Question

Describe the relationship between the values of ΔG, Keq, and the direction that a reaction will spontaneously proceed.

Answer 1

ΔG is related to Q by the equation ΔG=RTlnQK. If ΔG < 0, then K > Q, and the reaction must proceed to the right to reach equilibrium. If ΔG > 0, then K < Q, and the reaction must proceed to the left to reach equilibrium. If ΔG = 0, then K = Q, and the reaction is at equilibrium.

Answer 2

oop! typo. That should be dG = - RTlnK

Answer 3

[AI-generated answer — Explain Bot]

The relationship between ΔG (Gibbs free energy), Keq (equilibrium constant), and the direction of spontaneous reaction can be explained using the following principles:

1. ΔG: ΔG refers to the change in Gibbs free energy during a chemical reaction. It indicates whether the reaction is spontaneous or non-spontaneous. A negative ΔG value indicates that the reaction is spontaneous, while a positive ΔG value indicates a non-spontaneous reaction. If ΔG is zero, the reaction is said to be at equilibrium.

2. Keq: Keq is the equilibrium constant. It is a measure of the ratio of product concentrations to reactant concentrations at equilibrium. Keq values greater than 1 indicate that the concentration of products is greater than that of reactants at equilibrium, favoring the forward reaction. Keq values less than 1 indicate the opposite, favoring the reverse reaction.

3. Relationship between ΔG and Keq: The relationship between ΔG and Keq can be expressed by the equation: ΔG = -RT * ln(Keq), where R is the gas constant and T is the temperature in Kelvin. This equation shows that ΔG is directly related to Keq. If Keq is greater than 1, ln(Keq) is positive, resulting in a negative ΔG value. Hence, the reaction will proceed spontaneously in the forward direction. Conversely, if Keq is less than 1, ln(Keq) is negative, resulting in a positive ΔG value. In this case, the reaction will proceed spontaneously in the reverse direction.

In summary, a negative ΔG value indicates a spontaneous reaction moving in the forward direction (from reactants to products), while a positive ΔG value indicates a non-spontaneous reaction or a spontaneous reaction moving in the reverse direction (from products to reactants). The value of Keq determines the magnitude and direction of the ΔG value.