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 \( \frac{-E_a}{2.303R} \) and intercept is log A

Hint:

The Arrhenius equation helps determine the activation energy (E$_a$) of a reaction and explains how temperature affects reaction rates.

Answer 1

The Correct Option is D

The Arrhenius equation is given by: \[ \log k = \log A - \frac{E_a}{2.303RT} \] Comparing with the straight-line equation \( y = mx + c \), we see that: - Slope = \( \frac{-E_a}{2.303R} \) - Intercept = log A This equation describes the temperature dependence of reaction rates.