1. The role of a catalyst is to change the activation energy of reaction by providing an alternate reaction pathway that requires less energy.
2. In the presence of a catalyst, the heat evolved or absorbed during the reaction remains unchanged as the catalyst does not alter the enthalpy change of the reaction.
3. Activation energy of a chemical reaction can be determined by determining the rate constants at two temperatures.
4. For a general reaction A → B, if the concentration of A decreases exponentially with time, the reaction is first order with respect to A.
chemistry exemplar class 12 electrochemistry pdfRohit Raj Ranjan
Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction ("redox") reaction
1. This document provides a multiple choice quiz on concepts in thermodynamics. It covers topics like the properties of mixtures, open and closed systems, gas laws, heat capacities, ideal gases, and processes like compression and expansion.
2. There are 31 multiple choice questions testing understanding of concepts like intensive and extensive properties, different temperature scales, values of the universal gas constant, gas laws, standard temperature and pressure, heat capacities, ideal gas behavior, processes in turbines and compressors, and use of charts like Mollier diagrams.
3. The questions require identifying properties and processes, calculating values like partial pressures and molar densities, matching concepts to definitions, and determining final conditions based on given initial states and
Applied Chemistry Multiple Choice Questions with Answers Part 2 by Malik XufyanMalik Xufyan
This document provides a multiple choice quiz on green chemistry and sustainable methods of chemical synthesis. It includes 10 questions on needs of green chemistry, focusing on definitions of green chemistry, desirable properties of green solvents, and atom efficiency. Another 10 questions cover principles of green chemistry, including eliminating harmful treatments, safer products, and applying principles across the lifecycle. The final 10 questions are about methods of synthesis, discussing atom economy of green methods, microfluid reactors, catalysts, and producing high quality products with no waste.
Kinetics Limited is a company that studies ways to increase the rates of chemical reactions. They tested the effects of temperature, surface area, concentration, and stirring on two sets of chemical reactions. Increasing the temperature, surface area, or concentration generally increased the reaction rates. Stirring the solution also increased the reaction rate of one chemical set. The company recommends heating reactions to a certain temperature, increasing surface area by cutting one reactant, using a minimum concentration, and stirring solutions at a certain speed to increase reaction rates.
Applied Chemistry Multiple Choice Questions with Answers Part 3 by Malik XufyanMalik Xufyan
This document provides 15 multiple choice questions about the mechanisms of polymerization. It discusses chain polymerization which occurs through addition reactions in three steps: initiation, propagation, and termination. Initiators like benzoyl peroxide produce free radicals to start the chain reaction. Step polymerization occurs through condensation reactions between functional groups on monomers. Common mechanisms are free radical, ionic (cationic and anionic), and coordination polymerization which uses Ziegler-Natta catalysts.
Some basic concepts of chemistry exercise with solutionssuresh gdvm
This document contains sample questions and answers from Class 11 chemistry Chapter 1 on basic chemistry concepts. The questions calculate molecular masses, empirical and molecular formulas, mass percentages of elements in compounds, moles of reactants and products in chemical reactions, molarity and molality calculations. It also defines terms like significant figures, pressure, mass and prefixes related to the International System of Units.
chemistry exemplar class 12 electrochemistry pdfRohit Raj Ranjan
Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction ("redox") reaction
1. This document provides a multiple choice quiz on concepts in thermodynamics. It covers topics like the properties of mixtures, open and closed systems, gas laws, heat capacities, ideal gases, and processes like compression and expansion.
2. There are 31 multiple choice questions testing understanding of concepts like intensive and extensive properties, different temperature scales, values of the universal gas constant, gas laws, standard temperature and pressure, heat capacities, ideal gas behavior, processes in turbines and compressors, and use of charts like Mollier diagrams.
3. The questions require identifying properties and processes, calculating values like partial pressures and molar densities, matching concepts to definitions, and determining final conditions based on given initial states and
Applied Chemistry Multiple Choice Questions with Answers Part 2 by Malik XufyanMalik Xufyan
This document provides a multiple choice quiz on green chemistry and sustainable methods of chemical synthesis. It includes 10 questions on needs of green chemistry, focusing on definitions of green chemistry, desirable properties of green solvents, and atom efficiency. Another 10 questions cover principles of green chemistry, including eliminating harmful treatments, safer products, and applying principles across the lifecycle. The final 10 questions are about methods of synthesis, discussing atom economy of green methods, microfluid reactors, catalysts, and producing high quality products with no waste.
Kinetics Limited is a company that studies ways to increase the rates of chemical reactions. They tested the effects of temperature, surface area, concentration, and stirring on two sets of chemical reactions. Increasing the temperature, surface area, or concentration generally increased the reaction rates. Stirring the solution also increased the reaction rate of one chemical set. The company recommends heating reactions to a certain temperature, increasing surface area by cutting one reactant, using a minimum concentration, and stirring solutions at a certain speed to increase reaction rates.
Applied Chemistry Multiple Choice Questions with Answers Part 3 by Malik XufyanMalik Xufyan
This document provides 15 multiple choice questions about the mechanisms of polymerization. It discusses chain polymerization which occurs through addition reactions in three steps: initiation, propagation, and termination. Initiators like benzoyl peroxide produce free radicals to start the chain reaction. Step polymerization occurs through condensation reactions between functional groups on monomers. Common mechanisms are free radical, ionic (cationic and anionic), and coordination polymerization which uses Ziegler-Natta catalysts.
Some basic concepts of chemistry exercise with solutionssuresh gdvm
This document contains sample questions and answers from Class 11 chemistry Chapter 1 on basic chemistry concepts. The questions calculate molecular masses, empirical and molecular formulas, mass percentages of elements in compounds, moles of reactants and products in chemical reactions, molarity and molality calculations. It also defines terms like significant figures, pressure, mass and prefixes related to the International System of Units.
Based on the diagram above, name the labelled parts and state their functions:
A - Safety goggle
Function: To protect eyes from chemical splashes or flying objects.
B - Gloves
Function: To protect hands from chemicals and prevent skin contact with hazardous substances.
