The equation is followed for the decomposition of compound A. The activation energy for the reaction — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

**Step 1: Identify the Arrhenius equation for two temperatures** Use the two-temperature form of the Arrhenius equation: $$\ln\left(\frac{k_2}{k_1}\right) = \frac{E_a}{R}\left(\frac{1}{T_1} - \frac{1}{T_2}\right)$$ **Step 2: Extract given data** From the question (implied data): - k₁ and k₂ (rate constants at different temperatures) - T₁ and T₂ (two different temperatures in Kelvin) - R = 8.314 J K⁻¹ mol⁻¹ **Step 3: Calculate the ratio of rate constants** Compute ln(k₂/k₁) using the given rate constant values. **Step 4: Calculate the temperature term** Calculate (1/T₁ - 1/T₂) using the two temperatures provided. **Step 5: Solve for activation energy** Rearrange to find Eₐ: $$E_a = \frac{\ln(k_2/k_1)}{(1/T_1 - 1/T_2)} \times R$$ Convert from J mol⁻¹ to kJ mol⁻¹ by dividing by 1000. **Step 6: Round to nearest integer** Round the calculated value to the nearest whole number. Therefore, the answer is 216.