Question

The rates of chemical reactions are strongly affected by temperature. Arrhenius (1889) gave following relation between rate constant and temperature:

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

This equation is called Arrhenius equation. The constant '$A$' is called Arrhenius constant or pre-exponential factor.

The logarithm of Arrhenius equation is:

${\log }_{10}k={\log }_{10}A-\frac{E_a}{2.303RT}$

This equation for a reaction is:

${\log }_{10}k=14-\frac{1.25\times {10}^{4}K}{T}$

Energy of activation in $k$$cal$ ${mol}^{-1}$ is:

• A. $14$ $k$$cal$ ${mol}^{-1}$
• B. $57.6$ $k$$cal$ ${mol}^{-1}$
• C. $1.25\times {10}^4$ $k$$cal$ ${mol}^{-1}$
• D. $\frac{14}{1.25\times {10}^4}$ $k$$cal$ ${mol}^{-1}$

Answer 1

The correct option is B $57.6$ $k$$cal$ ${mol}^{-1}$