C - Laboratory coat
Function: To protect body from chemicals and prevent contamination of clothing.
D - Face mask
Function: To protect face and prevent inhalation of hazardous fumes/vapours.
E - Safety shoes
Function: To protect feet from chemicals, broken glass and prevent slips.
F - Fume chamber
Function: To contain and remove noxious fumes/vap
This document contains a 50 question chemistry exam with multiple choice answers for each question. The questions cover topics such as kinetics, equilibrium, organic chemistry, thermodynamics, and other general chemistry topics. No answers are provided for the multiple choice questions.
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
The document discusses key concepts about chemical reactions and equations including:
1. Chemical equations are used to represent chemical reactions, with reactants on the left side and products on the right side.
2. A reaction is endothermic if heat energy is absorbed, and exothermic if heat energy is released.
3. The law of conservation of matter states that the number and type of atoms is the same for both reactants and products, though they may be rearranged. Mass is also conserved in chemical reactions.
01. basic concepts of chemistry 1(final)Anurag Bhatt
This document provides an overview of basic chemistry concepts including the branches of chemistry, units and standards used in chemistry, significant figures, and dimensions. It discusses the SI system of units, fundamental and derived units, and conversions between units. It also defines key chemistry terms like matter, elements, compounds, and mixtures. The document contains examples of calculations involving significant figures and dimensional analysis.
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
F.Sc. Part 1 Chemistry Paper Faisalabad Board 2013 (Malik Xufyan)Malik Xufyan
1. The document contains a chemistry exam paper with multiple choice and subjective questions.
2. The multiple choice section has 17 questions testing concepts like the properties of different compounds, stoichiometry, gas laws, and acid-base chemistry.
3. The subjective section requires explaining concepts such as crystal structures, hybridization, kinetic molecular theory, X-rays, electrolysis, acid-base equilibria, and order of reactions. It also involves solving stoichiometry and pH problems.
1. The document discusses factors that affect the rate of chemical reactions, including temperature, concentration, and surface area of reactants.
2. It provides examples of experiments measuring the rate of production of gases over time to determine the rate of reactions.
3. Increasing the temperature was identified as the most effective way to increase the rate of reactions discussed in the examples, such as the decomposition of hydrogen peroxide and the reaction of zinc with hydrochloric acid.
This document describes a catalytic method for synthesizing 5-substituted 1H-tetrazoles using various nitriles and sodium azide. Copper powder and copper sulfate are used to generate active copper(I) catalyst in situ via a comproportionation reaction. This copper(I) species catalyzes the [3+2] cycloaddition of the nitriles and sodium azide to form the tetrazoles in good yields. Reaction calorimetry studies showed the reaction is slightly exothermic and can be safely conducted at 123°C with efficient cooling. A range of structurally diverse nitriles reacted smoothly under these conditions, demonstrating the generality of this copper-catalyzed method for
MCAT CHEMISTRY SOLVED PAST PAPERS (2008-2016) - Malik XufyanMalik Xufyan
This document contains 100 multiple choice questions from past MCAT Chemistry papers from 2008-2009. The questions cover various topics in chemistry including bonding, reactions, stoichiometry, states of matter, thermodynamics and organic chemistry. This review material is intended to help students prepare for the MCAT entrance exam by practicing with prior year exam questions.
This document outlines the learning outcomes for a unit on rates of reaction in Leaving Certificate Chemistry. It includes topics such as defining rate of reaction, factors that affect rates like concentration and temperature, using graphs to analyze reaction rates, the concept of activation energy, and using catalysts to lower activation energy and increase reaction rates based on surface adsorption and intermediate formation theories of catalysis. Pupils are expected to conduct experiments on catalysts and reaction rates and explain concepts like dust explosions and catalytic converters.
Chemical speciation studies on complexation of ditopic ligands: Interaction o...iosrjce
IOSR Journal of Applied Chemistry (IOSR-JAC) is a double blind peer reviewed International Journal that provides rapid publication (within a month) of articles in all areas of applied chemistry and its applications. The journal welcomes publications of high quality papers on theoretical developments and practical applications in Chemical Science. Original research papers, state-of-the-art reviews, and high quality technical notes are invited for publications.
Definitions and MCQs of Ninth class chemistry (solution and suspension)Dr. Sajid Ali Talpur
The document defines key terms related to solutions and suspensions, including solute, solvent, saturated solution, and suspension. It then provides 16 multiple choice questions testing understanding of these concepts. Key topics covered include how temperature and pressure affect solubility, definitions of saturation, unsaturated and supersaturated solutions, and the processes of crystallization and sublimation.
This document provides information about mole concept, oxidation-reduction reactions, and titrations. It begins with defining oxidation and reduction processes and listing examples. Rules for determining oxidation numbers and methods for calculating individual oxidation numbers are outlined. The concepts of oxidizing agents, reducing agents, and disproportionation reactions are explained. The document describes how to balance redox reactions using the ion-electron method in both acidic and basic media. Equivalents, normality, and the law of equivalence are defined. Finally, the document discusses types of titrations and provides a table of common redox titrations.
unit-03,04 :- Coarse dispersion, Drug StabilityGourav Singh
1. The document contains a quiz on physical pharmaceutics topics like reaction kinetics, order of reactions, and shelf life.
2. The questions cover concepts like determining the order of a reaction, rate constants, half lives, and examples of first order and second order reactions.
3. The quiz also includes questions related to suspensions like sedimentation volume, factors affecting flocculation, and examples of suspending agents.
This document discusses the syllabus for the JEE chemistry exam, which is divided into 3 sections: physical chemistry, inorganic chemistry, and organic chemistry. It provides details on the topics covered and number of units in each section. These include chemical thermodynamics, kinetics, and bonding in physical chemistry; p-block and d-block elements and coordination compounds in inorganic chemistry; and organic compounds containing oxygen, halogen, and basic principles of organic chemistry. It also contains example questions and solutions to help understand various chemistry concepts.
