The standard free energy of activation of a reaction A is Reaction B is ten million times faster than reaction A at the same temperature. The products of each reaction are 10.0 kJ mol-1 (2.39 kcal mol-1) more stable than the reactants. (a) What is the standard free energy of activation of reaction B

Eb = 7.7 kJ/mol

Explanation:

The formula for determining the rate of change of reaction based on the activation energies of the reactants is given as;

Log (k1 / k2) = (Eb - E a) / (2.3 x R x T)

Here, K1 is the rate of reaction of A; K2 the rate of reaction of B

Eb is the activation energy of B

Ea is the activation energy of A

R, real gas constant and T is the temperature.

As per given information, putting the values in above formula;

log (1/10,000,000) = Eb - 83.7 kJ/mol / 2.3 (0.008314 kJ/K mol) (298K)

-7 = Eb - 83.7 kJ/mol / 5.69 kJ/mol

Eb = - 7 + 14.7

Eb = 7.7 kJ/mol