What is the impact on K if ΔG is zero?

When the Gibbs free energy change (ΔG) for a reaction is zero, this indicates that the system is at equilibrium. At this state, the forward and reverse reactions occur at equal rates, meaning there is no net change in the concentration of reactants and products.

Under these conditions, the relationship between the standard Gibbs free energy change (ΔG°) and the equilibrium constant (K) is given by the equation:

ΔG = ΔG° + RT ln(Q),

where Q is the reaction quotient. At equilibrium, Q equals K, and thus the equation simplifies to:

0 = ΔG° + RT ln(K).

This leads to:

ΔG° = -RT ln(K).

If ΔG is zero, it simplifies to:

0 = ΔG°, which means ΔG° must equal to zero. When ΔG° equals zero, it indicates that the standard Gibbs free energy of the reactants and products are equal, leading to the conclusion that K must equal 1. This means the concentrations of products and reactants are such that they are proportionate, resulting in the equilibrium constant being equal to one. Therefore, the correct answer to the question about the impact on K when ΔG is zero is that K equals