(B) According to the collision theory,the rate of a reaction is directly proportional to the number of collisions per unit time (collision frequency).

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Rate is directly proportional to the number of collisions per second.

(B) According to the collision theory,the rate of a reaction is directly proportional to the number of collisions per unit time (collision frequency). An increase in collision frequency leads to an increase in the number of effective collisions,thereby increasing the rate of the reaction.

Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

Medium

According to the collision theory of chemical reactions:

A
$A$ chemical reaction occurs with every molecular collision.
B
Rate is directly proportional to the number of collisions per second.
C
Reactions in the gas phase are always of zero order.
D
Reaction rates are of the order of molecular speeds.

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Class 12 Questions

Class 12

Chemistry Questions

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

The activation energy for the reaction $X \rightarrow Y$ is $150 \text{ kJ mol}^{-1}$. The change in enthalpy for the above reaction is $-135 \text{ kJ mol}^{-1}$. What is the activation energy for the reverse reaction $Y \rightarrow X$?

DifficultKCET 2026

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The temperature coefficient of a reaction is $2$. When the temperature is increased from $30^{\circ} C$ to $90^{\circ} C$,the rate of reaction is increased by: (in $\times$)

DifficultKCET 2013

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Find True $(T)$ and False $(F)$ statements in the following:
$1.$ Effective collision depends on rate.
$2.$ When the reactant converts into product,the bonds in the reactant break and new bonds form.
$3.$ The breaking of old bonds and the formation of new bonds take place simultaneously.

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The activation energy for the forward reaction is $150 \ kJ \ mol^{-1}$ and that of the reverse reaction is $260 \ kJ \ mol^{-1}$. The enthalpy change for the reaction is:

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In the Arrhenius plot of $\log_{10} k$ versus $1 / T$,find the value of the intercept on the $y$-axis.

MediumMHT CET 2024

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According to the collision theory of chemical reactions:

Similar Questions

The activation energy for the reaction $X \rightarrow Y$ is $150 \text{ kJ mol}^{-1}$. The change in enthalpy for the above reaction is $-135 \text{ kJ mol}^{-1}$. What is the activation energy for the reverse reaction $Y \rightarrow X$?

The temperature coefficient of a reaction is $2$. When the temperature is increased from $30^{\circ} C$ to $90^{\circ} C$,the rate of reaction is increased by: (in $\times$)

Find True $(T)$ and False $(F)$ statements in the following:$1.$ Effective collision depends on rate.$2.$ When the reactant converts into product,the bonds in the reactant break and new bonds form.$3.$ The breaking of old bonds and the formation of new bonds take place simultaneously.

The activation energy for the forward reaction is $150 \ kJ \ mol^{-1}$ and that of the reverse reaction is $260 \ kJ \ mol^{-1}$. The enthalpy change for the reaction is:

In the Arrhenius plot of $\log_{10} k$ versus $1 / T$,find the value of the intercept on the $y$-axis.

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Find True $(T)$ and False $(F)$ statements in the following:
$1.$ Effective collision depends on rate.
$2.$ When the reactant converts into product,the bonds in the reactant break and new bonds form.
$3.$ The breaking of old bonds and the formation of new bonds take place simultaneously.