Question

Below is a list of 5 hypothetical chemical reactions with their respective $\triangle$ G standard and $\triangle$ G values. Which reaction has the most free energy to release as the reaction reaches equilibrium?

a) $\triangle$ G standard = 183kJ/mol $\triangle$ G = -26kJ/mol

b) $\triangle$ G standard = -32kJ/mol $\triangle$ G = -57kJ/mol

c) $\triangle$ G standard = 23kJ/mol $\triangle$ G = 35kJ/mol

d) $\triangle$ G standard = -247kJ/mol $\triangle$ G =48kJ/mol

e) $\triangle$ G standard = 252kJ/mol $\triangle$ G = 0kJ/mol

(answer is B, please explain)

Answer 1

delta G = delta G degree + Rt lnK delta G = delta G degree = delta G degree + 2.303 RT log(k) for an exothermic reaction and spontaneous reaction delta G degree is negative. At equilibrium delta G is equal to zero.