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