The document summarizes a chemistry experiment that investigated how the concentration of hydrochloric acid (HCl) affects the rate of reaction when magnesium (Mg) is added. It was hypothesized that higher HCl concentrations would increase the reaction rate. Experiments were conducted using different HCl concentrations from 0.1M to 0.5M. The results showed that higher concentrations produced hydrogen gas faster, supporting the hypothesis. A graph of the reaction rates demonstrated they increased quadratically with increasing HCl concentration. However, the conclusion noted some weaknesses in temperature control and material reuse that could be improved.
F.Sc. Part 1 Paper Faisalabad Board 2007 (Malik Xufyan)Malik Xufyan
This document contains a chemistry exam with multiple choice and subjective questions covering various topics in chemistry including stoichiometry, atomic structure, chemical bonding, solutions, equilibrium, and thermochemistry. The exam has two sections - the first with 22 short answer questions and the second containing 3 long answer questions to attempt. Some sample questions ask about the mass of an electron, diffusion vs effusion of gases, ionic character of hydrogen halides, quantum numbers and their significance, classification of atomic orbital hybridization, and balancing chemical equations using oxidation numbers.
This chapter discusses stoichiometry, including atomic masses, the mole concept, molar masses, percent composition of compounds, determining empirical and molecular formulas, writing and balancing chemical equations, and stoichiometric calculations involving amounts of reactants and products. Key aspects covered are determining the limiting reagent, using balanced equations to determine mole ratios, and calculating mass relationships in chemical reactions based on these mole ratios.
Chemistry zimsec chapter 8 chemical equilibriaalproelearning
(1) This document discusses chemical equilibria, including reversible reactions, factors that affect equilibrium, and acid-base theories.
(2) It describes how reversible reactions reach equilibrium when the rates of the forward and reverse reactions are equal. Le Chatelier's principle states that if a stress is applied to a system at equilibrium, it will shift in a way to counteract the stress.
(3) Equilibrium constants Kc and Kp are introduced, which do not depend on concentration or pressure changes. The Brønsted-Lowry acid-base theory defines acids as proton donors and bases as proton acceptors.
This document discusses reaction kinetics including:
1) Rate equations relate the rate of reaction to reactant concentrations and can be determined experimentally. The orders of reaction indicate how changing concentrations affect rate.
2) Reaction mechanisms involve multiple steps, with the rate determined by the slowest step. Molecularity refers to the number of species involved in a step.
3) Catalysts increase reaction rates by providing alternative reaction pathways. Heterogeneous catalysts involve different phases while homogeneous catalysts are the same phase as reactants. Common examples are discussed.
Based on the diagram above, name the labelled parts and state their functions:
A - Safety goggle
Function: To protect eyes from chemical splashes or flying objects.
B - Gloves
Function: To protect hands from chemicals and prevent skin contact with hazardous substances.
C - Laboratory coat
Function: To protect body from chemicals and prevent contamination of clothing.
D - Face mask
Function: To protect face and prevent inhalation of hazardous fumes/vapours.
E - Safety shoes
Function: To protect feet from chemicals, broken glass and prevent slips.
F - Fume chamber
Function: To contain and remove noxious fumes/vap
This document contains a 50 question chemistry exam with multiple choice answers for each question. The questions cover topics such as kinetics, equilibrium, organic chemistry, thermodynamics, and other general chemistry topics. No answers are provided for the multiple choice questions.
Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions based on mole ratios from balanced equations. Key concepts include:
1) Balanced equations show mole, mass, and particle relationships between reactants and products
2) Limiting reactants determine the maximum amount of product that can be formed
3) Excess reactants remain after the limiting reactant is used up in the reaction
The document discusses key concepts about chemical reactions and equations including:
1. Chemical equations are used to represent chemical reactions, with reactants on the left side and products on the right side.
2. A reaction is endothermic if heat energy is absorbed, and exothermic if heat energy is released.
3. The law of conservation of matter states that the number and type of atoms is the same for both reactants and products, though they may be rearranged. Mass is also conserved in chemical reactions.
01. basic concepts of chemistry 1(final)Anurag Bhatt
This document provides an overview of basic chemistry concepts including the branches of chemistry, units and standards used in chemistry, significant figures, and dimensions. It discusses the SI system of units, fundamental and derived units, and conversions between units. It also defines key chemistry terms like matter, elements, compounds, and mixtures. The document contains examples of calculations involving significant figures and dimensional analysis.
Here is a one page paper relating chemistry and gases:
Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxide
F.Sc. Part 1 Chemistry Paper Faisalabad Board 2013 (Malik Xufyan)Malik Xufyan
1. The document contains a chemistry exam paper with multiple choice and subjective questions.
2. The multiple choice section has 17 questions testing concepts like the properties of different compounds, stoichiometry, gas laws, and acid-base chemistry.
3. The subjective section requires explaining concepts such as crystal structures, hybridization, kinetic molecular theory, X-rays, electrolysis, acid-base equilibria, and order of reactions. It also involves solving stoichiometry and pH problems.
1. The document discusses factors that affect the rate of chemical reactions, including temperature, concentration, and surface area of reactants.
2. It provides examples of experiments measuring the rate of production of gases over time to determine the rate of reactions.
3. Increasing the temperature was identified as the most effective way to increase the rate of reactions discussed in the examples, such as the decomposition of hydrogen peroxide and the reaction of zinc with hydrochloric acid.
This document describes a catalytic method for synthesizing 5-substituted 1H-tetrazoles using various nitriles and sodium azide. Copper powder and copper sulfate are used to generate active copper(I) catalyst in situ via a comproportionation reaction. This copper(I) species catalyzes the [3+2] cycloaddition of the nitriles and sodium azide to form the tetrazoles in good yields. Reaction calorimetry studies showed the reaction is slightly exothermic and can be safely conducted at 123°C with efficient cooling. A range of structurally diverse nitriles reacted smoothly under these conditions, demonstrating the generality of this copper-catalyzed method for
MCAT CHEMISTRY SOLVED PAST PAPERS (2008-2016) - Malik XufyanMalik Xufyan
This document contains 100 multiple choice questions from past MCAT Chemistry papers from 2008-2009. The questions cover various topics in chemistry including bonding, reactions, stoichiometry, states of matter, thermodynamics and organic chemistry. This review material is intended to help students prepare for the MCAT entrance exam by practicing with prior year exam questions.
