Question

If under a given set of conditions the reaction a b occurs with δg = –14 kj/mol, and the reaction c b occurs with δg = 16 kj/mol, then _______.

Answer 1

conversion of a to c is exergonic

Answer 2

The given information allows us to determine that both reactions can occur spontaneously but under different conditions. However, the conversion between A and C and its reversibility cannot be determined.

The given information states that the reaction A -> B occurs with a standard free energy change (ΔG) of -14 kJ/mol, and the reaction C -> B occurs with a ΔG of +16 kJ/mol. From this information, we can determine the following:

1. The standard free energy change (ΔG) of a reaction indicates whether the reaction is exergonic (releases free energy) or endergonic (absorbs free energy). A negative value of ΔG indicates an exergonic reaction.
2. Since the given reactions have different ΔG values, it means that both A -> B and C -> B can occur spontaneously but under different conditions.
3. The conversion of A to C cannot be determined solely based on the provided information.
4. The statement about the conversion of A to C being entropically driven is not accurate because entropic factors are not mentioned in the given information.
5. Finally, the reversibility of the conversion between C and A cannot be determined from the given information.

Complete Question:

If under a given set of conditions the reaction A → B occurs with ΔG--14 kJ/mol, and the reaction C-> B occurs with G-+ 16 kJ/mol, thena. conversion of A to C is exergonic. b.A and C can never be at equilibrium, even under different reaction conditions. c.conversion of A to C is entropically driven. d. conversion of C to A is freely reversible.