Foundation Level (Fail → Pass)

Basic prompts to build initial understanding.

1. Define a reversible reaction.

2. What is meant by chemical equilibrium?

3. Explain the term “dynamic equilibrium.”

4. State one condition required for equilibrium to occur.

5. What does it mean when the forward and reverse reaction rates are equal?

6. Give one everyday example of equilibrium.

7. Define Le Chatelier’s Principle in simple words.

8. State what happens to equilibrium when concentration increases.

9. What happens to equilibrium when temperature increases in an endothermic reaction?

10. What happens when pressure is increased in a gas reaction?

 Intermediate Level (Pass → Credit)

Prompts requiring explanation, application, and reasoning.

1. Explain how Le Chatelier’s Principle predicts changes in equilibrium.

2. Describe how catalysts affect equilibrium position.

3. Write the equilibrium constant expression (Kc) for a given reaction.

4. Explain what a high Kc value indicates about a reaction.

5. Analyse what happens to equilibrium when reactant concentration decreases.

6. Describe the effect of temperature on exothermic equilibrium reactions.

7. Explain what happens when pressure is decreased in a gas-phase equilibrium.

8. Explain why solids and liquids do not appear in Kc expressions.

9. Use the reaction quotient (Q) to determine direction of shift.

10. Compare Kc and Q for predicting equilibrium movement.

Advanced Level (Credit → Distinction)

High-order analytical and multi-step reasoning prompts.

1. Derive the expression for Kc from stoichiometric coefficients.

2. Analyse how temperature changes affect the numerical value of Kc.

3. Evaluate the role of entropy and enthalpy in determining equilibrium position.

4. Discuss why catalysts do not alter the value of Kc.

5. Use thermodynamic principles to explain equilibrium in industrial processes.

6. