(B) For a $10 \ K$ rise in temperature,the collision frequency increases only by about $1 \%$ to $2 \%$. However,the fraction of molecules possessing

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fraction of molecules possessing threshold energy increases by a factor of $2$ to $3$

(B) For a $10 \ K$ rise in temperature,the collision frequency increases only by about $1 \%$ to $2 \%$. However,the fraction of molecules possessing energy equal to or greater than the threshold energy increases significantly,typically by a factor of $2$ to $3$. This leads to a doubling or tripling of the rate constant.

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

Medium

In most cases,for a rise of $10 \ K$ temperature,the rate constant is doubled or tripled. This is due to the reason that

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A
collision frequency increases by a factor of $2$ to $3$
B
fraction of molecules possessing threshold energy increases by a factor of $2$ to $3$
C
Activation energy is lowered by a factor of $2$ to $3$
D
none of these

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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The rate of a first order reaction doubles when the temperature changes from $300 \ K$ to $310 \ K$. The activation energy of the reaction (in $kJ \ mol^{-1}$) is
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In most cases,for a rise of $10 \ K$ temperature,the rate constant is doubled or tripled. This is due to the reason that

Similar Questions

The rate of a certain biochemical reaction at physiological temperature $T$ occurs $10^{6}$ times faster with an enzyme than without. The change in the activation energy upon adding the enzyme is

The equilibrium constant at $27\,^{\circ}C$ and $127\,^{\circ}C$ is $30$ and $40$ respectively. What will be the ratio of activation energy $(E_{a})_{f} / (E_{a})_{b}$?

In a reaction,the rate of reaction doubles with a $10^\circ C$ rise in temperature. If the temperature is increased from $10^\circ C$ to $100^\circ C$,by how many times will the rate of reaction increase?

Choose the incorrect statement -

The rate of a first order reaction doubles when the temperature changes from $300 \ K$ to $310 \ K$. The activation energy of the reaction (in $kJ \ mol^{-1}$) is$R=8.3 \ J \ K^{-1} \ mol^{-1}, \log 2=0.3$ (in $.33$)

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The rate of a first order reaction doubles when the temperature changes from $300 \ K$ to $310 \ K$. The activation energy of the reaction (in $kJ \ mol^{-1}$) is
$R=8.3 \ J \ K^{-1} \ mol^{-1}, \log 2=0.3$ (in $.33$)