity of each step may be different. Therefore, discussion of the molecularity of overall complex reaction is meaningless. On the other hand, order of a complex reaction is determined by the slowest step in its mechanism and is not meaningless even in the case of complex reactions.

5. The kinetics of the reaction

mA + nB + pC —–>  m′X + n′Y + p′Z

obey the rate expression dx/dt = k[A] m [B] n

Calculate total order and molecularity of the reaction.

Ans. The total order of reaction = m + n

The molecularity of the reaction = m + n + p

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Get here all the Important questions for Class 12 Chemistry chapter wise as free PDF download. Here you will get Extra Important Questions with answers, Numericals and Multiple Choice Questions (MCQ's) chapter wise in Printable format. Solving Chapter wise questions is one of the best ways to prepare for the examination. Students are advised to understand the concepts and theories of Chemistry properly before the exam. You can easily find 1 Mark, 2 marks, 3 marks, and 5 marks questions from each chapter of Class 12 Chemistry and prepare for exam more effectively. These preparation material for Class 12 Chemistry , shared by teachers, parents and students, are as per latest NCERT and CBSE Pattern syllabus and assure great success in achieving high score in Final CBSE Board Examinations.

Latest MCQ's and Important Questions for CBSE Class 12 Chemistry

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Total Papers :

CBSE Class 12 Chemistry Syllabus

• Solid State
• Electrochemistry
• Chemical Kinetics
• Surface Chemistry
• General Principles and Processes of Isolation of Elements
• p-Block Elements
• d- and f-Block Elements
• Coordination Compounds
• Haloalkanes and Haloarenes.
• Alcohols, Phenols and Ethers
• Aldehydes, Ketones and Carboxylic Acids
• Organic compounds containing Nitrogen
• Biomolecules
• Chemistry in Everyday life

Unit II: Solutions 15 Periods

Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in liquids, solid solutions, Raoult's law, colligative properties - relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular mass, Van't Hoff factor.

Unit III: Electrochemistry 18 Periods

Redox reactions, EMF of a cell, standard electrode potential, Nernst equation and its application to chemical cells, Relation between Gibbs energy change and EMF of a cell, conductance in electrolytic solutions, specific and molar conductivity, variations of conductivity with concentration, Kohlrausch's Law, electrolysis and law of electrolysis (elementary idea), dry cell-electrolytic cells and Galvanic cells, lead accumulator, fuel cells, corrosion.

Unit IV: Chemical Kinetics 15 Periods

Rate of a reaction (Average and instantaneous), factors affecting rate of reaction: concentration, temperature, catalyst; order and molecularity of a reaction, rate law and specific rate constant, integrated rate equations and half-life (only for zero and first order reactions), concept of collision theory (elementary idea, no mathematical treatment), activation energy, Arrhenius equation.

Unit VIII: d and f Block Elements 18 Periods

General introduction, electronic configuration, occurrence and characteristics of transition metals, general trends in properties of the first-row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7 and KMnO4.

Lanthanoids – Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.

Actinoids - Electronic configuration, oxidation states and comparison with lanthanoids.

Unit IX: Coordination Compounds 18 Periods

Coordination compounds - Introduction, ligands, coordination number, colour, magnetic properties and shapes, IUPAC nomenclature of mononuclear coordination compounds. Bonding, Werner's theory, VBT, and CFT; structure and stereoisomerism, the importance of coordination compounds (in qualitative analysis, extraction of metals and biological system).

Unit X: Haloalkanes and Haloarenes. 15 Periods Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation mechanism of substitution reactions.

Haloarenes: Nature of C–X bond, substitution reactions (Directive influence of halogen in monosubstituted compounds only). Uses and environmental effects of - dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT.

Unit XI: Alcohols, Phenols and Ethers 14 Periods

Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, uses with special reference to methanol and ethanol.

Phenols: Nomenclature, methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols.

Ethers: Nomenclature, methods of preparation, physical and chemical properties, uses.

Unit XII: Aldehydes, Ketones and Carboxylic Acids 15 Periods

Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, reactivity of alpha hydrogen in aldehydes, uses.

Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.

Unit XIII: Amines 14 Periods

Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, identification of primary, secondary and tertiary amines.

Diazonium salts: Preparation, chemical reactions and importance in synthetic organic chemistry.

Unit XIV: Biomolecules 18 Periods

Carbohydrates - Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); Importance of carbohydrates.

Proteins - Elementary idea of - amino acids, peptide bond, polypeptides, proteins, structure of proteins - primary, secondary, tertiary structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes. Hormones - Elementary idea excluding structure.

Vitamins - Classification and functions. Nucleic Acids: DNA and RNA.

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Case Study Questions for Class 12 Chemistry Chapter 15 Polymers

Case study questions for class 12 chemistry chapter 12 aldehydes, ketones and carboxylic acids, case study questions for class 12 chemistry chapter 4 chemical kinetics, case study questions for class 12 chemistry chapter 9 coordination compounds, case study questions for class 12 chemistry chapter 10 haloalkanes and haloarenes, case study questions for class 12 chemistry chapter 11 alcohols, phenols and ethers, case study questions for class 12 chemistry chapter 13 amines, case study questions for class 12 chemistry chapter 14 biomolecules, case study questions for class 12 chemistry chapter 8 the d- and f-block elements, case study questions for class 12 chemistry chapter 7 the p-block elements, case study questions for class 12 chemistry chapter 5 surface chemistry, case study questions for class 12 chemistry chapter 3 electrochemistry, case study questions for class 12 chemistry chapter 2 solutions, case study questions for class 12 chemistry chapter 1 the solid state.

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CBSE Board Class 12 Chemistry Case Based Questions With Solutions

CBSE Board Class 12 Chemistry Case Based Questions With Solutions to prepare for the upcoming term 1 board exams are given here. It is extremely helpful since the expert team has crafted this by following the Syllabus of class 12th. Case study questions are also known as passage based problems because it includes the paragraph from which 5 or more problems are curated. 

To solve these types of problems students need to have a thorough understanding of all the basics and fundamental concepts. Also, a student who is good in problem solving skills can easily answer such questions.

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CBSE Class 12 Chemistry Case Based Questions, Assertion & Reason, MCQs

CBSE Class 12 Chemistry includes many chemical reactions, chemical bondings, theories, experiments, discoveries, etc. All of these types of things should be well versed by the students to answer the Case study, Multiple Choice Questions, Assertion and Reason. So, practicing the given CBSE Class 12 Chemistry Case Study PDF will be very handy in boosting the basic knowledge and preparing for the final papers. 

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CBSE Case Based Questions with Answers are designed and developed for the term 1 exam which is developed by the subject matter experts. The answers are provided to help the learners to solve the problem if they are stuck at some questions and don’t know how to tackle that.

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CBSE Class 12 Chemistry Case Study Questions PDF

Case studies play a pivotal role in CBSE Class 12 Chemistry, as they enable students to apply theoretical knowledge to real-life scenarios. CBSE Class 12 Chemistry Case Study Questions PDF section introduces the significance of case studies in enhancing analytical skills and understanding complex chemical reactions.

Case studies challenge students to think critically, analyze experimental data, and devise problem-solving strategies. They provide a deeper understanding of chemical principles and their practical applications, fostering a holistic learning experience. Familiarize yourself with the structure of case study questions to streamline your preparation. Each case study presents a unique chemical problem, encouraging students to identify relevant concepts and devise accurate solutions.

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Class 12 Chemistry Case Study Questions

CBSE Class 12 Chemistry question paper will have case study questions too. These case-based questions will be objective type in nature. So, Class 12 Chemistry students must prepare themselves for such questions. First of all, you should study NCERT Textbooks line by line, and then you should practice as many questions as possible.

Chapter-wise Solved Case Study Questions for Class 12 Chemistry

Class 12 students should go through important Case Study problems for Chemistry before the exams. This will help them to understand the type of Case Study questions that can be asked in Grade 12 Chemistry examinations. Our expert faculty for standard 12 Chemistry have designed these questions based on the trend of questions that have been asked in last year’s exams. The solutions have been designed in a manner to help the grade 12 students understand the concepts and also easy-to-learn solutions.

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Excel in your Chemistry exams with these practical tips.

A. Regular Practice with Case Studies

Consistent practice with case study questions enhances your ability to tackle complex problems. Dedicate time to solving various case studies to build confidence.

B. Understanding Analytical Skills

Develop strong analytical skills to approach case studies logically. Break down complex problems into simpler components and analyze them step-by-step.

C. Time Management Strategies

Allocate sufficient time for each case study during the exam. Practice time management in mock tests to complete the paper within the stipulated time.

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Strictly as per the new term-wise syllabus for Board Examinations to be held in the academic session 2024 for class 12 Multiple Choice Questions based on new typologies introduced by the board- Stand-Alone MCQs, MCQs based on Assertion-Reason Case-based MCQs. Include Questions from CBSE official Question Bank released in April 2024 Answer key with Explanations What are the updates in the book: Strictly as per the Term wise syllabus for Board Examinations to be held in the academic session 2024. Chapter-wise -Topic-wise Multiple choice questions based on the special scheme of assessment for Board Examination for Class 12th Chemistry.

Mastering CBSE Class 12 Chemistry case study questions is crucial for excelling in the exams. Embrace case studies as a valuable learning tool, and with practice, you’ll ace your Chemistry exams with confidence.

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• Enhanced Learning Experience : The case study PDF offers practical examples and scenarios, making the learning process engaging and relatable for students.
• Application of Theoretical Concepts : It enables students to apply theoretical knowledge to practical situations, honing their problem-solving and analytical skills.
• Real-World Relevance : By connecting classroom learning to real-life applications, students can grasp the practical significance of chemistry in various industries.
• Critical Thinking Development : Analyzing case studies encourages students to think critically and make informed decisions based on chemical principles.
• Exam Preparation : Exposure to case studies aids in better preparation for chemistry examinations by providing a comprehensive understanding of the subject.

The CBSE Class 12 Chemistry case study PDF brings a refreshing perspective to the world of education. By intertwining theoretical knowledge with practical applications, it equips students to face real-world challenges with confidence. The diverse case studies provide invaluable insights, encouraging students to explore chemistry beyond the classroom and make a positive impact on society.

What is the CBSE Class 12 Chemistry case study PDF?

The CBSE Class 12 Chemistry case study PDF is a curated document by CBSE, presenting real-life applications of chemistry concepts for students to understand the subject’s practical relevance.

How does the case study PDF benefit students?

The case study PDF enhances the learning experience, fosters critical thinking, promotes application-based learning, and prepares students for examinations.

Are the case studies diverse in content?

