The standard free energy of activation of a reaction A is 90 kJ mol-1 (21.5 kcal mol-1) at 298 K. Reaction B is one million times faster than reaction A at the same temperature. The products of each reaction are 10 kJ mol-1 (2.4 kcal mol-1) more stable than the reactants.
(a) What is the standard free energy of activation of reaction B?
(b) Draw reaction free-energy diagrams for the two reactions showing the two values of ∆G°* to scale.
(c) What is the standard free energy of activation of the reverse reaction in each case?