Reversible Reactions and Equilibrium Quiz
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5 questions, one answer each
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1. Which symbol is used to represent a reversible reaction?
- A. ⇌
- B. →
- C. ⇒
- D. ↔
2. When copper(II) sulfate crystals (CuSO₄·5H₂O) are heated, they turn from blue to white. What does this demonstrate about reversible reactions?
- A. The forward reaction is exothermic
- B. Changing temperature can change the direction of a reversible reaction
- C. The reaction has reached equilibrium
- D. Water is a catalyst
3. A reversible reaction reaches equilibrium in a closed system. What must be true at equilibrium?
- A. The forward reaction has stopped completely
- B. The concentrations of reactants and products are equal
- C. The rate of the forward reaction equals the rate of the reverse reaction
- D. All reactants have been converted to products
4. In the Haber process (N₂(g) + 3H₂(g) ⇌ 2NH₃(g)), the equilibrium position is shifted to the right by increasing the pressure. Which explanation best accounts for this?
- A. Increasing pressure increases the temperature of the reaction
- B. Increasing pressure favours the side with fewer gas molecules, which is the product side
- C. A catalyst is added when pressure increases
- D. Increasing pressure increases the concentration of ammonia only
5. The Haber process operates at 450°C and the Contact process operates at 450°C, yet both are exothermic reactions. Explain why these processes do not use even higher temperatures to maximise product yield.
- A. Higher temperatures would cause the reaction vessel to explode
- B. Although higher temperatures would increase reaction rate, they would shift the equilibrium position to the left, reducing product yield and making the choice uneconomical
- C. Higher temperatures would prevent the catalyst from working
- D. It is impossible to heat reactions above 450°C