Yes, the case studies cover various branches of chemistry, including organic, inorganic, physical, environmental, and analytical chemistry.

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• Chemistry Concept Questions and Answers
• Kinetics Questions

Chemical Kinetics Questions

Chemical Kinetics deals with the rates of the reactions. The study of Kinetics involves the factors affecting the rate of the chemical reactions, the mechanisms and the transitions states involved, if any.

Chemical Kinetics Chemistry Questions with Solutions

Q1: What is the difference between the average rate and instantaneous rate?

Answer: Average rate is the rate measured for a long period of time. While the instantaneous rate is the rate measured for an infinitesimally small period of time.

Q2. What does the given graph represent about the nature of reaction? Which of the following expressions are in favour of the graph?

• Δ[A]/Δt = Δ[B]/Δt
• -Δ[B]/Δt = Δ[A]/Δt
• -Δ[A]/Δt = Δ[B]/Δt
• None of the above

Answer: (c.)

Explanation: The given graph represents that with the decrease in the concentration of A, the concentration of B increases. This implies that A is the reactant and B is the product of the reaction. The reaction can be represented as: A → B.

Since in this reaction, A is the reactant and B is the product; the change in concentration of either of A and B with time gives the rate of the reaction.

Hence, the average rate of formation of B can be written as: Δ[B]/Δt (with a + sign as the concentration of B increases through the reaction).

While the average rate of consumption of A can be written as: -Δ[A]/Δt (with a – sign as the concentration of A decreases through the reaction)

The correct expression for the reaction curves shown in the graph is -Δ[A]/Δt = Δ[B]/Δt.

Q3. The reaction rate of a substance is directly proportional to its_____.

Answer: Active Mass

The active mass is the concentration of the reacting substance in mol l -1 . Hence, the rate of the reaction of the substance is directly proportional to its active mass.

Q4. In the reaction rate expression, the change in concentration of each of the reactants and products are divided by the respective stoichiometric number present in the reaction equation. Why is this division done?

Answer: To understand the above fact, we must look at the following balanced equation:

2N 2 O 5 → 4NO 2 + O 2

The rate of decomposition of N 2 O 5 is -d[N 2 O 5 ]/dt. The rate of formation of NO 2 and O 2 are d[NO 2 ]/dt and d[O 2 ]/dt respectively.

However, these rates are not equal. This is because when 2 moles of N 2 O 5 decompose, 4 moles of NO 2 and 1 mole of O 2 are formed. This implies that the rate of decomposition of N 2 O 5 is twice the rate of formation of O 2 and the rate of formation of NO 2 is 4 times the rate of formation of O 2 .

Hence, the rate of formation of products and the rate of decomposition of the reactants are divided by their stoichiometric coefficients in the reaction in order to get an identical value for the rate of the reaction.

Therefore, the rate of reaction in terms of each of the reactants and the products is :

Rate of the reaction =

Q5. Calculate the rate of the reaction in terms of the different reactants and products for the following reaction.

4NH 3 (g) + 5O 2 (g) → 4NO (g) + 6H 2 O (g)

Given the rate of formation of NO is 3.6 x 10 -3 molL -1 s -1 , calculate the rate of disappearance of NH 3 and the rate of formation of H 2 O.

Answer: The rate of the reaction in terms of each of the reactants and products is given as:

Rate of Reaction =

Since, the coefficients of NO and NH 3 in the balanced chemical equation are the same, both of them have the same rate of formation and disappearance respectively.

Hence, rate of formation of NO = rate of disappearance of NH 3 = 3.6 x 10 -3 mol L -1 s -1

Now, the rate of reaction :

Hence, the rate of formation of water :

Hence, the rate of formation of water is 5.4 x 10 -3 mol L -1 s -1 .

Q6. Calculate the overall order from the given rate expressions.

• Rate = k[A] ½ [B] 3/2
• Rate = k[A] 3/2 [B] -1

Answer: The overall orders are calculated as:

• The order w.r.t. A = 1/2

The order w.r.t. B = 3/2

Overall Order = ½ + 3/2 = 2

• The order w.r.t. A = 3/2

The order w.r.t. B = -1

Overall Order = 3/2 – 1 = 1/2

Q7. The rate constants of 3 reactions are given. Identify the order of each of the given reactions.

• k = 2.3 x 10 -5 L mol -1 s -1
• k = 3.1 x 10 -4 s -1
• k = 9.3 x 10 -4 mol L -1 s -1

Answer: Since only rate constants for each reaction are given, the order of the reactions will be determined based on the units of the rate constants.

Q8. What are the differences between the rate of the reaction and the reaction rate constant?

Answer: The differences between the two are:

Q9. Give an example of the reaction of the 4th order.

Answer: The dissociation of potassium chlorate to form potassium perchlorate is an example of the reaction of 4th order.

4KClO 3 → 3KClO 4 + KCl

Q10. Derive the general expression of the time taken by the reactant to reduce to its nth fraction in the first order reaction.

Answer: Let us assume the initial amount of the reactant (A) = a

Hence, the nth fraction decreased from “a” in time t = a/n

From the first order reaction,

Hence, the general expression of the time taken by the reactant to reduce to its nth fraction in the first order reaction is represented by t = (2.303/k) logn.

Q11. The half-life period of a 1st order reaction is 60 min. What percentage of the substance will be left after 240 min?

Answer: 1 half-life period = 60 min

Number of half-lives after 240 min = 240/60 = 4 hal-lives i.e. n = 4

Amount of substance left after n half-lives = A o /2 n

Percentage of the amount of substance left after 4 half-lives = A o /2 4 x 100 = A o /16 x 100 = 6.25% of A.

Q12. The dissociation of N 2 O 5 in CCl 4 takes place by the 1st order rate law. The table below shows the concentration of N 2 O 5 measured at different times.

From the given observations, calculate k at t = 410 s and t = 1130 s.

Answer: From the first order rate law:

So, the value of k for the given reaction at t = 410 s is 7.768 x 10 -4 s -1 and that at t = 1130 s is 7.341 x 10 -4 s -1 .

Q13. A 1st order reaction gets 40% completed in 50 minutes. Calculate:

(i.) the rate constant

(ii.) the time in which the reaction will get 80% completed.

Answer: (i.) From the 1st order:

Where 𝑥 = (40/100)a = 0.4a, t= 50 min

The rate constant for the reaction is 0.010216 min -1 .

(ii.)To determine t = ?, 𝑥 = 0.8a

As k is constant for a given reaction, k = 0.010216 min -1

Hence, the time in which the reaction will get 80% completed is 157.58 min.

Q14. Determine the order of a reaction whose rate constant has the same unit as the rate of the reaction.

Answer: Zero Order reaction.

Q15. A reaction is 2nd ordered w.r.t. a reactant. Determine the change in the rate of the reaction when the amount of the reactant is:

• Reduced to its half

Answer: For a 2nd order reaction, Rate = k[A] 2 = ka 2

• When A = 2a, Rate = k(2a) 2 = 4.ka 2 , the reaction rate increases 4 times.
• When A = ½ a, Rate = k(½ a) 2 = ¼ times, the reaction rate decreases by ¼ times.

Practise Questions on Chemical Kinetics

Q1. The given reaction is carried out in a closed vessel:

2N 2 O 5 (g) ⇌ 4NO 2 (g) + O 2 (g)

It was observed that the concentration of NO 2 increased by 2.0 x 10 -2 mol L -1 within 5 seconds of the reaction. Calculate:

(i.) the rate of the reaction.

(ii.) the rate of change of concentration of N 2 O 5 .

Q2. For A → Products, k = 2.0 x 10 -2 s -1 . Calculate the concentration of A after 100 s.

Given [A] o = 1.0 mol L -1

Q3. The equation followed by the composition of a hydrocarbon is:

k = (4.5 x 10 11 s -1 )e -28000 K/T

Calculate the E a .

Q4. A 1st order reaction gets 30% decomposed in 40 min. Calculate its t 1/2 .

Q5. The rate law for a reaction is: Rate = k = [A][B] ½ . Can this be an elementary reaction?

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Class 12 Chemistry Case Study Questions PDF Download

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You need to improve your preparation for the Class 12 Chemistry Case Study Questions exams if you want to achieve a 95+% on the boards. You may find case study questions from every chapter that will be covered in the CBSE Class 12 Chemistry Board Exams in this post.

Table of Contents

Case Study-Based Questions for Class 12 Chemistry

Welcome to the world of Class 12 Chemistry Case Study Questions! As a student pursuing Chemistry in the 12th grade, you have already shown dedication and commitment to the subject. However, dealing with case study-based questions can be both intriguing and challenging. In this article, we will explore the nuances of such questions and offer valuable guidance to excel in your exams.

Class 12 Physics Case Study Questions Class 12 Chemistry Case Study Questions Class 12 Biology Case Study Questions Class 12 Maths Case Study Questions

Importance of Class 12 Chemistry Case Study-Based Questions

Class 12 Chemistry case study-based questions play a vital role in your overall understanding of the subject. They enable you to:

• Apply Theoretical Knowledge : Case studies allow you to apply the concepts you have learned in real-life situations, bridging the gap between theory and practical application.
• Develop Analytical Skills : By critically analyzing case scenarios, you enhance your analytical abilities, which are essential in various professional fields.
• Enhance Problem-Solving Abilities : Tackling case study-based questions hones your problem-solving skills, preparing you to face challenges with confidence.
• Gain Deeper Insights : Exploring different case studies exposes you to a wide range of chemical reactions and phenomena, broadening your understanding of Chemistry.

Tips to Excel in Class 12 Chemistry Case Study Questions

• Thoroughly Understand the Concepts: Before attempting case study questions, ensure you have a strong grasp of the underlying concepts and theories.
• Analyze the Scenario Carefully: Take your time to read and comprehend the given case study. Pay attention to every detail to identify the key points.
• Relate to Real-Life Scenarios: Try to connect the case study with real-life situations, as this will make the problem-solving process more intuitive.
• Practice Regularly: Practice a wide variety of case study questions to familiarize yourself with different scenarios and improve your problem-solving skills.
• Collaborate with Peers: Engage in group discussions and brainstorming sessions with your peers. This will provide diverse perspectives and enhance your critical thinking.

Best Books for Class 12 Chemistry

Strictly in accordance with the new term-by-term curriculum for the Class 12 Chemistry Case Study Questions exams to be held in the academic session 2024, including the new board-introduced multiple-choice question types, Stand-Alone MCQs, and MCQs based on Assertion-Reason Case-based MCQs. Included are inquiries from the official CBSE Question Bank that was released in April 2024. What changes have been made to the book: strictly in accordance with the term-by-term syllabus for the board exams that will be held during the 2024 academic year? Chapter- and topic-specific multiple-choice questions based on the unique assessment plan for the Class 12 Chemistry Case Study Questions Board Examination.

