QJEEM22Ch180c: JEE Main 2022 Chemistry - Class 12 JEEM22Ch180c Solution: Catalyst A reduces the activation energy for a reaction by 10…

Activation Energy : It is the minimum amount of energy required to activate the molecules/ atoms so that they can undergo the chemical reaction.

A catalyst increases the rate of a reaction by lowering the activation energy so that more reactant molecules collide with enough energy to surmount the smaller energy barrier.

In the Question,

Given : $\mathrm{E}_{\text {cat }}-\mathrm{E}_{\text {uncat }}=10 \mathrm{~kJ} / \mathrm{mol}$

$\mathrm{T}=300 \mathrm{~K}$

According to Arrhenius Equation,

$\begin{aligned}& \mathrm{K}=A \mathrm{e}^{-\mathrm{Ea} / \mathrm{RT}} \\\\& \frac{\mathrm{E}_{\text {cat }}}{\mathrm{E}_{\text {uncat }}}=e^{\frac{E a-E_a^1}{R T}}\end{aligned}$

$\begin{aligned}& =e^{\frac{10 \times 10^3}{8.21 \times 300}} \\\\& =e^4 \\\\& =4\end{aligned}$