A reaction with an equilibrium constant of 2.00 × 10^–5 is conducted at 25°C. To increase the equilibrium constant by a factor of 100, what is the required change in each of the following?
(i) ΔG°
(ii) ΔH°, if ΔS° = 0
(iii) ΔS°, if ΔH° = 0

(i) The ΔG° must decrease by 2.73 kcal/mol.

(ii) The ΔH° must decrease by 2.73 kcal/mol.

(iii) The ΔS° must increase by 9.16×10^–3 kcal/mol∙K.

(i) The ΔG° must increase by 2.73 kcal/mol.

(ii) The ΔH° must increase by 2.73 kcal/mol.

(iii) The ΔS° must decrease by 9.16×10^–3 kcal/mol∙K.

(i) The ΔG° must decrease by 10.1 kcal/mol.

(ii) The ΔH° must decrease by 10.1 kcal/mol.

(iii) The ΔS° must increase by 3.38×10^–2 kcal/mol∙K.

(i) The ΔG° must increase by 10.1 kcal/mol.

(ii) The ΔH° must increase by 10.1 kcal/mol.

(iii) The ΔS° must decrease by 3.38×10^–2 kcal/mol∙K.