Chemistry Syllabus for 2024

Unit II: Solutions (15 Periods)

Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in liquids, solid solutions, Raoult’s law, colligative properties – relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular mass, Van’t Hoff factor.

Unit III: Electrochemistry (18 Periods)

Redox reactions, EMF of a cell, standard electrode potential, Nernst equation and its application to chemical cells, Relation between Gibbs energy change and EMF of a cell, conductance in electrolytic solutions, specific and molar conductivity, variations of conductivity with concentration, Kohlrausch’s Law, electrolysis and law of electrolysis (elementary idea), dry cell-electrolytic cells and Galvanic cells, lead accumulator, fuel cells, corrosion.

Unit IV: Chemical Kinetics (15 Periods)

Rate of a reaction (Average and instantaneous), factors affecting rate of reaction: concentration, temperature, catalyst; order and molecularity of a reaction, rate law and specific rate constant, integrated rate equations and half-life (only for zero and first order reactions), concept of collision theory (elementary idea, no mathematical treatment), activation energy, Arrhenius equation.

Unit VIII: d and f Block Elements (18 Periods)

General introduction, electronic configuration, occurrence and characteristics of transition metals, general trends in properties of the first-row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K 2 Cr 2 O 7  and KMnO 4 .

Lanthanoids –  Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.

Actinoids –  Electronic configuration, oxidation states and comparison with lanthanoids.

Unit IX: Coordination Compounds (18 Periods)

Coordination compounds – Introduction, ligands, coordination number, colour, magnetic properties and shapes, IUPAC nomenclature of mononuclear coordination compounds. Bonding, Werner’s theory, VBT, and CFT; structure and stereoisomerism, the importance of coordination compounds (in qualitative analysis, extraction of metals and biological system).

Unit X: Haloalkanes and Haloarenes (15 Periods)

Haloalkanes:  Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation mechanism of substitution reactions.

Haloarenes:  Nature of C–X bond, substitution reactions (Directive influence of halogen in monosubstituted compounds only). Uses and environmental effects of – dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT.

Unit XI: Alcohols, Phenols and Ethers (14 Periods)

Alcohols:  Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, uses with special reference to methanol and ethanol.

Phenols:  Nomenclature, methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols.

Ethers:  Nomenclature, methods of preparation, physical and chemical properties, uses.

Unit XII: Aldehydes, Ketones and Carboxylic Acids (15 Periods)

Aldehydes and Ketones:  Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, reactivity of alpha hydrogen in aldehydes, uses.

Carboxylic Acids:  Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.

Unit XIII: Amines (14 Periods)

Amines:  Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, identification of primary, secondary and tertiary amines

Diazonium salts:  Preparation, chemical reactions and importance in synthetic organic chemistry.

Unit XIV: Biomolecules (18 Periods)

Carbohydrates –  Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); Importance of carbohydrates.

Proteins –  Elementary idea of – amino acids, peptide bond, polypeptides, proteins, structure of proteins – primary, secondary, tertiary structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes.

Hormones –  Elementary idea excluding structure.

Vitamins –  Classification and functions.

Nucleic Acids:  DNA and RNA.

FAQ on Class 12 Chemistry Case Study Questions

Q: can i rely solely on class 12 chemistry case study based questions exam preparation.

Yes, case study-based questions are an essential part of your preparation. However, it is advisable to supplement them with other study materials and revision of theoretical concepts for comprehensive preparation.

Q: How often should I practice Class 12 Chemistry Case Study Based Questions?

Frequent practice is crucial for mastering case study-based questions. Set aside dedicated practice sessions and gradually increase the difficulty level of the questions.

Q: Can I discuss case study questions with my teachers?

Absolutely! Engaging with your teachers regarding case study questions will provide valuable insights and clarifications.

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The Topper Combo Flashcards

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• General Chemistry
• Homogeneous Catalysis

Chemical Reaction Kinetics: Concepts, Methods and Case Studies

ISBN: 978-1-119-22700-7

Digital Evaluation Copy

Jorge Ancheyta

A practical approach to chemical reaction kinetics—from basic concepts to laboratory methods—featuring numerous real-world examples and case studies

This book focuses on fundamental aspects of reaction kinetics with an emphasis on mathematical methods for analyzing experimental data and interpreting results. It describes basic concepts of reaction kinetics, parameters for measuring the progress of chemical reactions, variables that affect reaction rates, and ideal reactor performance. Mathematical methods for determining reaction kinetic parameters are described in detail with the help of real-world examples and fully-worked step-by-step solutions. Both analytical and numerical solutions are exemplified.    The book begins with an introduction to the basic concepts of stoichiometry, thermodynamics, and chemical kinetics. This is followed by chapters featuring in-depth discussions of reaction kinetics; methods for studying irreversible reactions with one, two and three components; reversible reactions; and complex reactions. In the concluding chapters the author addresses reaction mechanisms, enzymatic reactions, data reconciliation, parameters, and examples of industrial reaction kinetics. Throughout the book industrial case studies are presented with step-by-step solutions, and further problems are provided at the end of each chapter.

• Takes a practical approach to chemical reaction kinetics basic concepts and methods
• Features numerous illustrative case studies based on the author’s extensive experience in the industry
• Provides essential information for chemical and process engineers, catalysis researchers, and professionals involved in developing kinetic models
• Functions as a student textbook on the basic principles of chemical kinetics for homogeneous catalysis
• Describes mathematical methods to determine reaction kinetic parameters with the help of industrial case studies, examples, and step-by-step solutions

Chemical Reaction Kinetics  is a valuable working resource for academic researchers, scientists, engineers, and catalyst manufacturers interested in kinetic modeling, parameter estimation, catalyst evaluation, process development, reactor modeling, and process simulation. It is also an ideal textbook for undergraduate and graduate-level courses in chemical kinetics, homogeneous catalysis, chemical reaction engineering, and petrochemical engineering, biotechnology.

Jorge Ancheyta, is Manager of Products for Transformation of the Crude Oil at the Mexican Petroleum Institute (IMP). He also has been a Professor in the School of Chemical Engineering and Extractive Industries at the National Polytechnic Institute of Mexico (ESIQIE-IPN) since 1992. Dr. Ancheyta works on the development and application of petroleum refining catalysts, kinetic and reactor models, and process technologies mainly in catalytic cracking, catalytic reforming, middle distillate hydrotreating and heavy oils upgrading.

NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12

Important Questions for Class 12 Chemistry Chapter 4 Chemical Kinetics Class 12 Important Questions

December 6, 2019 by Bhagya

Chemical Kinetics Class 12 Important Questions Very Short Answer Type

Question 1. Define ‘rate of a reaction’. (Delhi 2010) Answer: Rate of a reaction: Either, The change in the concentration of any one of the reactants or products per unit time is called rate of a reaction. Or, The rate of a chemical reaction is the change in the molar concentration of the species taking part in a reaction per unit time.

Question 2. Define ‘order of a reaction’. (All India 2011) Answer: The sum of powers of the concentration of the reactants in the rate law expression is called the order of reaction.

Question 3. Define ‘activation energy’ of a reaction. (All India 2011) Answer: The minimum extra amount of energy absorbed by the reactant molecules to form the activated complex is called activation energy. The activation energy of the reaction decreases by the use of catalyst.

Question 5. If the rate constant of a reaction is k = 3 × 10 -4 s -1 , then identify the order of the reaction. (Comptt. All India 2013) Answer: S -1 is the unit for rate constant of first order reaction.

Question 6. Write the unit of rate constant for a zero order reaction. (Comptt. All India 2013) Answer: Mol L -1 S -1 is unit of rate constant for a zero order reaction.

Question 7. Define rate of reaction. (Comptt. Delhi 2016) Answer: The change in concentration of reactant or product per unit time is called rate of reaction.

Question 8. Define rate constant (K). (Comptt. All India 2016) Answer: Rate constant. It is defined as the rate of reaction when the concentration of reaction is taken as unity.

Question 9. For a reaction R → P, half-life (t 1/2 ) is observed to be independent of the initial concentration of reactants. What is the order of reaction? (Delhi 2017) Answer: The t 1/2 of a first order reaction is independent of initial concentration of reactants.

Chemical Kinetics Class 12 Important Questions Short Answer Type -I [SA-I]

Question 10. A reaction is of second order with respect to a reactant. How will the rate of reaction be affected if the concentration of this reactant is (i) doubled, (ii) reduced to half? (Delhi 2009) Answer: Since Rate = K[A] 2 For second order reaction Let [A] = a then Rate = Ka 2 (i) If [A] = 2a then Rate = K (2a) 2 = 4 Ka 2 ∴Rate of reaction becomes 4 times

(ii) If [A] = \(\frac{a}{2}\) then Rate = K \(\left(\frac{a}{2}\right)^{2}=\frac{\mathrm{K} a^{2}}{4}\) ∴ Rate of reaction will be \(\frac{1}{4}^{\text { th }}\) .

Question 11. Define the following : (i) Elementary step in a reaction (ii) Rate of a reaction (All India 2009) Answer: (i) Elementary step in a reaction: Those reactions which take place in one step are called elementary reactions. Example : Reaction between H 2 , and I 2 to form 2HI H 2 + I 2 → 2HI (ii) Rate of a reaction: The change in the concentration of any one of the reactants or products per unit time is called rate of reaction.

Question 12. Define the following : (i) Order of a reaction (ii) Activation energy of a reaction (All India 2009) Answer: (i) Order of a reaction :

• It is the sum of powers of molar concentrations of reacting species in the rate equation of the reaction.
• It may be a whole number, zero, fractional, positive or negative.
• It is experimentally determined.
• It is meant for the reaction and not for its individual steps.

(ii) Activation energy of a reaction: The minimum extra amount of energy absorbed by the reactant molecules to form the activated complex is called activation energy.

Question 13. A reaction is of first order in reactant A and of second order in reactant B. How is the rate of this reaction affected when (i) the concentration of B alone is increased to three times (ii) the concentrations of A as well as B are doubled? (Delhi 2010) Answer: r = K[A] 1 [B] 2 (i) When concentration of B increases to 3 times, the rate of reaction becomes 9 times r = KA(3B) 2 ∴ r = 9KAB 2 = 9 times (ii) r = K(2A) (2B) 2 ∴ r = 8KAB 2 = 8 times

Question 15. Distinguish between ‘rate expression’ and ‘rate constant’ of a reaction. (Delhi 2011) Answer: Rate expression: The expression which expresses the rate of reaction in terms of molar concentrations of the reactants with each term raised to their power, which may or may not be same as the stoichiometric coefficient of that reactant in the balanced chemical equation. Rate constant: The rate of reaction when the molar concentration of each reactant is taken as unity.

