A chemistry student needs to determine the effect on the equilibrium position of a chemical reaction when the concentration of a reactant is decreased. The student is given the balanced equation: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + heatIf the concentration of H₂ is decreased by removing 50% of its concentration, what would be the effect on the concentration of N₂, NH₃, and the position of equilibrium?

Question

A chemistry student needs to determine the effect on the equilibrium position of a chemical reaction when the concentration of a reactant is decreased. The student is given the balanced equation: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + heatIf the concentration of H₂ is decreased by removing 50% of its concentration, what would be the effect on the concentration of N₂, NH₃, and the position of equili

Answer 1

When the concentration of H is decreased by 50%, the system will no longer be at equilibrium. According to Le Chatelier's principle, the system will shift to counteract the change and re-establish equilibrium. In this case, the system will shift to the left  towards the reactants  to compensate for the decrease in H concentration.As a result, the concentration of NH will decrease as it is converted back into N and H. The concentration of N will increase as more N is produced from the conversion of NH. The position of equilibrium will shift to the left, favoring the reactants.In summary, the concentration of N will increase, the concentration of NH will decrease, and the position of equilibrium will shift to the left.