(B) The fraction of molecules $(f)$ having energy equal to or greater than the activation energy $(E_a)$ is given by the Arrhenius equation: $f = e^{-

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(B) The fraction of molecules $(f)$ having energy equal to or greater than the activation energy $(E_a)$ is given by the Arrhenius equation: $f = e^{-E_a/RT}$.Given:$E_a = 200 \ kJ \ mol^{-1} = 200,000 \ J \ mol^{-1}$$R = 8.314 \ J \ K^{-1} \ mol^{-1}$$T = 600 \ K$Substituting the values:$f = e^{-(200,000) / (8.314 \times 600)}$$f = e^{-(200,000) / (4988.4)}$$f \approx e^{-40.09} \approx e^{-40}$.

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

Medium

The activation energy for the reaction $2HI_{(g)} \to H_{2_{(g)}} + I_{2_{(g)}}$ is $200 \ kJ \ mol^{-1}$ at $600 \ K$. Calculate the fraction of molecules of reactant having energy equal to or greater than activation energy.

A
$e^{-30}$
B
$e^{-40}$
C
$e^{-2.5}$
D
$e^{-1/3}$

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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The activation energy for the reaction $2HI_{(g)} \to H_{2_{(g)}} + I_{2_{(g)}}$ is $200 \ kJ \ mol^{-1}$ at $600 \ K$. Calculate the fraction of molecules of reactant having energy equal to or greater than activation energy.

Similar Questions

For a reaction where the activation energies of the forward and reverse directions are equal in value,then:

The rate constant is doubled when temperature increases from $27^{\circ} C$ to $37^{\circ} C$. What is the activation energy in $kJ \ mol^{-1}$?

The activation energy of a reaction is zero. Its rate constant at $280 \ K$ is $1.6 \times 10^{-6} \ s^{-1}$,the rate constant at $300 \ K$ is

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