Question

In the case of a simple conversion reaction such as X->Y, which value of ΔG° is associated with a larger concentration of X than Y at equilibrium? (Hint: How is ΔG° related to K?)

(a) ΔG°=-5
(b) ΔG°=-1
(c) ΔG° = 0
(d) ΔG° = 1

Answer 1

In a simple conversion reaction, a positive value of ΔG° indicates a non-spontaneous reaction and a larger concentration of X than Y at equilibrium.

Step-by-step explanation:

In a simple conversion reaction such as X -> Y, the value of ΔG° is associated with a larger concentration of X than Y at equilibrium when ΔG° is greater than zero. This is because a positive value of ΔG° indicates that the reaction is non-spontaneous in the forward direction, meaning that there will be a larger concentration of reactants (X) than products (Y) at equilibrium.

Furthermore, the relationship between ΔG° and the equilibrium constant (K) is given by the equation: ΔG° = -RTln(K), where R is the gas constant and T is the temperature in Kelvin. When ΔG° is positive, which indicates a non-spontaneous reaction, the value of K will be less than 1. This means that there will be a larger concentration of X (reactant) than Y (product) at equilibrium.

Therefore, a positive value of ΔG° indicates a non-spontaneous reaction and a larger concentration of X than Y at equilibrium.