Consider the given plots for a reaction obeying Arrhenius equation
Question:

Consider the given plots for a reaction obeying Arrhenius equation $\left(\begin{array}{lll}0 & \left.{ }^{\circ} \mathrm{C}<\mathrm{T}<300{ }^{\circ} \mathrm{C}\right) \text { : }\end{array}\right.$ ( $\mathrm{K}$ and $\mathrm{E}_{\mathrm{a}}$ are rate constant and activation energy, respectively)

Choose the correct option:

1. I is right but II is wrong

2. Both I and II are correct

3. I is wrong but II is right

4. Both I and II are wrong.

Correct Option: , 2

Solution:

From Arrhenius equation,

$K=A e^{-E_{a} / R T}$

So, as $\mathrm{E}_{\mathrm{a}}$ increases, $e^{-E_{a} / R T}$ decreases, $K$ decreases

and as T increases, $\frac{E_{a}}{R T}$ decreases, $e^{-E_{a} / R T}$ increases,