This document outlines the learning outcomes for a unit on rates of reaction in Leaving Certificate Chemistry. It includes topics such as defining rate of reaction, factors that affect rates like concentration and temperature, using graphs to analyze reaction rates, the concept of activation energy, and using catalysts to lower activation energy and increase reaction rates based on surface adsorption and intermediate formation theories of catalysis. Pupils are expected to conduct experiments on catalysts and reaction rates and explain concepts like dust explosions and catalytic converters.
Chemical speciation studies on complexation of ditopic ligands: Interaction o...iosrjce
IOSR Journal of Applied Chemistry (IOSR-JAC) is a double blind peer reviewed International Journal that provides rapid publication (within a month) of articles in all areas of applied chemistry and its applications. The journal welcomes publications of high quality papers on theoretical developments and practical applications in Chemical Science. Original research papers, state-of-the-art reviews, and high quality technical notes are invited for publications.
Definitions and MCQs of Ninth class chemistry (solution and suspension)Dr. Sajid Ali Talpur
The document defines key terms related to solutions and suspensions, including solute, solvent, saturated solution, and suspension. It then provides 16 multiple choice questions testing understanding of these concepts. Key topics covered include how temperature and pressure affect solubility, definitions of saturation, unsaturated and supersaturated solutions, and the processes of crystallization and sublimation.
This document provides information about mole concept, oxidation-reduction reactions, and titrations. It begins with defining oxidation and reduction processes and listing examples. Rules for determining oxidation numbers and methods for calculating individual oxidation numbers are outlined. The concepts of oxidizing agents, reducing agents, and disproportionation reactions are explained. The document describes how to balance redox reactions using the ion-electron method in both acidic and basic media. Equivalents, normality, and the law of equivalence are defined. Finally, the document discusses types of titrations and provides a table of common redox titrations.
unit-03,04 :- Coarse dispersion, Drug StabilityGourav Singh
1. The document contains a quiz on physical pharmaceutics topics like reaction kinetics, order of reactions, and shelf life.
2. The questions cover concepts like determining the order of a reaction, rate constants, half lives, and examples of first order and second order reactions.
3. The quiz also includes questions related to suspensions like sedimentation volume, factors affecting flocculation, and examples of suspending agents.
This document discusses the syllabus for the JEE chemistry exam, which is divided into 3 sections: physical chemistry, inorganic chemistry, and organic chemistry. It provides details on the topics covered and number of units in each section. These include chemical thermodynamics, kinetics, and bonding in physical chemistry; p-block and d-block elements and coordination compounds in inorganic chemistry; and organic compounds containing oxygen, halogen, and basic principles of organic chemistry. It also contains example questions and solutions to help understand various chemistry concepts.
The document summarizes a chemistry experiment that investigated how the concentration of hydrochloric acid (HCl) affects the rate of reaction when magnesium (Mg) is added. It was hypothesized that higher HCl concentrations would increase the reaction rate. Experiments were conducted using different HCl concentrations from 0.1M to 0.5M. The results showed that higher concentrations produced hydrogen gas faster, supporting the hypothesis. A graph of the reaction rates demonstrated they increased quadratically with increasing HCl concentration. However, the conclusion noted some weaknesses in temperature control and material reuse that could be improved.
F.Sc. Part 1 Paper Faisalabad Board 2007 (Malik Xufyan)Malik Xufyan
This document contains a chemistry exam with multiple choice and subjective questions covering various topics in chemistry including stoichiometry, atomic structure, chemical bonding, solutions, equilibrium, and thermochemistry. The exam has two sections - the first with 22 short answer questions and the second containing 3 long answer questions to attempt. Some sample questions ask about the mass of an electron, diffusion vs effusion of gases, ionic character of hydrogen halides, quantum numbers and their significance, classification of atomic orbital hybridization, and balancing chemical equations using oxidation numbers.
This chapter discusses stoichiometry, including atomic masses, the mole concept, molar masses, percent composition of compounds, determining empirical and molecular formulas, writing and balancing chemical equations, and stoichiometric calculations involving amounts of reactants and products. Key aspects covered are determining the limiting reagent, using balanced equations to determine mole ratios, and calculating mass relationships in chemical reactions based on these mole ratios.
Chemistry zimsec chapter 8 chemical equilibriaalproelearning
(1) This document discusses chemical equilibria, including reversible reactions, factors that affect equilibrium, and acid-base theories.
(2) It describes how reversible reactions reach equilibrium when the rates of the forward and reverse reactions are equal. Le Chatelier's principle states that if a stress is applied to a system at equilibrium, it will shift in a way to counteract the stress.
(3) Equilibrium constants Kc and Kp are introduced, which do not depend on concentration or pressure changes. The Brønsted-Lowry acid-base theory defines acids as proton donors and bases as proton acceptors.
This document discusses reaction kinetics including:
1) Rate equations relate the rate of reaction to reactant concentrations and can be determined experimentally. The orders of reaction indicate how changing concentrations affect rate.
2) Reaction mechanisms involve multiple steps, with the rate determined by the slowest step. Molecularity refers to the number of species involved in a step.
3) Catalysts increase reaction rates by providing alternative reaction pathways. Heterogeneous catalysts involve different phases while homogeneous catalysts are the same phase as reactants. Common examples are discussed.
This document discusses key concepts in chemical kinetics including:
1. Chemical kinetics is the study of reaction rates and mechanisms under different conditions. Reaction rates can be expressed as changes in concentration over time.
2. Rate laws describe the relationship between reaction rates and reactant concentrations. Rate constants are measured at specific temperatures.
3. The Arrhenius equation relates reaction rates to temperature via an activation energy term, explaining why higher temperatures increase reaction rates by providing more molecules with sufficient kinetic energy.
