(C) According to collision theory,for a reaction to occur,molecules must collide with both sufficient kinetic energy (activation energy) and the corre

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The collision of the reactant molecules should be from any direction.

(C) According to collision theory,for a reaction to occur,molecules must collide with both sufficient kinetic energy (activation energy) and the correct orientation (steric factor). Option $C$ is incorrect because collisions must occur with a specific,favorable orientation to be effective; they cannot be from any random direction.

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

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Which statement is incorrect for collision theory?

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A
The reactant experiencing fruitful collisions are converted to products.
B
There must be a certain minimum energy for the reactant experiencing collision.
C
The collision of the reactant molecules should be from any direction.
D
The collision between the reacting molecules is essential.

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Class 12

Chemistry Questions

Chapter

Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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For an exothermic reaction $A \rightarrow B$,the activation energy is $15 \, K \, cal/mol$ and the heat of reaction is $5 \, K \, cal/mol$. The activation energy for the reverse reaction $B \rightarrow A$ will be ......... $K \, cal/mol$.

Medium

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$A$ catalyst:

MediumAIPMT 1995

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The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

Easy

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The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^/RT}$. The activation energy $(E^)$ of the reaction can be calculated by plotting:

DifficultAIPMT 2003

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The rate of the chemical reaction doubles for an increase of $10 \text{ K}$ in absolute temperature from $298 \text{ K}$. What will be the activation energy?

DifficultGUJCET 2026

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Which statement is incorrect for collision theory?

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For an exothermic reaction $A \rightarrow B$,the activation energy is $15 \, K \, cal/mol$ and the heat of reaction is $5 \, K \, cal/mol$. The activation energy for the reverse reaction $B \rightarrow A$ will be ......... $K \, cal/mol$.

$A$ catalyst:

The variation of the rate constant with temperature is given by the Arrhenius equation $k = A e^{-E_a / (RT)}$. If $T \to \infty$,the rate constant $k$ will be equal to:

The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^*/RT}$. The activation energy $(E^*)$ of the reaction can be calculated by plotting:

The rate of the chemical reaction doubles for an increase of $10 \text{ K}$ in absolute temperature from $298 \text{ K}$. What will be the activation energy?

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The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^/RT}$. The activation energy $(E^)$ of the reaction can be calculated by plotting: