Chemistry 1st Year Chapter 11 Reaction Kinetics Notes MCQs Bank

chemistry 11th notes chapter 11

1. The unit of the rate constant of a second-order reaction is:


2. The rate of reaction between two specific time intervals is called:


3. Which one of the following is not a characteristic of a catalyst:


4. If the rate of decay of radio-active isotope decreases from 200 cpm to 25 cpm after 24 hours. What is its half life:


5. The specific rate constant of a chemical reaction is the rate of the reaction when the concentration of the reactant is:


6. A catalyst can:


7. The half life of zero order reaction is:


8. The 2nd order reaction becomes 1st when:


9. The rate of reaction is doubled for every 10°C rise in temperature. The increase in reaction rate as a result of temperature rise from 10°C to 100°C is:


10. The activation energy of reaction:


11. For the 1st order decomposition reaction 2N₂O₅ (g) → 4NO₂(g) + O₂(g) the half-life is given as:


12. The unit of rate constant K for a first order reaction:


13. The change in concentration of reactants or products per unit time is called:


14. If 75% of any given amount of radioactive element disintegrates in 60 min. The half life of a radioactive element is.


15. In a multistep reaction, the slowest step is:


16. The unit of rate constant “K” is mol.dm³.sec⁻¹ for a chemical reaction the order of reaction is:


17. The rate expression for a reaction A+B → products is rate = k [A]2/3 [B]-1/2 the order of reaction is:


18. The slope of the curve between 1/T and log k gives:


19. The mathematical relation between the rate of reaction and the concentrations of the reactants is known as the:


20. Oxidation of SO₂(g) in the presence of NO(g) catalyst is an example of:


21. Which technique is used to determine the absorption of radiations:


22. Enzymes are:


23. The unit of rate constant depends on?


24. Photosynthesis has order of reaction:


25. For a chemical reaction to occur:


26. Rate = Ka₂[B] for the reaction 2A + B —> Product and ‘A’ is present in large excess, then order of reaction is:


27. The unit of the rate constant is the same as that of the rate of reaction in:


28. When rate of reaction is retarded by adding a substance, it is said to be:


29. The reaction that involves gases, its rate does not depend upon?


30. Which one affects the specific rate constant?


31. The half-life period of the zero-order reaction is equal to:


32. The influence of temperature on the reaction rate is predicted by:


33. A substance which itself is not a catalyst but increases the activity of a catalyst is called:


34. When the concentration of a reactant in the reaction is increased by 8 times, the rate increased only by 2 times. The order of the reaction is:


35. Which property of a liquid is measured by polarimeter:


36. Which one is a chemical method for the determination of the rate of reaction?


37. Which of the following statements regarding a catalyst is not true?


38. Which one of the following is correct about the following reaction if the iron is not 100% pure?
2Fe + 3H₂O + O₂ → Fe₂O₃.3H₂O


39. Arrhenius equation can be used for evaluating:


40. Which types of metals are usually used as catalyst:


41. The rate equation for a reaction is Rate = KIM, what are the units of K:


42. Oxidation of SO₂(g) in the presence of V₂O₅(s) is an example of:


43. An endothermic reaction A → B has an activation energy 15kcal /mol and the heat of reaction 5kcal/mol. The activation energy for the reaction B → A will be:


44. If the energy of the activated complex lies close to the energy of reactants, it means that reaction is:


45. The half life for a 1st order decomposition of a substance dissolved in CCl₄ is 2.5 hours at 30°C. The amount of substance left after 10 hours if the initial weight of the substance is 160g:


Short Questions

1. 50% of a hypothetical first order reaction completes in one hour. The remaining 50% needs more than one hour to convert itself into products?
2. A finally divided catalyst may prove to be more effective. Give reasons?
3. A particular catalyst is suitable for a particular chemical reaction. Give examples?
4. Activation energy is the minimum amount of energy more than the average energy which is just sufficient is convert reactants into products?
5. Define order of reaction with the help of an example?
6. Differentiate between average and instantaneous rate of reaction?
7. How does a catalyst chemically remain the same at the end of the chemical reaction?
8. How does a catalyst effect the reversible chemical reactions and their energy of activation?
9. How does the increase of temperature increases the rate of the chemical reactions?
10. How the energy of activation can be calculated from the Arrhenius plots?
11. How the enzymes act as catalyst?
12. How the half life periods and initial concentrations are related to give the order of reaction?
13. How the half life periods of the chemical reactions are related with the initial concentrations of the reactants for first, second and third order reactions?
14. How the mechanism of a chemical reaction can help to point out the rate determining step?
15. How the rate of reaction is affected by surface area?
16. How the reactions of fractional order can be studied by the method of half life periods?
17. How the temperature is related with the rate constant?
18. The order of a reaction is obtained from the rate expression of a reaction and the rate expression is obtained from the experiments?
19. The radioactive decay is always a first order reaction. How?
20. The rate of a chemical reaction is an ever changing parameter under the given conditions. Comment upon the statement?
21. The reaction rate decreases every moment but the rate constant ‘K’ of the reaction is a constant quantity, under the given conditions. Justify it?
22. The reactions happen due t⁰Collisions among the molecules, but all the collisions are not fruitful. Justify it?
23. The sum of the coefficient of a balanced chemical equation is not necessarily important to give the order of reaction. Justify it?
24. The units of “rate constant “of second order reaction reaction is dm³, mol⁻¹, sec⁻¹, but the unit of “rate of reaction” is mol. Dm⁻³ Justify it?
25. What are the controlling factors on the activity of the enzyme?
26. What do you mean by autocatalysis?
27. What is catalytic poisoning? Give two examples of catalytic poisoning.
28. What is order of a reaction? When the reactions become zero order?
29. What is promoter or activator?
30. What is temperature coefficient of a reaction?
31. What is the effect of light on the rate of reaction?
32. What is the effect of temperature on the activation energy of a reaction?
33. What type of information is obtained for the order of reaction from half life period of that reaction?
34. Why the reactions having lower energies of activation have faster rates?

Long Questions

1. How will you find the order of reaction by half-life method?
2. How Arrhenius equation explains the effect of temperature on the rate constant of a reaction?
3. What is energy of activation? Discuss collision theory.
4. What is enzyme catalysis? Give an example & give four characteristics of enzyme catalysis.
5. What is catalysis? Write down its types and explain any one of them.
6. Explain Half-life method for the Determination of order of Reaction.
7. Give four characteristics of enzyme catalysis.
8. Write a note on (i) Homogeneous catalysis (ii) Heterogeneous catalysis
9. Write a detailed note on determination of rate of reaction by chemical method.
10. How does Arrhenius equation help us to calculate the energy of activation of a reaction?
11. What is catalyst? Write its three characteristics.
12. A catalyst is required in small amount. Why?
13. What are pseudo first order reactions? Give example.
14. Some reaction taking place around room temperature have activation energies around 50 kJ mol⁻¹. What is the value of the factor at 25°C, 35°C and 45°C?
15. How arrhenius equation explains the effect of temperature on the rate constant of a reaction?
16. In the reaction of NO and H₂, it was observed that equimolecular mixture of gases at 340.5 mm pressure was half changed in 102 seconds. In another experiment with an initial pressure of 288 mm of Hg, the reaction was half completed in 140 seconds. Calculate the order of reaction.
17. How will you find the order of reaction by half life method.
18. Explain second and third order reactions with examples?
19. Define the following terms with examples. (I) Catalyst for a catalyst (ii) Negative catalysis (iii) Autocatalysis
20. How rate of a reaction can be determined? Explain with example

Leave a Reply

Your email address will not be published. Required fields are marked *