F.Sc. Part 1 Chemistry Paper Faisalabad Board 2011 (Malik Xufyan)Malik Xufyan
This document contains a chemistry exam with multiple choice and subjective questions covering various topics:
1. The multiple choice section contains 17 questions testing concepts like the octet rule, standard enthalpy change, pH calculations, cathode materials in batteries, percentage compositions, and isotopes.
2. The subjective section asks students to define key terms, explain concepts like limiting reactants and gas behavior, solve problems involving electron mass and molecular formula determination, and balance a chemical equation.
3. Students must also answer 3 out of 7 multi-part essay questions covering topics such as liquid crystals, combustion analysis, Dalton's law of partial pressures, electronegativity, bomb calorimetry, and colligative properties.
The document summarizes key concepts relating to chemical kinetics and chemical equilibrium. It discusses how the rates of chemical reactions are determined by measuring changes in concentration over time. It also explains how reaction rates are affected by molecular collisions, activation energy, nature of reactants, concentration, temperature, and presence of catalysts. The document introduces chemical equilibrium as a dynamic steady state and defines equilibrium constants. It describes Le Chatelier's principle, explaining how changing concentrations, temperature, or pressure shifts equilibrium.
This document discusses methods for determining the order of a chemical reaction. It defines key terms like rate of reaction, order of reaction, molecularity, and half-life. It describes several methods to determine the order of a reaction:
1) The substitution method involves substituting concentration data into integrated rate equations for zero, first, and second order reactions to determine which gives a constant rate constant.
2) The graphical method plots concentration data versus time in different ways depending on the suspected order to identify linear relationships.
3) The half-life method examines how half-life depends on initial concentration to infer order.
4) Ostwald's isolation method determines partial orders with respect to each reactant by
Chemical kinetics describes the rates of chemical reactions. The three factors that affect reaction rates are concentration of reactants, temperature, and presence of a catalyst. An instantaneous rate is the rate of reaction at a specific moment in time. Beer's law relates the absorption of light to the concentration of an absorbing substance in a solution. First and second order reactions have rates dependent on the first or second power of the concentration of a reactant. Half-life is the time required for half of the reactants to be converted to products at a given reaction rate. Activation energy is the minimum energy that reactant molecules must possess for a reaction to occur.
This document contains a chemistry revision paper with 30 questions covering topics on the solid state and chemical kinetics. It provides instructions for the exam, including the number of marks allocated to each question and guidelines on using tables or calculators. The questions range from 1 to 5 marks and cover various concepts such as stoichiometric defects, rate constants, crystal structures, reaction orders, and activation energy. Graphical and numerical problems are included to calculate values like half-lives, rate constants, and Arrhenius parameters from experimental data. Definitions and examples are also tested around terms like isotropic, amorphous solids, and ferromagnetism. Reaction mechanisms and rate laws are analyzed for some hypothetical chemical reactions.
Chemical kinetics is the study of reaction rates and mechanisms. The rate of a reaction describes how quickly reactants are converted to products and is affected by factors like concentration, temperature, catalysts, and surface area. The rate law expresses the reaction rate in terms of reactant concentrations and can be used to determine the order of a reaction. Integrated rate laws relate concentration over time and are used to calculate quantities like half-life, the time for half the reactants to be consumed.
The document discusses chemical equilibrium and reversible reactions. It explains that in a reversible reaction, the reactants can transform into products, and the products can then react in reverse to reform the original reactants. At equilibrium, the rates of the forward and reverse reactions are equal and the concentrations of reactants and products remain constant. Mercury(II) oxide decomposing into mercury and oxygen, and then recombining, is provided as an example of a reversible reaction system at equilibrium. Factors that affect the rate and position of equilibrium, such as temperature, concentration, catalysts and pressure, are also described.
The document discusses kinetics and reaction rates. It defines kinetics as the branch of chemistry that studies the speed or rate of chemical reactions. It explains that reaction rates can be measured by changes in concentration, temperature, or pressure over time. The rate depends on factors like the nature of reactants, concentration, temperature, catalysts, surface area, and pressure. Reactions may occur in multiple steps through reaction intermediates rather than a single step. The collision theory and concept of activation energy are introduced to explain why certain collisions result in reactions. Reaction coordinate diagrams are used to illustrate the energy changes in reactions.
This document contains information about the II PUC Chemistry question bank and model question papers for the subject. It begins with a disclaimer noting that while efforts have been made to make the question bank comprehensive, errors may exist, and questions from the bank may not be the only ones appearing on examinations. It notes that the copyright of the question bank lies with the Director of the Department of Pre-University Education and it is for academic purposes only.
The document then provides the blueprints for two model question papers, outlining the distribution of questions from different topics across various parts of the papers. It allocates a total of 105 marks to the papers and divides them into parts A, B, C and D, with part A containing
The document discusses chemical kinetics and complex reaction mechanisms. It defines elementary reactions, complex reactions, and reaction intermediates. Complex reactions can involve competing reactions, opposing reactions, or consecutive reactions. Competing reactions are when a reactant undergoes two or more independent reactions simultaneously. Opposing reactions involve reversible reactions where the product reacts to reform the original reactants. Consecutive reactions occur in a sequence where the products of one reaction participate in subsequent reactions. Chain reactions are also discussed, which involve reactive intermediates that continuously generate and consume themselves in the reaction steps. Examples of each type of complex reaction are provided.
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
3. Provides information about the time it takes for a chemical reaction to occur
4. Provides information about the series of elementary steps which lead to the formation of product
The document discusses chemical kinetics and provides information about:
- The factors that affect the speed of a chemical reaction, including concentration, temperature, and catalysts.
- How to determine the rate law, rate constant, order, and mechanism of reactions from experimental data.
- The relationship between concentration and time for reactions of different orders (zero, first, and second order).
- How to calculate half-life, effect of temperature on reaction rate using the Arrhenius equation, and the role of homogeneous and heterogeneous catalysts.
F.Sc. Part 1 Chemistry.Ch.11.Test (Malik Xufyan)Malik Xufyan
This document contains information about Malik's Chemistry test series books for classes 9th, 10th, F.Sc part 1 and part 2. It provides chapter-wise and board paper-wise test series. It also mentions the publisher Jhang Institute for Advanced Studies and provides their contact details. The document contains the list of chapters and topics covered in the test series books along with their page numbers.
