This common misconceptions covers Common Misconceptions within Equilibrium (HT) for GCSE Chemistry. Revise Equilibrium (HT) in Rates of Reaction for GCSE Chemistry with 23 exam-style questions and 18 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 9 of 14 in this topic. Use this common misconceptions to connect the idea to the wider topic before moving on to questions and flashcards.
⚠️ 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.
Practice questions for Equilibrium (HT)
At dynamic equilibrium, which of the following is true?
Explain the effect of increasing temperature on the position of an equilibrium where the forward reaction is exothermic.