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:

In the Arrhenius equation, the slope of the plot of \(\log k\) vs. \(1/T\) is directly related to the activation energy (\(E_a\)) of the reaction.

Answer 1

The Correct Option is D

The Arrhenius equation is given by: \[ \log k = \frac{-E_a}{2.303R} \cdot \frac{1}{T} + \log A \] where the slope is \(\frac{-E_a}{2.303R}\) and the intercept is log A. This linear relationship is used to determine the activation energy and pre-exponential factor from experimental data.