Question

The activation energy for a reaction at the temperature $T$ K was found to be 2.303 RT $J/mo{l}^{-1}$. The ratio of the rate constant to the Arrhenius factor is:

• A. ${10}^{-1}$
• B. ${10}^{-2}$
• C. $2\times {10}^{-3}$
• D. $2\times {10}^{-2}$

Answer 1

Answer: (A)

${10}^{-1}$

Arrhenius equation is,

rate constant, $k=A{e}^{-E_a/RT}$

$k=A{e}^{-2.303RT/RT}\Rightarrow \frac{k}{A}=e^{-2.303}$

On solving, we get

$\frac{k}{A}={10}^{-1}$

Hence, the correct option is $\text{A}$