Chemical kinetics is the study of the speed of chemical reactions and factors that affect the reaction rate. It provides information about reaction feasibility, timescales, and reaction mechanisms. The rate of a reaction can be examined by measuring changes in reactant or product concentrations over time. Reaction rates are determined experimentally and may follow zero-order, first-order, pseudo-first order, or second-order rate laws depending on the rate-determining step. Factors like temperature, concentration, physical state, and catalysts influence reaction rates.
This document discusses kinetics and factors that affect reaction rates. It defines kinetics as how quickly reactions occur and the factors that influence reaction rates, such as temperature, concentration, and the presence of catalysts. Reaction rates are linked to reaction mechanisms - the step-by-step processes by which reactions take place. Increasing temperature leads to more collisions between reactant particles and faster reaction rates, as described by the Arrhenius equation. Catalysts lower the activation energy of reactions, speeding up reaction rates without being consumed.
F.Sc. Part 1 Chemistry.Ch.07.Test (Malik Xufyan)Malik Xufyan
The document provides information about chemistry test series books published by Malik Xufyan of JIAS Academy. It includes the following:
1. Test series books for 9th, 10th, F.Sc part 1 and part 2 classes covering chapters and full papers.
2. Contact details for Msc chemistry test series and other publications.
3. Index listing chapter topics and page numbers for chemistry tests covering experimental techniques, gases, liquids, atomic structure, chemical bonding, thermochemistry and other topics.
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chemistry exemplar class 12 chemical kinetics pdf
1. 1. The role of a catalyst is to change ______________.
(i) gibbs energy of reaction.
(ii) enthalpy of reaction.
(iii) activation energy of reaction.
(iv) equilibrium constant.
2. In the presence of a catalyst, the heat evolved or absorbed during the reaction
___________.
(i) increases.
(ii) decreases.
(iii) remains unchanged.
(iv) may increase or decrease.
3. Activation energy of a chemical reaction can be determined by _____________.
(i) determining the rate constant at standard temperature.
(ii) determining the rate constants at two
temperatures.
(iii) determining probability of collision.
(iv) using catalyst.
4. Consider Fig. 4.1 and mark the correct option.
(i) Activation energy of forward reaction is
E1
+ E2
and product is less stable than
reactant.
(ii) Activation energy of forward reaction is
E1
+E2
and product is more stable than
reactant.
I. Multiple Choice Questions (Type-I)
U
U
Un
n
ni
iit
t
t
4
4
C
C
CH
H
HE
E
EM
M
MI
IIC
C
CA
A
AL
L
L K
K
KI
IIN
N
NE
E
ET
T
TI
IIC
C
CS
S
S
C
C
CH
H
HE
E
EM
M
MI
IIC
C
CA
A
AL
L
L K
K
KI
IIN
N
NE
E
ET
T
TI
IIC
C
CS
S
S
Fig. 4.1
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2. 48
Exemplar Problems, Chemistry
(iii) Activation energy of both forward and backward reaction is E1
+E2
and
reactant is more stable than product.
(iv) Activation energy of backward reaction is E1 and product is more stable
than reactant.
5. Consider a first order gas phase decomposition reaction given below :
A(g) ⎯→ B(g) + C(g)
The initial pressure of the system before decomposition of A was pi
. After lapse
of time ‘t’, total pressure of the system increased by x units and became ‘pt’
The rate constant k for the reaction is given as _________.
(i)
2.303
log i
i
p
k
t p x
=
−
(ii)
2.303
log
2
i
i t
p
k
t p p
=
−
(iii)
2.303
log
2
i
i t
p
k
t p p
=
+
(iv)
2.303
log i
i
p
k
t p x
=
+
6. According to Arrhenius equation rate constant k is equal to a
–E / RT
A e . Which
of the following options represents the graph of ln k vs
1
T
?
(i) (ii)
(iii) (iv)
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3. 49 Chemical Kinetics
7. Consider the Arrhenius equation given below and mark the correct option.
a
–E / RT
= A e
k
(i) Rate constant increases exponentially with increasing activation energy
and decreasing temperature.
(ii) Rate constant decreases exponentially with increasing activation energy
and decreasing temperature.
(iii) Rate constant increases exponentially with decreasing activation energy
and decreasing temperature.
(iv) Rate constant increases exponentially with decreasing activation energy
and increasing temperature.
8. A graph of volume of hydrogen released vs time for the reaction between zinc
and dil.HCl is given in Fig. 4.2. On the basis of this mark the correct option.
(i) Average rate upto 40s is
3 2
40
V V
−
(ii) Average rate upto 40 seconds is 3 2
40 30
V V
−
−
(iii) Average rate upto 40 seconds is
3
40
V
(iv) Average rate upto 40 seconds is
3 1
40 20
V V
−
−
9. Which of the following statements is not correct about order of a reaction.
(i) The order of a reaction can be a fractional number.
(ii) Order of a reaction is experimentally determined quantity.
(iii) The order of a reaction is always equal to the sum of the stoichiometric
coefficients of reactants in the balanced chemical equation for a reaction.
(iv) The order of a reaction is the sum of the powers of molar concentration
of the reactants in the rate law expression.
10. Consider the graph given in Fig. 4.2. Which of the following options does not
show instantaneous rate of reaction at 40th second?
(i)
5 2
50 30
V V
−
−
(ii) 4 2
50 30
V V
−
−
(iii)
3 2
40 30
V V
−
−
(iv)
3 1
40 20
V V
−
−
Fig. 4.2
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4. 50
Exemplar Problems, Chemistry
11. Which of the following statements is correct?
(i) The rate of a reaction decreases with passage of time as the concentration
of reactants dereases.
(ii) The rate of a reaction is same at any time during the reaction.
(iii) The rate of a reaction is independent of temperature change.
(iv) The rate of a reaction decreases with increase in concentration of
reactant(s).
12. Which of the following expressions is correct for the rate of reaction given
below?
