Question

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

The rate constant of a reaction quadruples when the temperature changes from 300 K to 320 K. Calculate the activation energy for this reaction. [log 2 = 0.30, log 4 = 0.60, 2.303 R = 19.15 J K⁻¹mol⁻¹]

A first order reaction is 50% complete in 30 minutes at 300 K and in 10 minutes at 320 K. Calculate activation energy (Ea) for the reaction. [R = 8.314 J K⁻¹ mol⁻¹] [Given : log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021]

The rate constant for the first order decomposition of N₂O₅ is given by the following equation : log k = 23·6 − (2×10⁴ K)/T Calculate Ea for this reaction. [R = 8·314 J K⁻¹ mol⁻¹]