Common Misconceptions

⚠️ Common Misconceptions

Misconception 1: "Equilibrium means equal amounts of products and reactants"

At equilibrium, the rates of the forward and backward reactions are equal — not the concentrations. The equilibrium mixture may contain much more product than reactant, or vice versa. The ratio of products to reactants depends on the specific reaction and the conditions.

Misconception 2: "A catalyst shifts the equilibrium position to the right"

A catalyst speeds up both the forward and backward reactions equally. Therefore it has no effect on the equilibrium position — the ratio of products to reactants at equilibrium is unchanged. It only makes equilibrium reached faster.

Misconception 3: "Increasing temperature always increases the yield of products"

Increasing temperature shifts equilibrium in the endothermic direction. If the forward reaction is exothermic (as in the Haber process), increasing temperature shifts equilibrium left — towards reactants — actually reducing the yield of products. Temperature and yield trade off against each other in industrial processes.