5Br
–
(aq) + BrO3
–
(aq) + 6H
+
(aq) ⎯→ 3Br2(aq) + 3H2O(l)
(i)
− +
Δ Δ
=
Δ Δ
[Br ] [H ]
5
t t
(ii)
[Br ] 6 [H ]
t 5 t
− +
Δ Δ
=
Δ Δ
(iii)
[Br ] 5 [H ]
t 6 t
− +
Δ Δ
=
Δ Δ
(iv)
[Br ] [H ]
6
t t
− +
Δ Δ
=
Δ Δ
13. Which of the following graphs represents exothermic reaction?
(a) (b)
(c)
(i) (a) only
(ii) (b) only
(iii) (c) only
(iv) (a) and (b)
5. 51 Chemical Kinetics
14. Rate law for the reaction A + 2B ⎯→ C is found to be
Rate = k [A][B]
Concentration of reactant ‘B’ is doubled, keeping the concentration of ‘A’
constant, the value of rate constant will be______.
(i) the same
(ii) doubled
(iii) quadrupled
(iv) halved
15. Which of the following statements is incorrect about the collison theory of
chemical reaction?
(i) It considers reacting molecules or atoms to be hard spheres and ignores
their structural features.
(ii) Number of effective collisions determines the rate of reaction.
(iii) Collision of atoms or molecules possessing sufficient threshold energy
results into the product formation.
(iv) Molecules should collide with sufficient threshold energy and proper
orientation for the collision to be effective.
16. A first order reaction is 50% completed in 1.26 × 1014
s. How much time
would it take for 100% completion?
(i) 1.26 × 1015
s
(ii) 2.52 × 1014 s
(iii) 2.52 × 1028 s
(iv) infinite
17. Compounds ‘A’ and ‘B’ react according to the following chemical equation.
A (g) + 2 B (g) ⎯→ 2C (g)
Concentration of either ‘A’ or ‘B’ were changed keeping the concentrations of
one of the reactants constant and rates were measured as a function of initial
concentration. Following results were obtained. Choose the correct option for
the rate equations for this reaction.
Experiment Initial Initial Initial rate of
concentration concentration formation of
of [A]/mol L–1
of [B]/mol L–1
[C]/mol L–1
s–1
1. 0.30 0.30 0.10
2. 0.30 0.60 0.40
3. 0.60 0.30 0.20
(i) Rate = k [A]2 [B]
(ii) Rate = k [A] [B]2
(iii) Rate = k [A] [B]
(iv) Rate = k [A]2 [B]0
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6. 52
Exemplar Problems, Chemistry
18. Which of the following statement is not correct for the catalyst?
(i) It catalyses the forward and backward reaction to the same extent.
(ii) It alters ΔG of the reaction.
(iii) It is a substance that does not change the equilibrium constant of a
reaction.
(iv) It provides an alternate mechanism by reducing activation energy
between reactants and products.
19. The value of rate constant of a pseudo first order reaction ____________.
(i) depends on the concentration of reactants present in small amount.
(ii) depends on the concentration of reactants present in excess.
(iii) is independent of the concentration of reactants.
(iv) depends only on temperature.
20. Consider the reaction A B. The concentration of both the reactants and
the products varies exponentially with time. Which of the following figures
correctly describes the change in concentration of reactants and products
with time?
(i) (ii)
(iii) (iv)
II. Multiple Choice Questions (Type-II)
Note : In the following questions two or more options may be correct.
21. Rate law cannot be determined from balanced chemical equation if _______.
(i) reverse reaction is involved.
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7. 53 Chemical Kinetics
(ii) it is an elementary reaction.
(iii) it is a sequence of elementary reactions.
(iv) any of the reactants is in excess.
22. Which of the following statements are applicable to a balanced chemical
equation of an elementary reaction?
(i) Order is same as molecularity.
(ii) Order is less than the molecularity.
(iii) Order is greater than the molecularity.
(iv) Molecularity can never be zero.
23. In any unimolecular reaction ______________.
(i) only one reacting species is involved in the rate determining step.
(ii) the order and the molecularity of slowest step are equal to one.
(iii) the molecularity of the reaction is one and order is zero.
(iv) both molecularity and order of the reaction are one.
24. For a complex reaction ______________.
(i) order of overall reaction is same as molecularity of the slowest step.
(ii) order of overall reaction is less than the molecularity of the slowest
step.
(iii) order of overall reaction is greater than molecularity of the slowest step.
(iv) molecularity of the slowest step is never zero or non interger.
25. At high pressure the following reaction is zero order.
2NH3
(g) ⎯⎯⎯⎯⎯⎯⎯⎯⎯⎯
→
1130 K
Platinum catalyst N2
(g) + 3H2
(g)
Which of the following options are correct for this reaction?
(i) Rate of reaction = Rate constant
(ii) Rate of the reaction depends on concentration of ammonia.
(iii) Rate of decomposition of ammonia will remain constant until ammonia
disappears completely.
(iv) Further increase in pressure will change the rate of reaction.
26. During decomposition of an activated complex
(i) energy is always released
(ii) energy is always absorbed
(iii) energy does not change
(iv) reactants may be formed
28. According to Maxwell Boltzmann distributon of energy, __________.
(i) the fraction of molecules with most probable kinetic energy decreases
at higher temperatures.
(ii) the fraction of molecules with most probable kinetic energy increases
at higher temperatures.
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8. 54
Exemplar Problems, Chemistry
(iii) most probable kinetic energy increases at higher temperatures.
(iv) most probable kinetic energy decreases at higher temperatures.
28. In the graph showing Maxwell Boltzman distribution of energy, ___________.
(i) area under the curve must not change with increase in temperature.
(ii) area under the curve increases with increase in temperature.
(iii) area under the curve decreases with increase in temperature.
(iv) with increase in temperature curve broadens and shifts to the right
hand side.
29. Which of the following statements are in accordance with the Arrhenius
equation?
(i) Rate of a reaction increases with increase in temperature.
(ii) Rate of a reaction increases with decrease in activation energy.
(iii) Rate constant decreases exponentially with increase in temperature.