Question 16. What do you understand by the rate law and rate constant of a reaction? Identify the order of a reaction if the units of its rate constant are : (i) L -1 mol s -1 (ii) L mol -1 s -1 (All India 2011) Answer: The rate of reaction is found to depend on α concentration of term of reactant A and β concentration term of reactant B Then Rate of reaction ∝ [A] α [B] β or Rate = K [A] α [B] β This expression is called Rate law. ‘K’ in this expression is called Rate constant. Rate constant’s unit : (i) Unit = L -1 mol s -1 → Zero order reaction (ii) Unit = L mol -1 s -1 → Second order reaction.

Question 18. A reaction is of second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is reduced to half? What is the unit of rate constant for such a reaction? (All India 2011) Answer: Rate = K [A] 2 = Ka 2 If [A] = \(\frac{1}{2}\)a Rate = K \(\left(\frac{a}{2}\right)^{2}=\frac{1}{4}\) Ka 2 ∴ Rate = 1/4 th (one fourth of origina rate) The unit of rate constant is L mol -1 s -1

Question 19. What do you understand by the ‘order of a reaction’? Identify the reaction order from each of the following units of reaction rate constant: (i) L -1 mol s -1 (ii) L mol -1 s -1 (Delhi 2012) Answer: Order of reaction: The sum of powers of the concentration of the reactants in the rate law expression is called the order of that chemical reaction. r = K[A] x [B] y Order = x + y (i) Zero order (ii) Second order

Question 25. Write two differences between ‘order of reaction’ and ‘molecularity of reaction’. (Delhi 2014) Answer:

Question 26. Define the following terms : (a) Pseudo first order reaction. (b) Half life period of reaction (t 1/2 ). (Delhi 2014) Answer: (a) Those reactions which are not truly of the first order but under certain conditions become first order reactions are called pseudo first order reaction. (b) The time taken for half of the reaction to complete is called half life period.

Question 27. Explain the following terms : (i) Rate constant (k) (ii) Half life period of a reaction (t 1/2 ) (Delhi 2014) Answer: (i) Rate constant (k): It is a proportionality constant and is equal to the rate of reaction when the molar concentration of each of the reactants is unity. (ii) Half life period of a reaction (t 1/2 ): The time taken for half of the reaction to complete is called half life penod.(R)t

Question 29. (a) For a reaction, A + B → Product, the rate law is given by, Rate = k[A] 1 [B] 2 . What is the order of the reaction? (b) Write the unit of rate constant ‘k’ for the first order reaction. (Comptt. Delhi 2014) Answer: (a) For a reaction, A + B Rate = k [A] 1 [B] 2 This is the third order of reaction. (b) Unit of rate constant for first order reaction is S -1

Question 30. Define the following terms : (i) Rate constant (k) (ii) Activation energy (E a ) (Comptt. Delhi 2014) Answer: (i) Rate constant (k): It is a proportionality constant and is equal to the rate of reaction when the molar concentration of each of the reactants is unity. (ii) Activation energy (E a ): The minimum extra amount of energy absorbed by the reactant molecules to form the activated complex is called activation energy.

Question 31. How does a change in temperature affect the rate, of a reaction? How can this effect on the rate constant of a reaction be represented quantitatively? (Comptt. All India 2014) Answer: The rate constant of a reaction increases with increase of temperature and becomes nearly double for every 10° rise in temperature. The effect can be represented quantitatively by Arhenius equation K = Ae -Ea/RT Where [Ea = Activation energy of the reaction; A = Frequency factor]

Question 32. Define each of the following : (i) Specific rate of a reaction (ii) Energy of activation of a reaction (Comptt. All India 2014) Answer: (i) Specific rate of a reaction: Specific rate of reaction is the rate of reaction when the molar concentration of each of the reactants is unity. (ii) Activation energy of a reaction: The minimum extra amount of energy absorbed by the reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

Question 33. A reaction is of second order with respect to its reactant. How will its reaction rate be affected if the concentration of the reactant is (i) doubled (ii) reduced to half? (Comptt. All India 2014) Answer: Since Rate = K[A] 2 For second order reaction Let [A] = a then Rate = Ka 2 (i) If [A] = 2a then Rate = K (2a) 2 = 4 Ka 2 ∴Rate of reaction becomes 4 times (ii) If [A] = \(\frac{a}{2}\) then Rate = K \(\left(\frac{a}{2}\right)^{2}=\frac{\mathrm{K} a^{2}}{4}\) ∴ Rate of reaction will be \(\frac{1}{4}^{\text { th }}\) .

Question 34. Define the following terms : (i) Half-life of a reaction (t 1/2 ) (ii) Rate constant (k) (Comptt. Delhi 2015) Answer: (i) Half-life of a reaction (t 1/2 ): Half-life period (t 1/2 ) is the time in which half of the substance has reacted and its concentration is reduced to one-half of its initial concentration. (ii) Rate constant (k): Rate constant may be defined as the rate of reaction when the molar concentration of each reactant is taken as unity.

Question 35. Write units of rate constants for zero order and for the second order reactions if the concentration is expressed in mol L -1 and time in second. (Comptt. All India 2015) Answer: Using formula of rate constant, K = [mol L -1 ] 1 – n s -1 (n = order of rx n ) Unit for zero order reaction, K = [mol L -1 ] 1 – 0 s -1 K = [mol L -1 ] s -1 = mol L -1 s -1 Unit for second order reaction, K = [mol L -1 ] 1 – 2 = [mol L -1 ] -1 s -1

Question 36. For a reaction: 2NH 2 (g) \(\stackrel{\mathrm{Pt}}{\longrightarrow}\) N 2 (g) + 3H 2 (g) Rate = k (i) Write the order and molecularity of this reaction. (ii) Write the unit of k. (Delhi 2016) Answer: 2NH 2 (g) \(\stackrel{\mathrm{Pt}}{\longrightarrow}\) N 2 (g) + 3H 2 (g) (i) It is a zero order reaction and its molecularity is two. (ii) Unit of k is mol L -1 s -1 .

Question 37. For a reaction: H 2 + Cl 2 \(\stackrel{\mathrm{hv}}{\longrightarrow}\) 2HCl Rate = k (i) Write the order and molecularity of this reaction. (ii) Write the unit of k. (All India 2016) Answer: H 2 + Cl 2 \(\stackrel{\mathrm{hv}}{\longrightarrow}\) 2HCl This reaction is zero order reaction and molecularity is two. (ii) Unit of k = mol L -1 s -1

Question 39. (a) Explain why H 2 and O 2 do not react at room temperature. (b) Write the rate equation for the reaction A 2 + 3B 2 → 2C, if the overall order of the reaction is zero. (Comptt. All India 2017) Answer: (i) H 2 and O 2 do not react at room temperature because they do not have enough activation energy to overcome the exceptionally high activation energy barrier. (ii) A 2 + 3B 2 → 2C Rate = \(\left(\frac{d x}{d t}\right)\) = K[A] 0 [B] 0 = K (rate constant)

Question 41. (i) What is the order of the reaction whose rate constant has same units as the rate of reaction? (ii) For a reaction A + H 2 O → B; Rate ∝ [A], What is the order of this reaction? (Comptt. All India 2017) Answer: (i) The reaction whose rate constant has same units as the rate of reaction, will have zero order of reaction. (ii) The reaction A + H 2 O → B Rate ∝ [A] The order of this reaction will be pseudo first order reaction as the rate of reaction depends only on concentration of A only.

Chemical Kinetics Class 12 Important Questions Short Answer Type – II [SA-II]

Question 44. Nitrogen pentoxide decomposes according to equation : 2N 2 O 5 (g) → 4 NO 2 (g) + O 2 (g). This first order reaction was allowed to proceed at 40°C and the data below were collected :

Question 45. For the reaction 2NO(g) + Cl 2 (g) → 2NOCl(g) the following data were collected. All the measurements were taken at 263 K :

(a) Write the expression for rate law. (b) Calculate the value of rate constant and specify its units. (c) What is the initial rate of disappearance of Cl 2 in exp. 4? (Delhi 2012) Answer: (a) Rate law = K[NO] 2 [Cl 2 ] (b) 0.60 M min -1 = K[0.15] 2 [0.15] M 3 ∴ K = 177.7 M -2 min -1 (c) Initial rate of disappearance of Cl 2 in exp. 4 Formula : Rate = K[NO] 2 [Cl 2 ] ∴ Initial rate = 177.7M -2 min -1 × (0.25) 2 × (0.25)M 3 = 2.8 M min -1

Question 46. (a) A reaction is first order in A and second order in B. (i) Write differential rate equation. (ii) How is rate affected when concentration of B is tripled? (iii) How is rate affected when concentration of both A and B is doubled? (b) What is molecularity of a reaction? (Comptt. All India 2009) Answer: (a) (i) Differential rate equation : \(\frac{d x}{d t}\) = rate = K [A] 1 [B] 2 (ii) Rate, r 1 = K [A] 1 [B] 2 …………… (i) When concentration of B is increased three times then Rate, r 2 = K [A] 1 [3B] 2 ………..(ii) Dividing equation (ii) by (i) we get r 2 = 9r 1 rate increases by n*ne times. (iii) When concentration of both A and B are doubled, then r 3 = K [2A] 1 [2B] 2 ………….. (iii) Dividing equation {Hi) by (t), we get r 3 = 8r 1 Hence rate increases by eight times.

(b) The number of reacting species (atoms, ions or molecules) taking part in an elementary reaction is called Molecularity of a reaction.

