Question

The condition of a system at equilibrium represents a balance between the tendency toward lowest energy (E) and the tendency toward molecular chaos or maximum entropy (S). The Gibbs Free Energy, G, is the state function that combines energy and entropy into an equation that allows us to find the balance between these two tendencies. For a system undergoing change at constant temperature, ΔG = ΔH - TΔS. The system stops changing when it reaches the equilibrium condition, ΔG = 0.

If a system is not initially at equilibrium, the direction the reaction will proceed (toward products or toward reactants) is determined by calculating ΔG for the initial concentrations:

If Q < K, is ΔG positive or negative? In which direction will the reaction (or other chemical process) proceed?

1. Towards the reactants

2. Towards products

3. Nothing Happens

Answer 1

If Q < K, then the reaction is not at equilibrium, in order to reach the equilibrium state, Q should increase and reach to a value of K. Therefore reaction will proceed in toward products.(2)
As the reaction is going spontaneously in the forward direction, hence $\Delta G$ will be negative.