Question

The rate of a reaction quadruples when temperature changes from 27°c to 57°c. Calculate the energy of activation
Given R=8.314 J K-1 mol-1, log 4=0.6021

• A. 38.04 KJ/mol
• B. 380.4 KJ/mol
• C. 3.80 KJ/mol
• D. 3804 KJ/mol

Answer 1

The Correct Option is A

Step 1: Use Arrhenius equation:

$\ln\left(\frac{k_2}{k_1}\right) = \frac{E_a}{R}\left(\frac{T_2 - T_1}{T_1T_2}\right)$

Step 2: Plug values:

$\ln 4 = \frac{E_a}{8.314} \times \frac{30}{300 \times 330}$

$E_a = 38.04 \, kJ/mol$