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Question

(C) According to the collision theory,for a reaction to occur,colliding molecules must possess kinetic energy at least equal to the activation energy

Vedclass · Accepted Answer

$A$ larger fraction of molecules possess energy greater than the activation energy.

Vedclass · Answer

(C) According to the collision theory,for a reaction to occur,colliding molecules must possess kinetic energy at least equal to the activation energy $(E_a)$.At higher temperatures,the distribution of kinetic energy shifts such that a larger fraction of molecules have energy $\ge E_a$.This leads to an increase in the number of effective collisions,thereby increasing the rate of reaction.Additionally,as per the Arrhenius equation,$k = Ae^{-E_a/RT}$,the rate constant $k$ increases exponentially with temperature.

Why does the rate of a reaction increase with a rise in temperature?

Similar Questions

The time required for $10 \%$ completion of a first order reaction at $298 \,K$ is equal to that required for its $25 \%$ completion at $308 \,K$. If the value of $A$ is $4 \times 10^{10} \,s^{-1}$,calculate $k$ at $318 \,K$ and $E_a$.

What is the value of the slope of the plot $\ln K$ versus $\frac{1}{T}$ for a reaction having $E_{a} = 33.256 \ J \ mol^{-1}$?

Assertion : According to transition state theory for the formation of an activated complex,one of the vibrational degrees of freedom is converted into a translational degree of freedom.
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At $298 \text{ K}$ temperature,the activation energy for the reaction $x_2 + y_2 \rightarrow 2xy + 20 \text{ kJ}$ is $15 \text{ kJ}$. What will be the activation energy for the reaction $2xy \rightarrow x_2 + y_2$?

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