Question 48. The following data were obtained during the first order thermal decomposition of SO 2 Cl 2 at a constant volume : SO 2 Cl 2 (g) → SO 2 (g) + Cl 2 (g)

Question 57. Following data are obtained for the reaction: N 2 O 5 → 2NO 2 + \(\frac{1}{2}\)O 2

Question 59. The following data were obtained during the first order thermal decomposition of SO 2 Cl 2 at a constant volume :

Question 60. For the first order decomposition of azoisopropane to hexane and nitrogen at 543 K , the following data were obtained : Calculate the rate constant. The equation for the reaction is :

(CH 3 ) 2 CHN = NCH(CH 3 ) 2 C 6 H 14 (g) + N 2 (g) [Given : log 3 = 0.4771; log 5 = 0.6990] (Comptt. Delhi 2016) Answer: (CH 3 ) 2 CHN = NCH(CH 3 ) 2  → N 2 + C 6 H 14

Chemical Kinetics Class 12 Important Questions Long Answer Type (LA)

Question 63. (a) Explain the following terms : (i) Rate of a reaction (ii) Activation energy of a reaction (b) The decomposition of phosphine, PH 3 , proceeds according to the following equation: 4 PH 3 (g) → P 4 (g) + 6 H 2 (g) It is found that the reaction follows the following rate equation : Rate = K [PH 3 ]. The half-life of PH 3 is 37.9 s at 120° C. (i) How much time is required for 3/4th of PH 3 to decompose? (it) What fraction of the original sample of PH 3 remains behind after 1 minute? (All India 2010) Answer: (a) (i) Rate of a reaction: The change in the concentration of any one of the reactants or products per unit time is called rate of reaction. (ii) The minimum extra amount of energy absorbed by the reactant molecules to form the activated complex is called activation energy. The activation energy of the reaction decreases by the use of catalyst.

Question 64. (a) Explain the following terms : (i) Order of a reaction (ii) Molecularity of a reaction (b) The rate of a reaction increases four times when the temperature changes from 300 K to 320 K. Calculate the energy of activation of the reaction, assuming that it does not change with temperature. (R = 8.314 J K -1 mol -1 ) (All India 2016) Answer: (a) (i) Order of a reaction: It is the sum of powers of the molar concentrations of reacting species in the rate equation of the reaction. (ii) Molecularity of a reaction :

• It is the total number of reacting species (molecules, atoms or ions) which bring the chemical change.
• It is always a whole number.
• It is a theoretical concept.
• It is meaningful only for simple reactions or individual steps of a complex reaction. It is meaningless for overall complex reaction.

Question 67. (a) A reaction is second order in A and first order in B. (i) Write the differential rate equation, (ii) How is the rate affected on increasing the concentration of A three times? (iii) How is the rate affected when the concentrations of both A and B are doubled? (b) A first order reaction takes 40 minutes for 30% decomposition. Calculate t 1/2 for this reaction. (Given log 1.428 = 0.1548) (Delhi 2013) Answer: (a) (i) Differential rate equation : \(\frac{d x}{d t}\) = K [A] 2 [B] (ii) When concentration of A is increased to three times, the rate of reaction becomes 9 times r = K[3A] 2 B ∴ r = 9KA 2 B i.e. = 9 times (iii) r = K[2A] 2 [2B] ∴ r = 8KA 2 B i.e. = 8 times

(b) (i) t 1/2 = \(\frac{0.693}{\mathrm{K}}\) (For first order reaction) t 3/4 = K ⇒ t 3/4 = \(\frac{1.3864}{\mathrm{K}}\) According to condition (The value 1.3864 is double of 0.693) From the above equation it is clear that t 3/4 = 2t 1/2 ∴ y = 2X (ii) It is due to improper orientation of the colliding molecules at the time of collision.

Question 71. For the hydrolysis of methyl acetate in aqueous solution, the following results were obtained :

Question 72. (a) For a reaction A + B → P, the rate is given by Rate = k[A] [B] 2 (i) How is the rate of reaction affected if the concentration of B is doubled? (ii) What is the overall order of reaction if A is present in large excess? (b) A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction. (log 2 = 0.3010) (Delhi 2015) Answer: (a) For the reaction A + B → P rate is given by Rate = k[A] 1 [B] 2 (i) r 1 = k[A]1 [B]2 r 2 = k[ A] 1 [2B] 2 = r 2 = k[A] 1 [2B] 2 =4k[A] 1 [B] 2 r 1 = 4r 2 , rate will increase four times of actual rate.

Question 73. For the hydrolysis of methyl acetate in aqueous solution, the following results were obtained:

Question 74. (a) For a reaction A + B → P, the rate is given by Rate = k[A] [B] 2 (i) How is the rate of reaction affected if the concentration of B is doubled? (ii) What is the overall order of reaction if A is present in large excess? (b) A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction. (All India 2015) Answer: (a) For the reaction A + B → P rate is given by Rate = k[A] 1 [B] 2 (i) r 1 = k[A] 1 [B] 2 r 2 = k[A] 1 [2B] 2 = 4k[A] 1 [B] 2 r 1 = 4r 2 (rate of reaction becomes 4 times)

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Class 12th Chemsitry - Chemical Kinetics Case Study Questions and Answers 2022 - 2023

By QB365 on 08 Sep, 2022

QB365 provides a detailed and simple solution for every Possible Case Study Questions in Class 12 Chemsitry Subject - Chemical Kinetics, CBSE. It will help Students to get more practice questions, Students can Practice these question papers in addition to score best marks.

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Chemical kinetics case study questions with answer key.

12th Standard CBSE

Final Semester - June 2015

(ii) Find the-value of the equilibrium constant

(iii) The initial rate of conversion of A will be

(iv) For the reaction,  if  \(\frac{d[B]}{d t}=2 \times 10^{-4}\)  , value of  \(-\frac{d[A]}{d t}\)  will be

Read the passage given below and answer the following questions: For the reaction:  \(2 \mathrm{NO}_{(g)}+\mathrm{Cl}_{2(g)} \rightarrow 2 \mathrm{NOCl}_{(g)}\) ,  the following data were collected. All the measurements were taken at 263 K.

The following questions are multiple choice questions. Choose the most appropriate answer: (i) The molecularity of the reaction is 

(ii) The expression for rate law is

(iii) The overall order of the reaction is

(iv) The value of rate constant is

Read the passage given below and answer the following questions: A reaction is said to be of the first order if the rate of the reaction depends upon one concentration term only. For a first order reaction of the type A \(\rightarrow\)  Products, the rate of the reaction is given as : rate = k[A]. The differential rate law is given as  \(\frac{d A}{d t}=-k[A]\)  .The integrated rate law : In  \(\frac{[A]}{[A]_{0}}=-k t\)  where [A] is the concentration of reactant left at time t and [A] o is the initial concentration of the reactant, k is the rate constant. The following questions are multiple choice questions. Choose the most appropriate answer : (i) The unit of rate constant for a first order reaction is

(ii) Half-life period of a first order reaction is 10 min. Starting with initial concentration 12 M, the rate after 20 min is

(iii) For a first order reaction, (A) \(\rightarrow\) products, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M, is

(iv) The half-life period of a 1 st  order reaction is 60 minutes. What percentage will be left over after 240 minutes?

Read the passage given below and answer the following questions : Number of molecules which must collide simultaneously to give product is called molecularity. It is equal to sum of coefficients of reactants present in stoichiometric chemical equation. For reaction, \(m_{1} A+m_{2} B \rightarrow \text { Product }\)   Molecularity = [m 1 + m 2 ] In complex reaction each step has its own molecularity which is equal to the sum of coefficients of reactants present in a particular step. Molecularity is a theoretical property. Its value is any whole number. Number of concentration terms on which rate of reaction depends is called order of reaction or sum of powers of concentration terms present in the rate equation is called order of reaction. If rate equation of reaction is : Rate =  \(k \cdot C_{A}^{m_{1}} \cdot C_{B}^{m_{2}}\)   Then order of reaction = m 1 + m 2 In simple reaction, order and molecularity are same. In complex reaction, order of slowest step is the order of over all reaction. This step is known as rate determining step. Order is an experimental property. Its value may be zero, fractional or negative. The following questions are multiple choice questions. Choose the most appropriate answer: (i) Higher order (> 3) reactions are rare due to

​​​​​​(ii) The molecularity of the reaction: \(6 \mathrm{FeSO}_{4}+3 \mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{KClO}_{3} \rightarrow \mathrm{KCl}+3 \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}+3 \mathrm{H}_{2} \mathrm{O} \text { is }\)

(iii) Which of the following statements is false in the following?

(iv) The rate of the reaction  \(A+B+C \rightarrow \text { products }\)  , is given by  \(r=-\frac{d[A]}{d t}=k[A]^{1 / 2}[B]^{1 / 3}[C]^{1 / 4}\)  ,The order of the reaction is

Read the passage given below and answer the following questions : In a reaction, the rates of disappearance of different reactants or rates of formation of different products may not be equal but rate of reaction at any instant of time has the same value expressed in terms of any reactant or product. Further, the rate of reaction may not depend upon the stoichiometric coefficients of the balanced chemical equation. The exact powers of molar concentrations of reactants on which rate depends are found experimentally and expressed in terms of 'order of reaction'. Each reaction has a characteristic rate constant depends upon temperature. The units of the rate constant depend upon the order of reaction. The following questions are multiple choice questions. Choose the most appropriate answer : (i) The rate constant of a reaction is found to be 3 x 10 -3 mol -2 L 2 sec -1 .The order of the reaction is

(ii) In the reaction  \(A+3 B \rightarrow 2 C\)  ,the rate of formation of C is

(iii) Rate of a reaction can be expressed by following rate expression, Rate = k[A] 2 [B], if concentration of A is increased by 3 times and concentration of B is increased by 2 times, how many times rate of reaction increases?

(iv) The rate of a certain reaction is given by,rate = k[H + ] n . The rate increases 100 times when the pH changes from 3 to 1. The order (n) of the reaction is

(ii) The rate constant for a first order reaction is 7.0x 10 -4  s -1 . If initial concentration of reactant is 0.080 M, what is the half life of reaction?

(iii) For the half-life period of a first order reaction, which one of the following statements is generally false?

(iv) The rate of a first order reaction is 0.04 mol L -1  s -1 at 10 minutes and 0.03 mol L -1 s -1  at 20 minutes after initiation. The half-life of the reaction is

Read the passage given below and answer the following questions : The following reaction, \(A_{(g)} \stackrel{\Delta}{\longrightarrow} P_{(g)}+Q_{(g)}+R_{(g)}\)   follows first order kinetics. The half-life period of this reaction is 69.3 s at 500°C. The gas A is enclosed in a container at 500°C and at a pressure of 0.4 atm The following questions are multiple choice questions. Choose the most appropriate answer: (i) The rat constant for the reaction is

(ii) The total pressure of the system after 230 s will be

(iii) The plot of ln[A] vs t will be

(iv) Which of the following is not an example of first order reaction?

