List of top Chemistry Questions on Chemical Kinetics asked in CBSE CLASS XII

The rate for the following reaction is given by: \[ A + B \rightarrow C, \quad \text{Rate} = k[A][B]^2 \] How is the rate affected if we double the concentration of B?

For a reaction : $ N_2 + 3H_2 \rightarrow 2NH_3 $, the rate of reaction with respect to $ NH_3 $ is

Following reaction takes place in one step :
$ 2A + B \rightarrow 2C $
How will the rate of above reaction change if the volume of the reaction vessel is decreased to one third of its original volume? Will there be any change in the order of reaction with the reduced volume?

Half-life ($ t_{1/2} $) of a first order reaction is 1386 s. The value of rate constant is:

For the first order thermal decomposition reaction, following data was obtained : Calculate rate constant.
[Given : log 3 = 0.48]

Which of the following curve represents the first order reaction?

Rate constant $k$ for the first order reaction is $2.54 \times 10^{-3} \text{ s}^{-1}$. Calculate the time required for three-fourth of the reactant to decompose. ($\log 4 = 0.60$)

The concentration of the reactant is reduced from $0.6 \text{ mol L}^{-1}$ to $0.2 \text{ mol L}^{-1}$ in 5 minutes in a first order reaction. Calculate rate constant of the reaction. ($\log 3 = 0.48$)

Write the unit of (i) second order reaction and (ii) zero order reaction.

Define Effective collision.

Assertion (A): The molecularity of the given reaction is 2. \[ 2\text{HI} \rightarrow \text{H}_2 + \text{I}_2 \] Reason (R): Two molecules of the reactants are involved in simultaneous collision between them. Choose the correct option:

The order for the given reaction is: \[ \text{A} + 2\text{B} \rightarrow \text{Products} \] \[ \text{Rate} = k[\text{A}]^{1/2}[\text{B}]^{1} \]

Identify the correct statement:

The rate of a chemical reaction doubles when the temperature is raised from 298 K to 308 K. Calculate the activation energy ($E_a$) for this reaction assuming it does not change with temperature. (Given: $ R = 8.314 \, \text{J mol}^{-1}\text{K}^{-1} $, $ \log 2 = 0.30 $)

Write the overall order of a reaction if A is present in large excess.

Define order of a reaction.

Observe the graph in the given figure and answer the following questions:

linear relationship between log |R0| and time.

(a) Predict the order of reaction.
(b) What is the slope of the curve?

Reactant ‘A’ underwent a decomposition reaction. The concentration of ‘A’ was measured periodically and recorded in the table given below:

Based on the above data, predict the order of the reaction and write the expression for the rate law.

(ii) Account for the following:
(I) We cannot determine the order of a reaction by taking into consideration the balanced chemical equation.
(II) A bimolecular reaction may become kinetically first order under a specified condition.

Assertion (A): In a first order reaction, if the concentration of the reactant is doubled, its half-life is also doubled.
Reason (R): The half-life of a reaction does not depend upon the initial concentration of the reactant in a first order reaction.

The number of molecules that react with each other in an elementary reaction is a measure of the:

Which of the following is the slope of the first order reaction in the plot of ln[R] vs. time ?

Unit of rate constant ‘k’ for a second order reaction is:

Assertion (A): Actinoids show wide range of oxidation states.
Reason (R): Actinoids are radioactive in nature.