Chemistry – Chemical reactions - Reversible reactions and equilibrium | e-Consult

As the reaction reaches equilibrium, the concentrations of N₂ and H₂ will decrease. This is because at equilibrium, the rates of the forward and reverse reactions are equal. Since the forward reaction involves the consumption of N₂ and H₂ to produce NH₃, the rate of consumption of these reactants must be equal to the rate of their production. Therefore, the concentrations of N₂ and H₂ will be lower at equilibrium than they were at the start of the reaction. The concentrations of NH₃ will be higher than they were at the start of the reaction. This is a direct consequence of the definition of equilibrium: a state where the forward and reverse processes are balanced, leading to no net change in the concentrations of reactants and products.