Read the passage given below and answer the following questions: A reaction in which rate of reaction is independent of concentration of the reactants is called zero order reaction. Photochemical combination of hydrogen and chlorine to give hydrogen chloride is an example of zero order reaction. The rate constant of a zero order reaction is equal to the rate of reaction. The half life period of a zero order reaction is directly proportional to initial concentration of the reactant. For a zero order reaction,  \(k=\frac{1}{t}\left\{[A]_{0}-[A]\right\}\)   In these questions (i-iv), a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

(i) Assertion : For a zero order reaction, plot of rate vs concentration will be a straight line parallel to concentration axis. Reason : For a zero order reaction, rate is independent of concentration. (ii) Assertion : Photochemical combination of hydrogen and chlorine to give hydrogen chloride is an example of zero order reaction. Reason : The rate of reaction depends on the concentration of hydrogen and independent of concentration of chlorine. (iii) Assertion : If in a zero order reaction, the concentration of the reactant is doubled, the half-life period is also doubled. Reason : For a zero order reaction, the rate of reaction is independent of initial concentration (iv) Assertion : In a reaction A -7 products, the concentration of the reactant is reduced to zero after a finite time. Reason : The order of reaction is zero.

Read the passage given below and answer the following questions : Decrease in concentration of reactant or increase in concentration of product per unit time is called rate of reaction. It is of two types: (i) Instantaneous rate of reaction : Rate of change of concentration of reactant or product at a particular time is called instantaneous rate of reaction. \(r_{\text {inst. }}=\frac{d C}{d t}\)   where, dC = infinitely small change in concentration dt = infinitely small change in time. (ii) Average rate of reaction: Ratio of change in concentration and time required for the change is average rate of reaction. \(r_{a v}=\frac{\Delta x}{\Delta t}=\frac{\text { Change in concentration }}{\text { Time required for the change }}\)   For a reaction of the type,  \(m_{1} A+m_{2} B \rightarrow n_{1} C+n_{2} D\)   Rate of reaction is given as \(-\frac{1}{m_{1}} \frac{d[A]}{d t}=-\frac{1}{m_{2}} \frac{d[B]}{d t}=+\frac{1}{n_{1}} \frac{d[C]}{d t}=+\frac{1}{n_{2}} \frac{d[D]}{d t}\)   In these questions (i-iv), a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.

(i) Assertion : The kinetics of the reaction, \(m A+n B+p C \rightarrow m^{\prime} X+n^{\prime} Y+p^{\prime} Z\)  obey the rate expression as  \(\frac{d x}{d t}=k[A]^{m}[B]^{n}\)  . Reason : The rate of the reaction does not depend upon the concentration of C. (ii) Assertion: Instantaneous rate of reaction is equal to dx/ dt. Reason : It is the rate of reaction at any particular instant of time. (iii) Assertion : For the reaction, \(R \mathrm{Cl}+\mathrm{NaOH} \rightarrow \mathrm{ROH}+\mathrm{NaCl}\)  the rate of reaction is reduced to half on reducing the concentration of RCl to half. Reason : The sate of reaction is represented by k[RCl]. (iv) Assertion : In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients. Reason: It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.

Read the passage given below and answer the following questions : For a first order reaction  \(A \rightarrow \text { Products, } k=\frac{2.303}{t} \log \frac{a}{a-x}\)  were a is the initial concentration of A and (a-x) is the concentration of A after time t. k is rate constant. Its value is constant at constant temperature for a reaction. The time in which half of the reactant is consumed is called half-life period. Half-life period of a first order reaction is constant. Its value is independent of initial concentration or any other external conditions. In these questions (i-iv), a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices. (i) Assertion : Rate of reaction doubles when concentration of reactant is doubled if it is a first order reaction. Reason : Rate constant also doubles,

(ii) Assertion : Hydrolysis of ethyl acetate in presence of acid is a reaction of first order whereas in presence of alkali, it is a reaction of second order. Reason : Acid only acts as a catalyst whereas alkali acts as one of the reactants.

(iii) Assertion : For a first -order reaction, the concentration of the reactant decreases exponentially with time. Reason : Rate of reaction at any time depends upon the concentration of the reactant at that time.

(iv) Assertion : Half-life period for a first order reaction is independent of initial concentration of the reactant. Reason : For a first order reaction,  \(t_{1 / 2}=\frac{0.693}{k}\) , where k is rate constant.

Chemical kinetics deals with rate of chemical reactions, how fast reactants get used up or how fast products are formed in the reaction. Differed chemical reactions have different speed. Rate of reaction depends upon concentration of reactants, temperature, pressure especially in gaseous reactions and presence of catalyst. Chemical reaction takes place as a results of collision between reacting molecules. The rate of reaction does not depend upon total number of coUisions rather it depends upon number of effective coUisions. In a redox reaction, if \(\mathbf{E}_{\text {cell }}^{\circ} \text { is }+\mathbf{v e}, \Delta \mathbf{G}^{\circ}\)  will be -ve and 'K' equilibrium constant will be high i.e. products formed will be more than the reactants. (a) k (The rate constant), (Activation Energy) Ea and 'A' (Arrhenius constant) are 3 x 10 -4 s -1 , 104.4 k.J mol -1 and 6.0 x 10 14 S -1  respectively. What is value of 'k' when T  \(\mathbf{T} \rightarrow \infty ?\) (b) What is meant by activation energy? (c) What does e Ea/RT represent? (d) If Fe 3 + + 2I -  \(\rightarrow\)  Fe2 + + I 2 has E o = 0.24V, what is the value of log K? What does value of 'K' indicate? (e) What type of molecules undergo effective collisions?

Observe the table given' showing volume of CO 2 obtained by reaction of CaCO 3 and dilute HCI after every minute. Answer the questions that follow: Table showing volume of CO 2 at one minute interval by reaction of CaCO 3 with dilute HCI.

(a) What happens to rate of reaction with time? (b) Why does CaCO 3 powder react faster than marble chips? (c) What happens to rate of reaction if concentrated HCI is used? d) In manufacture of NH 3 , \(\mathbf{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) 2 \rightleftharpoons \mathrm{NH}_{3}+\text { heat }\) what is effect of pressure on rate of reaction? (e) Why does rate of reaction becomes almost double for energy 10° rise in temperature?

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Chemical kinetics case study questions with answer key answer keys.

(i) (b) : According to the figure, in the given time of 4 hours (1 to 5) concentration of A falls from 0.5 to 0.3 M, while in the same time concentration of B increases from 0.2 to 0.6 M. Decrease in concentration of A in 4 hours = 0.5 - 0.3 = 0.2 M Increase in concentration of B in 4 hours = 0.6 - 0.2 = 0.4 M Thus, increase in concentration of B in a given time is twice the decrease in concentration of A. Thus, n = 2 (ii) (b) :  \(K=\frac{[B]^{2}}{[A]}=\frac{(0.6)^{2}}{0.3}=1.2 \mathrm{M}\)   (iii) (a) : From t = 0 to t = 1 hr, For A, dx = 0.6 - 0.5 = 0.1 mol L -1 \(\therefore\)  Initial rate of conversion of  \(A=\frac{d x}{d t}\)   \(=\frac{0.1 \mathrm{~mol} \mathrm{~L}^{-1}}{1 \mathrm{hr}}=0.1 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{hr}^{-1}\)   (iv) (b) :   \(A \rightleftharpoons 2 B\)   \(-\frac{d[A]}{d t}=+\frac{1}{2} \frac{d[B]}{d t}=\frac{1}{2} \times 2 \times 10^{-4}=10^{-4}\)  

(i) (c) :   \(2 \mathrm{NO}_{(g)}+\mathrm{Cl}_{2(g)} \rightarrow 2 \mathrm{NOCl}_{(g)}\)   Molecularity = 3 (ii) (b) : Let rate of this reaction, r = k[NO] m [CI 2 ] n   then  \(\frac{r_{1}}{r_{2}}=\frac{0.60}{1.20}=\frac{k(0.15)^{m}(0.15)^{n}}{k(0.15)^{m}(0.30)^{n}}\)   or  \(\frac{1}{2}=\left(\frac{1}{2}\right)^{n} \Rightarrow n=1\)   Again from  \(\frac{r_{2}}{r_{3}}=\frac{1.20}{2.40}=\frac{k(0.15)^{m}(0.30)^{n}}{k(0.30)^{m}(0.15)^{n}}\)   or  \(\frac{1}{2}=\left(\frac{1}{2}\right)^{m} \cdot \frac{2}{1} \text { or } \frac{1}{4}=\left(\frac{1}{2}\right)^{m} \Rightarrow m=2\)   Hence, expression for rate law is r = k[NO]  2 [Cl 2 ] 1 (iii) (d) : As the order W.r.t. NO is 2 and order W.r.t. Cl 2 is 1, hence the overall order is 3. (iv) (c) : Substituting the values of experiment 1 in rate law expression 0.60 M min -1 = k(0.15 M) 2 (0.15 M) 1 or  \(k=\frac{0.60 \mathrm{Mmin}^{-1}}{0.0225 \times 0.15 \mathrm{M}^{3}}=177.77 \mathrm{M}^{-2} \mathrm{~min}^{-1}\)    

(i) (a) : Unit of rate constant for a reaction of n th order = (conc.)1 -n time -1 For a first order reaction, n = 1 Unit of rate constant = (mol L -1 ) 1 - 1  s -1 = s -1 (ii) (d) :   \(\underset{\text { Initial conc. }}{12 \mathrm{M} \stackrel{t_{1 / 2}}{\longrightarrow}} 6 \mathrm{M} \stackrel{t_{1 / 2}}{\longrightarrow} 3 \mathrm{M}\)   t 1/2 = 10 min  \(k=\frac{0.693}{10}=0.0693 \mathrm{~min}^{-1}\)   As t 1/2 is 10 min, after 20 minutes the concentration will be 3 M. Hence, Rate = 0.0693 x 3 M min -1 (iii) (a) : For the first order reaction, \(k=\frac{2.303}{t} \log \frac{a}{a-x}\)   a = 0.1 M, a - x = 0.025 M, t = 40 min \(k=\frac{2.303}{40} \log \frac{0.1}{0.025}=\frac{2.303}{40} \log 4=0.0347 \mathrm{~min}^{-1}\)   \([A] \rightarrow \text { product }\)   Thus, rate = k[A] rate = 0.0347 x 0.01 M min -1 = 3.47 x 10 -4 M min -1 (iv) (a) :   \(t_{1 / 2}=\frac{0.693}{k} \Rightarrow \frac{0.693}{t_{1 / 2}}=k \Rightarrow \frac{0.693}{60}=k\)   k = 0.01155 min -1 \(k=\frac{2.303}{t} \log \left(\frac{a}{a-x}\right)\)   Let the initial amount (a) be 100 \(0.01155 \mathrm{~min}^{-1}=\frac{2.303}{240 \mathrm{~min}} \log \left(\frac{100}{a-x}\right)\)   1.204 = log100 - log(a-x) 1.204 = 2 - log(a-x) log (a - x) = 2 - 1.204 = 0.796 (a - x) = 6.25%

