Question

The Arrhenius equation is, $k=A{e}^{-E_a/RT}$.
If the activation energy of the reaction is found to be equal to $RT$, then:

• A. the rate of reaction does not depend upon initial concentration
• B. the rate constant becomes about $37$% of the Arrhenius constant $A$
• C. the rate constant becomes equal to $73$% of the Arrhenius constant $A$
• D. the rate of the reaction becomes infinite or zero

Answer 1

The correct option is B the rate constant becomes about $37$% of the Arrhenius constant $A$

$k=A_e^{-E_a/RT}$

when $E_a=RT$, $k=\frac{A}{e}=0.37\times A=\frac{37}{100}\times A$

Hence rate constant becomes $37\%$ of A.