Question

The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. Calculate the energy of activation of the reaction, assuming that it does not change with temperature. (log 2 = 0·30, log 4 = 0·60) [R = 8·314 J K⁻¹ mol⁻¹]

The rate constant of a first order reaction increases from 2 × 10⁻² s⁻¹ to 4 × 10⁻² s⁻¹ when the temperature changes from 300 K to 310 K. Calculate the energy of activation (Ea). [log 2 = 0·3010, log 3 = 0·4771, log 4 = 0·6021] [2·303 R = 19·15 JK⁻¹ mol⁻¹]

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]

A certain reaction is 50% complete in 20 minutes at 300 K and the same reaction is 50% complete in 5 minutes at 350 K. Calculate the activation energy if it is a first order reaction. [R = 8.314 J K⁻¹ mol⁻¹; log 4 = 0.602]