(C) For a chemical reaction to occur,the reactant molecules must collide with each other.However,not all collisions lead to the formation of products.

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(C) For a chemical reaction to occur,the reactant molecules must collide with each other.However,not all collisions lead to the formation of products.Only those collisions where the colliding molecules possess a minimum amount of energy,known as the $Threshold \ energy$,result in a chemical reaction.Therefore,the minimum energy required for an effective collision is the $Threshold \ energy$.

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

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The minimum energy that reactant molecules must possess at the time of collision for an effective collision is called ...

A
Bond dissociation energy
B
Chemical energy
C
Threshold energy
D
Activation energy

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Class 12 Questions

Class 12

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

For an endothermic reaction,$\Delta H$ represents the enthalpy of the reaction in $kJ \ mol^{-1}$. The minimum amount of activation energy will be

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The Arrhenius plots of two reactions,$I$ and $II$ are shown graphically. The graph suggests that

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What is the activation energy $(kJ \, mol^{-1})$ for a reaction if its rate constant doubles when the temperature is raised from $300 \, K$ to $400 \, K$ ? $(R = 8.314 \, J \, mol^{-1} \, K^{-1})$

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The reaction between $H_{2(g)}$ and $O_{2(g)}$ is highly feasible,yet allowing the gases to stand at room temperature in the same vessel does not lead to the formation of water. Explain.

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For an effective collision to occur,the colliding molecules must possess:

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The minimum energy that reactant molecules must possess at the time of collision for an effective collision is called ...

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For an endothermic reaction,$\Delta H$ represents the enthalpy of the reaction in $kJ \ mol^{-1}$. The minimum amount of activation energy will be

The Arrhenius plots of two reactions,$I$ and $II$ are shown graphically. The graph suggests that

What is the activation energy $(kJ \, mol^{-1})$ for a reaction if its rate constant doubles when the temperature is raised from $300 \, K$ to $400 \, K$ ? $(R = 8.314 \, J \, mol^{-1} \, K^{-1})$

The reaction between $H_{2(g)}$ and $O_{2(g)}$ is highly feasible,yet allowing the gases to stand at room temperature in the same vessel does not lead to the formation of water. Explain.

For an effective collision to occur,the colliding molecules must possess:

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