How does the equilibrium constant relate to the concentrations of reactants and products at equilibrium?

Given the reaction: 2A + B ⇌ 3C + D, with equilibrium concentrations [A] = 0.5 M, [B] = 0.2 M, [C] = 0.8 M, [D] = 0.4 M, calculate the equilibrium constant (K).

In a graph showing free energy versus component concentrations, what does the lowest point on the curve represent?

For the reaction: 2X + 3Y ⇌ 4Z + W, with equilibrium concentrations [X] = 0.1 M, [Y] = 0.2 M, [Z] = 0.3 M, [W] = 0.4 M, calculate the equilibrium constant (K).

A reaction has an equilibrium constant of 100. What does this suggest about the concentrations of reactants and products at equilibrium?

What is the change in Gibbs free energy (ΔG) for a reaction at equilibrium?

In a reaction where the concentration of reactant A is decreased below its equilibrium concentration, what will happen to restore equilibrium?