(iv) Rate of reaction decreases with decrease in activation energy.
30. Mark the incorrect statements.
(i) Catalyst provides an alternative pathway to reaction mechanism.
(ii) Catalyst raises the activation energy.
(iii) Catalyst lowers the activation energy.
(iv) Catalyst alters enthalpy change of the reaction.
31. Which of the following graphs is correct for a zero order reaction?
(i) (ii)
(iii) (iv)
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9. 55 Chemical Kinetics
32. Which of the following graphs is correct for a first order reaction?
(i) (ii)
(iii) (iv)
III. Short Answer Type
33. State a condition under which a bimolecular reaction is kinetically first order
reaction.
34. Write the rate equation for the reaction 2A + B⎯→ C if the order of the reaction
is zero.
35. How can you determine the rate law of the following reaction?
2NO (g) + O2
(g) ⎯→ 2NO2
(g)
36. For which type of reactions, order and molecularity have the same value?
37. In a reaction if the concentration of reactant A is tripled, the rate of reaction
becomes twenty seven times. What is the order of the reaction?
38. Derive an expression to calculate time required for completion of zero order
reaction.
39. For a reaction A + B ⎯→ Products, the rate law is — Rate = k [A][B]3/2
Can the reaction be an elementary reaction? Explain.
40. For a certain reaction large fraction of molecules has energy more than the
threshold energy, yet the rate of reaction is very slow. Why?
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10. 56
Exemplar Problems, Chemistry
41. For a zero order reaction will the molecularity be equal to zero? Explain.
42. For a general reaction A ⎯→ B, plot of concentration of A vs time is given in
Fig. 4.3. Answer the following question on the basis of this graph.
(i) What is the order of the reaction?
(ii) What is the slope of the curve?
(iii) What are the units of rate constant?
Fig. 4.3
43. The reaction between H2
(g) and O2
(g) is highly feasible yet allowing the gases
to stand at room temperature in the same vessel does not lead to the formation
of water. Explain.
44. Why does the rate of a reaction increase with rise in temperature?
45. Oxygen is available in plenty in air yet fuels do not burn by themselves at
room temperature. Explain.
46. Why is the probability of reaction with molecularity higher than three
very rare?
47. Why does the rate of any reaction generally decreases during the course of
the reaction?
48. Thermodynamic feasibility of the reaction alone cannot decide the rate of the
reaction. Explain with the help of one example.
49. Why in the redox titration of KMnO4
vs oxalic acid, we heat oxalic acid solution
before starting the titration?
50. Why can’t molecularity of any reaction be equal to zero?
51. Why molecularity is applicable only for elementary reactions and order is
applicable for elementary as well as complex reactions?
52. Why can we not determine the order of a reaction by taking into consideration
the balanced chemical equation?
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11. 57 Chemical Kinetics
IV. Matching Type
Note : In the following questions match the items of Column I with
appropriate item given in Column II.
53. Match the graph given in Column I with the order of reaction given in Column II.
More than one item in Column I may link to the same item of Column II.
Column I Column II
(i)
(ii) (a) Ist order
(iii) (b) Zero order
(iv)
54. Match the statements given in Column I and Column II
Column I Column II
(i) Catalyst alters the rate of reaction (a) cannot be fraction or zero
(ii) Molecularity (b) proper orientation is not there
always
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12. 58
Exemplar Problems, Chemistry
(iii) Second half life of first order reaction (c) by lowering the activation
energy
(iv) E R T
a
– /
e (d) is same as the first
(v) Energetically favourable reactions (e) total probability is one
are sometimes slow
(vi) Area under the Maxwell (f) refers to the fraction of
Boltzman curve is constant molecules with energy equal
to or greater than activation
energy
55. Match the items of Column I and Column II.
Column I Column II
(i) Diamond (a) short interval of time
(ii) Instantaneous rate (b) ordinarily rate of conversion is
imperceptible
(iii) Average rate (c) long duration of time
56. Match the items of Column I and Column II.
Column I Column II
(i) Mathematical expression for (a) rate constant
rate of reaction
(ii) Rate of reaction for zero order (b) rate law
reaction is equal to
(iii) Units of rate constant for zero order (c) order of
reaction is same as that of slowest step
(iv) Order of a complex reaction is (d) rate of a reaction
determined by
V. Assertion and Reason Type
Note: In the following questions a statement of assertion followed by a statement
of reason is given. Choose the correct answer out of the following choices.
(i) Both assertion and reason are correct and the reason is correct explanation
of assertion.
(ii) Both assertion and reason are correct but reason does not explain
assertion.
(iii) Assertion is correct but reason is incorrect.
(iv) Both assertion and reason are incorrect.
(v) Assertion is incorrect but reason is correct.
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13. 59 Chemical Kinetics
57. Assertion : Order of the reaction can be zero or fractional.
Reason : We cannot determine order from balanced chemical equation.
58. Assertion : Order and molecularity are same.
Reason : Order is determined experimentally and molecularity is the
sum of the stoichiometric coefficient of rate determining
elementary step.
59. Assertion : The enthalpy of reaction remains constant in the presence of
a catalyst.
Reason : A catalyst participating in the reaction, forms different
activated complex and lowers down the activation energy but
the difference in energy of reactant and product remains the
same.
60. Assertion : All collision of reactant molecules lead to product formation.
Reason : Only those collisions in which molecules have correct
orientation and sufficient kinetic energy lead to compound
formation.
61. Assertion : Rate constants determined from Arrhenius equation are fairly
accurate for simple as well as complex molecules.
Reason : Reactant molecules undergo chemical change irrespective of
their orientation during collision.
VI. Long Answer Type
62. All energetically effective collisions do not result in a chemical change. Explain
with the help of an example.
63. What happens to most probable kinetic energy and the energy of activation
with increase in temperature?
64. Describe how does the enthalpy of reaction remain unchanged when a catalyst
is used in the reaction.
65. Explain the difference between instantaneous rate of a reaction and average
rate of a reaction.
66. With the help of an example explain what is meant by pseudo first order
reaction.
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