(i) (c) : The reactions of higher order are very rare because of the less chances of the molecules to come together simultaneously and collide. (ii) (c) : The total number of reactant molecules participating in a chemical reaction is known as its rnolecularity, hence the molecularity = 6 + 3 + 1 = 10. (iii) (c) : Molecularity mayor may not be equal to the order of a reaction. (iv) (d) : Order of reaction  \(=\frac{1}{2}+\frac{1}{3}+\frac{1}{4}=\frac{6+4+3}{12}=\frac{13}{12}\)

(i) (c) : Unit of k for nth order = (mol L -1 ) 1-n  sec -1 . Here,k = 3 x 10 -3 mol -2 L 2 sec -1  ...(i) Unit of  \(k=m o l^{-2} L^{2} \sec ^{-1} \Rightarrow\left(m o l L^{-1}\right)^{-2} \sec ^{-1}\)   ...(ii) Comparing (i) and (ii) we get,  \(1-n=-2 \Rightarrow n=3\)   (ii) (c) :   \(\text { Rate }=-\frac{d[A]}{d t}=-\frac{1}{3} \frac{d[B]}{d t}=\frac{1}{2} \frac{d[C]}{d t}\)   (iii) (c) : Given R 1 = k[A] 2  [B] According to question R 2 = k[3A] 2  [2B] = k x 9 [A] 2  x 2 [B] = 18 x k [A] 2  [B] = 18 R 1 (iv) (c) : Rate (r) = k[H+] n When pH = 3 ; [H + ] = 10 -3  and when pH = 1 ; [H + ] = 10 -1 . \(\therefore \quad \frac{r_{1}}{r_{2}}=\frac{k\left(10^{-3}\right)^{n}}{k\left(10^{-1}\right)^{n}} \Rightarrow \frac{1}{100}=\left(\frac{10^{-3}}{10^{-1}}\right)^{n}\left(\because r_{2}=100 r_{1}\right)\)   \(\Rightarrow \quad\left(10^{-2}\right)^{1}=\left(10^{-2}\right)^{n} \Rightarrow n=1\)

(i) (c) : For a first order reaction : \(t_{1 / 2}=\frac{0.693}{k}, k=3.01 \times 10^{-3} \mathrm{~s}^{-1}\)   \(\therefore \quad t_{1 / 2}=\frac{0.693}{3.01 \times 10^{-3}}=230.3 \mathrm{~s}\)   (ii) (a) : Half life (1/2) of a first order reaction is given as : \(t_{1 / 2}=\frac{0.693}{k}=\frac{0.693}{7.0 \times 10^{-4}}=990 \mathrm{~s}\)   (iii) (b) : For a first order reaction  \(t_{1 / 2}=\frac{0.693}{k}\)  therefore t 1/2 depends upon k and hence depends on temperature because rate constant k is a function of temperature. (iv) (c) : Let the concentrations of the reactant after  10 min and 20 min be C 1  and C 2 respectively. Rate after 10 min = k,C 2 = 0.03 x 60 mol L -1  min -1 \(\therefore \frac{C_{1}}{C_{2}}=\frac{4}{3}\)   Let the reaction starts after 10 minutes. \(k=\frac{2.303}{10} \log \frac{C_{1}}{C_{2}}=\frac{2.303}{10} \log \frac{4}{3}=0.02878\)   \(\therefore \quad t_{1 / 2}=\frac{0.6932}{k}=\frac{0.6932}{0.02878}=24.086 \mathrm{~min}\)

(i) (c) : t 1/2 = 69.3 s For first order reaction, \(k=\frac{0.693}{t_{1 / 2}}=\frac{0.693}{69.3}=0.01 \mathrm{~s}^{-1}\)   (ii) (b) : For the given reaction, \(\begin{array}{lccc} & A_{(g)} \stackrel{\Delta}{\longrightarrow} P_{(g)} & +Q_{(g)}+R_{(g)} \\ \text { Initial pressure } & 0.4 & 0 & 0 & 0 \\ \text { Final pressure } & 0.4-0.36 & 0.36 & 0.36 & 0.36 \end{array}\)   Total pressure = (0.4 - 0.36) + (3 x 0.36) = 1.12 atm (iii) (b) : Expression that relates concentration of reactant and time for first order reaction is In [A]= -kt +In [A] o So, the plot of ln [A] 0 vs t will be linear with slope = -k and intercept = In [A] 0 (iv) (c) : Decomposition of ammonia on a hot platinum surface at high pressure is a zero order reaction.

(i) (a) :  Rate expression  \(\frac{d x}{d t}=k[A]^{m}[B]^{n}\)   shows that the total order of reactions is m + n + 0 = m + n, as the rate of reaction is independent of concentration of C, i.e., the order with respect to C is zero. This is the reason that C does not figure in the rate expression. (ii) (b) : Instantaneous rate of a reaction is equal to small change in concentration (dx) during a small interval of time (dt) at that particular instant of time divided by the time interval. (iii) (a) : For the given reaction, rate of reaction (r) = k[RCl] (where k is rate constant). Therefore if the concentration of [RCl] is reduced to half, then new rate  \(\left(r^{\prime}\right)=\frac{k}{2}[R \mathrm{Cl}]\)   (iv) (a)

(i) (c) :  For first order .reaction, Rate. = k[A 1 ] According to question, [A 2 ] = [2A 1 ] \(\therefore\)  Rate 2 = k[2A 1 ] \(\Rightarrow \)   Rate 2 , = 2 Rate 1 .  For a given reaction, rate constant is constant and independent of the concentration of reactant. (ii) (a) :   \(\begin{aligned} \mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+\mathrm{H}_{2} \mathrm{O} \stackrel{\mathrm{H}^{+}}{\longrightarrow} \mathrm{CH}_{3} \mathrm{COOH} &+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} \end{aligned}\)   \(\text { Rate } \propto\left[\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}\right]\)   \(\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+\mathrm{NaOH} \rightarrow \mathrm{CH}_{3} \mathrm{COONa}+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\)   \(\text { Rate } \propto\left[\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}\right][\mathrm{NaOH}]\)   (iii) (b) : For a first order reaction,  \(\lfloor A]=[A]_{0} e^{-k t}\)   or  \(\log [A]=-\frac{k t}{2.303}+\log [A]_{0}\)   (iv) (a) : For a first order reaction, t 1/2 is inversely proportional to k, it does not depend on the initial concentration of the reactant.

(a) Arrhenius constant k = Ae -Ea/RT \(\Rightarrow k=\mathrm{Ae}^{-\mathrm{Ea} / \infty}=\mathrm{Ae}^{\circ}=\mathrm{A}=6.0 \times 10^{14} \mathrm{~s}^{-1}\) (b) The extra energy which must be supplied to reactants in order to undergo effective collision to form products. (c) It represents fraction of molecules possessing activation energy (Ea) or more than Ea. (d)  \(\log \mathrm{K}=\frac{\mathrm{nE}^{\circ}}{0.0591}=\frac{2 \times 0.24 \mathrm{~V}}{0.0591}=\frac{0.48 \mathrm{~V}}{0.0591}=8.122\) The value indicates that products are formed 10 o  , times than reactants. (e) Those molecules which possess activation energy and collide in proper orientation undergo effective collisions.

(a) Zero order reaction. (b)  \(\frac{k}{2.303}\)   where 'k' is rate constant. (c) t 1/2 is directly proportional to initial concentration. (d)  t  99. 9 % = 10 t 1/2 = 10 x 40 = 400 minutes (e)  \(t_{1 / 2}=\frac{[\mathrm{R}]_{0}}{2 k}\)   for zero order reaction.

(a) The rate of reaction first decreases with time then becomes constant. (b) CaCO 3 powder has more surface area than marble chips therefore, more rate of reaction. (c) The rate of reaction will increase because rate of reaction increases with the increase in concentration. (d) The rate of reaction increases with increase in pressure. (e) It is because number of molecules undergoing effective collisions become almost double, hence rate of reaction almost doubled.

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Chemical reaction kinetics : concepts, methods, and case studies

