The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy $\left( E_{a} \right)$ of the reaction?

Question

Dr. Abubacker · Accepted Answer

(b)
At $T_{1} = 200\ K,\ T_{2} = 400\ K,\ k_{1} = k,\ \ k_{2} = 10\ k$
$\because\log\frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303R}\ \left( \frac{T_{2} - T_{1}}{T_{1}\  \bullet T_{2}} ight)$
$\log\frac{10\ k}{k} = \frac{E_{a}}{2.303R}\ \left( \frac{400 - 200}{400 	imes 200} ight)$
$E_{a} = 921.2\ R$

Q. The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy $\left( E_{a} \right)$ of the reaction?

Explanation

Reviewed by Dr. Abubacker

Want more practice?