Chemical Equilibrium
Chemistry · 50 practice questions
Reversible reactions and the factors governing the equilibrium position; dynamic equilibrium; Le Chatelier's principle and the equilibrium constant, with simple examples (e.g. action of steam on iron; N₂O₄ ⇌ 2NO₂); no calculations required.
- Identify the factors that affect the position of equilibrium of a chemical reaction.
- Predict the effect of each factor on the position of equilibrium.
- Determine the effects of these factors on the equilibrium constant.
Try a few questions
- Practice question 1
A small value of the equilibrium constant, Kc, mainly indicates that at equilibrium
- A.the reaction strongly favours the reactants, with little product formed
- B.the reaction strongly favours the products, with little reactant remaining
- C.the reaction is proceeding extremely quickly
- D.the reaction is highly exothermic
Show the answer
A. the reaction strongly favours the reactants, with little product formed
A small Kc reflects an equilibrium position lying well over toward the reactants.
- Practice question 2
Continuously removing a product from a reaction mixture at equilibrium mainly shifts the equilibrium position
- A.backward, toward the reactants
- B.forward, toward the products, to help replace what was removed
- C.not at all, since removing a product has no effect on equilibrium
- D.backward, but only if a catalyst is also added
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B. forward, toward the products, to help replace what was removed
Le Chatelier's principle predicts the system will shift to replace the continuously removed product.
- Practice question 3
A decrease in temperature applied to an endothermic forward reaction at equilibrium mainly shifts the equilibrium position
- A.forward, favouring the products
- B.not at all, since temperature never affects this type of equilibrium
- C.backward, favouring the reactants
- D.forward, but only if pressure is also decreased
Show the answer
C. backward, favouring the reactants
Cooling disfavours the endothermic direction, so the equilibrium shifts back toward the reactants to release relatively more heat.
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