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• About the Author xi Preface xiii 1 Fundamentals of Chemical Reaction Kinetics 1 1.1 Concepts of Stoichiometry 1 1.1.1 Stoichiometric Number and Coefficient 1 1.1.2 Molecularity 2 1.1.3 Reaction Extent 3 1.1.4 Molar Conversion 4 1.1.5 Types of Feed Composition in a Chemical Reaction 5 1.1.6 Limiting Reactant 6 1.1.7 Molar Balance in a Chemical Reaction 7 1.1.8 Relationship between Conversion and Physical Properties of the Reacting System 8 1.2 Reacting Systems 11 1.2.1 Mole Fraction, Weight Fraction and Molar Concentration 11 1.2.2 Partial Pressure 13 1.2.3 Isothermal Systems at Constant Density 13 1.2.3.1 Relationship between Partial Pressure (pA) and Conversion (xA) 16 1.2.3.2 Relationship between Partial Pressure (pA) and Total Pressure (P) 16 1.2.3.3 Relationship between Molar Concentration (CA) and Total Pressure (P) 16 1.2.4 Isothermal Systems at Variable Density 18 1.2.5 General Case of Reacting Systems 22 1.2.6 Kinetic Point of View of the Chemical Equilibrium 22 1.3 Concepts of Chemical Kinetics 24 1.3.1 Rate of Homogeneous Reactions 24 1.3.2 Power Law 26 1.3.2.1 Relationship between kp and kc 27 1.3.2.2 Units of kc and kp 27 1.3.3 Elemental and Non-elemental Reactions 29 1.3.4 Comments on the Concepts of Molecularity and Reaction Order 30 1.3.5 Dependency of k with Temperature 30 1.3.5.1 Arrhenius Equation 30 1.3.5.2 Frequency Factor and Activation Energy 32 1.3.5.3 Evaluation of the Parameters of the Arrhenius Equation 32 1.3.5.4 Modified Arrhenius Equation 42 1.4 Description of Ideal Reactors 43 1.4.1 Batch Reactors 43 1.4.1.1 Modes of Operation 44 1.4.1.2 Data Collection 46 1.4.1.3 Mass Balance 48 1.4.2 Continuous Reactors 49 1.4.2.1 Space-Time and Space-Velocity 50 1.4.2.2 Plug Flow Reactor 50 1.4.2.3 Continuous Stirred Tank Reactor 52 2 Irreversible Reactions of One Component 55 2.1 Integral Method 56 2.1.1 Reactions of Zero Order 58 2.1.2 Reactions of the First Order 59 2.1.3 Reaction of the Second Order 61 2.1.4 Reactions of the nth Order 64 2.2 Differential Method 69 2.2.1 Numerical Differentiation 71 2.2.1.1 Method of Approaching the Derivatives ( dCA/dt) to ( CA/ t) or (dxA/dt) to ( xA/ t) 71 2.2.1.2 Method of Finite Differences 72 2.2.1.3 Method of a Polynomial of the nth Order 74 2.2.2 Graphical Differentiation 74 2.2.2.1 Method of Area Compensation 74 2.2.2.2 Method of Approaching the Derivative ( dCA/dt) to ( CA/ t) 76 2.2.2.3 Method of Finite Differences 77 2.2.2.4 Method of a Polynomial of the nth Order 78 2.2.2.5 Method of Area Compensation 80 2.2.2.6 Summary of Results 82 2.3 Method of Total Pressure 83 2.3.1 Reactions of Zero Order 84 2.3.2 Reactions of the First Order 85 2.3.3 Reactions of the Second Order 85 2.3.4 Reactions of the nth Order 86 2.3.5 Differential Method with Data of Total Pressure 88 2.4 Method of the Half-Life Time 91 2.4.1 Reactions of Zero Order 92 2.4.2 Reactions of the First Order 92 2.4.3 Reaction of the Second Order 93 2.4.4 Reaction of the nth Order 93 2.4.5 Direct Method to Calculate k and n with Data of t1/2 95 2.4.6 Extension of the Method of Half-Life Time (t1/2) to Any Fractional Life Time (t1/m) 97 2.4.7 Calculation of Activation Energy with Data of Half-Life Time 97 2.4.8 Some Observations of the Method of Half-Life Time 99 2.4.8.1 Calculation of n with Two Data of t1/2Measured with Different CAo 99 2.4.8.2 Generalization of the Method of Half-Life Time for Any Reaction Order 101 3 Irreversible Reactions with Two or Three Components 103 3.1 Irreversible Reactions with Two Components 103 3.1.1 Integral Method 103 3.1.1.1 Method of Stoichiometric Feed Composition 104 3.1.1.2 Method of Non-stoichiometric Feed Composition 109 3.1.1.3 Method of a Reactant in Excess 117 3.1.2 Differential Method 120 3.1.2.1 Stoichiometric Feed Composition 120 3.1.2.2 Feed Composition with a Reactant in Excess 120 3.1.2.3 Non-stoichiometric Feed Compositions 121 3.1.3 Method of Initial Reaction Rates 123 3.2 Irreversible Reactions between Three Components 127 3.2.1 Case
• 1: Stoichiometric Feed Composition 127 3.2.2 Case
• 2: Non-stoichiometric Feed Composition 129 3.2.3 Case
• 3: Feed Composition with One Reactant in Excess 130 3.2.4 Case
• 4: Feed Composition with Two Reactants in Excess 131 4 Reversible Reactions 135 4.1 Reversible Reactions of First Order 135 4.2 Reversible Reactions of Second Order 139 4.3 Reversible Reactions with Combined Orders 146 5 Complex Reactions 153 5.1 Yield and Selectivity 153 5.2 Simultaneous or Parallel Irreversible Reactions 155 5.2.1 Simultaneous Reactions with the Same Order 155 5.2.1.1 Case
• 1: Reactions with Only One Reactant 155 5.2.1.2 Case
• 2: Reactions with Two Reactants 161 5.2.2 Simultaneous Reactions with Combined Orders 163 5.2.2.1 Integral Method 165 5.2.2.2 Differential Method 166 5.3 Consecutive or In-Series Irreversible Reactions 167 5.3.1 Consecutive Reactions with the Same Order 167 5.3.1.1 Calculation of CR max and t 171 5.3.1.2 Calculation of CR max and t for k1= k2 172 5.3.2 Consecutive Reactions with Combined Orders 174 6 Special Topics in Kinetic Modelling 179 6.1 Data Reconciliation 180 6.1.1 Data Reconciliation Method 181 6.1.2 Results and Discussion 182 6.1.2.1 Source of Data 182 6.1.2.2 Global Mass Balances 185 6.1.2.3 Outlier Determination 187 6.1.2.4 Data Reconciliation 187 6.1.2.5 Analysis of Results 189 6.1.3 Conclusions 195 6.2 Methodology for Sensitivity Analysis of Parameters 196 6.2.1 Description of the Method 198 6.2.1.1 Initialization of Parameters 199 6.2.1.2 Non-linear Parameter Estimation 201 6.2.1.3 Sensitivity Analysis 201 6.2.1.4 Residual Analysis 202 6.2.2 Results and Discussion 202 6.2.2.1 Experimental Data and the Reaction Rate Model from the Literature 202 6.2.2.2 Initialization of Parameters 204 6.2.2.3 Results of Non-linear Estimation 206 6.2.2.4 Sensitivity Analysis 207 6.2.2.5 Analysis of Residuals 210 6.2.3 Conclusions 210 6.3 Methods for Determining Rate Coefficients in Enzymatic Catalysed Reactions 211 6.3.1 The Michaelis-Menten Model 213 6.3.1.1 Origin 213 6.3.1.2 Development of the Model 213 6.3.1.3 Importance of Vmax and Km 214 6.3.2 Methods to Determine the Rate Coefficients of the Michaelis-Menten Equation 214 6.3.2.1 Linear Regression 214 6.3.2.2 Graphic Method 215 6.3.2.3 Integral Method 215 6.3.2.4 Non-linear Regression 216 6.3.3 Application of the Methods 217 6.3.3.1 Experimental Data 217 6.3.3.2 Calculation of Kinetic Parameters 220 6.3.4 Discussion of Results 222 6.3.5 Conclusions 225 6.4 A Simple Method for Estimating Gasoline, Gas and Coke Yields in FCC Processes 226 6.4.1 Introduction 226 6.4.2 Methodology 227 6.4.2.1 Choosing the Kinetic Models 227 6.4.2.2 Reaction Kinetics 228 6.4.2.3 Estimation of Kinetic Parameters 229 6.4.2.4 Evaluation of Products Yields 230 6.4.2.5 Advantages and Limitations of the Methodology 230 6.4.3 Results and Discussion 231 6.4.4 Conclusions 234 6.5 Estimation of Activation Energies during Hydrodesulphurization of Middle Distillates 234 6.5.1 Introduction 234 6.5.2 Experiments 235 6.5.3 Results and Discussion 236 6.5.3.1 Experimental Results 236 6.5.3.2 Estimation of Kinetic Parameters 237 6.5.3.3 Effect of Feed Properties on Kinetic Parameters 240 6.5.4 Conclusions 241 Problems 243 Nomenclature 273 References 277 Index 283.
• (source: Nielsen Book Data)
• Chapter 1. Fundamentals of chemical reaction kinetics 1.1. Concepts of stoichiometry 1.1.1. Stoichiometric number and coefficient 1.1.2. Molecularity 1.1.3. Reaction extent 1.1.4. Molar conversion 1.1.5. Types of feed composition in a chemical reaction 1.1.6. Limiting reactant 1.1.7. Molar balance in a chemical reaction 1.1.8. Relationship between conversion and physical properties of the reacting system 1.2. Reacting systems 1.2.1. Mole fraction, weight fraction and molar concentration 1.2.2. Partial pressure 1.2.3. Isothermal systems at constant density 1.2.4. Isothermal systems at variable density 1.2.5. General case of reacting systems 1.2.6. Kinetic point of view of the chemical equilibrium 1.3. Concepts of chemical kinetics 1.3.1. Rate of homogeneous reactions 1.3.2. Power law 1.3.3. Elemental and non-elemental reactions 1.3.4. Comments on the concepts of molecularity and reaction order 1.3.5. Dependency of k with temperature 1.4. Description of ideal reactors 1.4.1. Batch reactor 1.4.2. Continuous reactors
• Chapter 2. Irreversible reactions of one component 2.1. Integral method 2.1.1. Reactions of zero order 2.1.2. Reactions of first order 2.1.3. Reaction of second order 2.1.4. Reactions of nth order 2.2. Differential method 2.2.1. Numerical differentiation 2.2.2. Graphical differentiation 2.3. Method of total pressure 2.3.1. Reactions of zero order 2.3.2. Reactions of first order 2.3.3. Reactions of second order 2.3.4. Reactions of nth order 2.3.5. Differential method with data of total pressure 2.4. Method of the half-life time 2.4.1. Reactions of zero order 2.4.2. Reactions of first order 2.4.3. Reaction of second order 2.4.4. Reaction of nth order 2.4.5. Direct method to calculate k and n with data of t1/2 2.4.6. Extension of the method of half-life time (t1/2) to any fractional life time (t1/m) 2.4.7. Calculation of activation energy with data of half-life time 2.4.8. Some observations of the method of half-life time
• Chapter 3. Irreversible reactions with two or three components 3.1. Irreversible reactions with two components 3.1.1. Integral method 3.1.2. Differential method 3.1.3. Method of initial reaction rates 3.2. Irreversible reactions between three components
• Chapter 4. Reversible reactions 4.1. Reversible reactions of first order 4.2. Reversible reactions of second order 4.3. Reversible reactions with combined orders
• Chapter 5. Complex reactions 5.1. Yield and selectivity 5.2. Simultaneous or parallel irreversible reactions 5.2.1. Simultaneous reactions with the same order 5.2.2. Simultaneous reactions with combined orders 5.3. Consecutive or in series irreversible reactions 5.3.1. Consecutive reactions with the same order 5.3.2. Consecutive reactions with combined orders
• Chapter 6. Special topics in kinetic modeling 6.1. Data reconciliation 6.1.1. Data reconciliation method 6.1.2. Results and discussion 6.1.3. Conclusions 6.2. Methodology for sensitivity analysis of parameters 6.2.1. Description of the method 6.2.2. Results and discussion 6.2.3. Conclusions 6.3. Methods for determining rate coefficients in enzymatic catalyzed reactions 6.3.1. The model of Michaelis-Menten 6.3.2. Methods to determine the rate coefficients of the Michaelis-Menten equation 6.3.3. Application of the methods 6.3.4. Discussion of results 6.3.5. Conclusions 6.4. A simple method for estimating gasoline, gas and coke yields in FCC processes 6.4.1. Introduction 6.4.2. Methodology 6.4.3. Results and discussion 6.4.4 Conclusions 6.5. Estimation of activation energies during hydrodesulfurization of middle distillates 6.5.1. Introduction 6.5.2. Experimental 6.5.3. Results and discussion 6.5.4. Conclusions Problems References Nomenclature.

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