(B) According to the collision theory,for a reaction to occur,molecules must collide with sufficient energy (activation energy) and proper orientation

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All collisions result in the formation of the products.

(B) According to the collision theory,for a reaction to occur,molecules must collide with sufficient energy (activation energy) and proper orientation. Therefore,not all collisions are effective. Only those collisions where molecules possess energy equal to or greater than the activation energy $(E_a)$ and have the correct orientation lead to product formation. Thus,statement $(B)$ is incorrect.

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

Medium

Which of the following statements is not true according to the collision theory of reaction rates?

A
Collision of molecules is a precondition for any reaction to occur.
B
All collisions result in the formation of the products.
C
Only activated collisions result in the formation of the products.
D
Molecules which have acquired the energy of activation can collide effectively.

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Class 12

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

It has been found that for a chemical reaction with a rise in temperature by $9 \, K$,the rate constant gets doubled. Assuming a reaction to be occurring at $300 \, K$,the value of activation energy is found to be $...... \, kJ \, mol^{-1}$. [nearest integer]
(Given $\ln 10 = 2.3, R = 8.3 \, J \, K^{-1} \, mol^{-1}, \log 2 = 0.30$ )

MediumJEE MAIN 2022

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In an exothermic reaction $A \to B$,the evolved heat is $280 \ kJ \ mol^{-1}$ and the activation energy is $200 \ kJ \ mol^{-1}$. The activation energy of the reverse reaction $B \to A$ is $.......... \ kJ \ mol^{-1}$.

Medium

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In the Arrhenius equation,$k = A e^{-E_a/RT}$,the Arrhenius constant $A$ will be equal to the rate constant when

Medium

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The rate constant of a reaction is $2 \times 10^{-3} \ min^{-1}$ at $300 \ K$. By increasing the temperature by $10 \ K$,its value becomes double. Calculate the energy of activation $(E_a)$ and the rate constant at $320 \ K$.

Medium

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The reaction $X \to Y$ is an exothermic reaction. The activation energy of the forward reaction $X \to Y$ is $150\,kJ\,mol^{-1}$. The enthalpy of the reaction is $-135\,kJ\,mol^{-1}$. The activation energy for the reverse reaction,$Y \to X$,will be $.......\,kJ\,mol^{-1}$.

DifficultJEE MAIN 2013

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Which of the following statements is not true according to the collision theory of reaction rates?

Similar Questions

In an exothermic reaction $A \to B$,the evolved heat is $280 \ kJ \ mol^{-1}$ and the activation energy is $200 \ kJ \ mol^{-1}$. The activation energy of the reverse reaction $B \to A$ is $.......... \ kJ \ mol^{-1}$.

In the Arrhenius equation,$k = A e^{-E_a/RT}$,the Arrhenius constant $A$ will be equal to the rate constant when

The rate constant of a reaction is $2 \times 10^{-3} \ min^{-1}$ at $300 \ K$. By increasing the temperature by $10 \ K$,its value becomes double. Calculate the energy of activation $(E_a)$ and the rate constant at $320 \ K$.

The reaction $X \to Y$ is an exothermic reaction. The activation energy of the forward reaction $X \to Y$ is $150\,kJ\,mol^{-1}$. The enthalpy of the reaction is $-135\,kJ\,mol^{-1}$. The activation energy for the reverse reaction,$Y \to X$,will be $.......\,kJ\,mol^{-1}$.

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