Question

In the Arrhenius equation, when \( \log k \) is plotted against \( 1/T \), a straight line is obtained whose:

• A. slope is \( \frac{A}{R} \) and intercept is \( E_a \)
• B. slope is \( A \) and intercept is \( -\frac{E_a}{R} \)
• C. slope is \( -\frac{E_a}{RT} \) and intercept is \( \log A \)
• D. slope is \( -\frac{E_a}{2.303 R} \) and intercept is \( \log A \)

Hint:

A higher activation energy (\( E_a \)) means a stronger temperature dependence of the reaction rate.

Answer 1

The Correct Option is D

Arrhenius equation: \[ \log k = \log A - \frac{E_a}{2.303RT} \] where slope \( = -\frac{E_a}{2.303 R} \) and intercept \( = \log A \).