Question

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]

The initial concentration of N₂O₅ in the first order reaction : N₂O₅(g) → 2NO₂(g) + ½O₂(g) was 1·2 × 10⁻² mol L⁻¹. The concentration of N₂O₅ after 60 minutes was 0·2 × 10⁻² mol L⁻¹. Calculate the rate constant of the reaction at 318 K. [log 6 = 0·778]