Chemical Kinetics involve the study of the rates of chemical reactions. The study includes the reaction pathways and the mechanism of the reaction. The factors that affect the rate of a reaction, the effect of change of concentration on the rate of the reaction and the order of the reaction are also studied well in this chapter.
Download Class 12 Chemistry Worksheet on Chapter 4 Chemical Kinetics Set 5 PDF.
CBSE Class 12 Chemistry Chapter 4 Chemical Kinetics Worksheet – Set 5
Q-1: The rate of a reaction can be maintained the same by:
a.) continuously stirring the compounds
b.) keeping the temperature of the reaction constant
c.) both (a.) and (b.)
d.) None of the above
Q-2: Consider the reaction:
2A + B → A2B
A will disappear at_____.
a.) half the rate at which B will decrease
b.) the same rate at which B will decrease
c.) the same rate at which A2B will form
d.) twice the rate at which B will decrease
Q-3: Does molecularity have any significance for the complex reactions?
Q-4: 2A → B + C would be a zero order reaction when ____.
a.) the rate is doubled as [B] is doubled
b.) the rate remains constant and independent of [B] and [C]
c.) the rate does not change with any change in [A]
d.) the rate is proportional to [A]2
Q-5: Can the value of activation energy for a reaction be negative?
Q-6: The rate constant for a reaction is constant and depends on_____.
a.) the temperature
b.) time
c.) mass
d.) weight
Q-7: Given that the temperature coefficient of a reaction is 2, calculate the increase in the rate when the temperature rises by 100 oC.
Q-8: Consider the reaction: NO2 (g) + CO (g) → CO2 (g) + NO (g)
The experimentally determined rate law expression for the given reaction is: Rate = k[NO2]2
Propose the mechanism of this reaction.
Q-9: The rate constant of a reaction when the activation energy is zero:
a.) increases with an increase in the temperature
b.) decreases with a decrease in the temperature
c.) is independent of the temperature
d.) decreases with an increase in the temperature
Q-10: Determine whether the following reaction is true or false.
The activation energy required for a slow reaction is less in comparison to that required for the fast reactions.
Q-11: Considering the given rate expression of a reaction, determine whether this reaction can be an elementary reaction.
Q-12: State one condition under which a second order bimolecular reaction may start behaving like a first order reaction kinetically.
Q-13: Justify the statement: the initial concentration of the reactant determines the half-life of a zero order reaction.
Q-14: Determine the order of a reaction, the unit of whose rate constant is equal to that of the rate of the reaction.
Q-15: Match the following:
| Column I | Column II | ||
|---|---|---|---|
| a. | Arrhenius equation | (i) | t1/2 = 0.693 / k |
| b. | Half life of first order reaction | (ii) | a / 2k |
| c. | Δ[A] / Δt | (iii) | k = Ae-Ea/RT |
| d. | Half life of zero order equation | (iv) | Average rate of the reaction |
Q-16: Write a few points that determine the failure of the Collision theory.
Q-17: State whether the given statements are true or false.
(a.) The rate of reaction increases with an increase in its activation energy.
(b.) The average and the instantaneous rates of a reaction are the same.
Q-18: The rate law for the reaction A + B → Products is: r = k[A]½[B]2. Determine the order of the reaction.
Q-19: The first order decomposition reaction of SO2Cl2 takes 60 minutes for the decomposition of half of its initial amount. Calculate the rate constant for the reaction.
Q-20: A reaction is first order in terms of A and second order in terms of B. Determine the change in rate of the reaction when the concentration of B is increased three times.
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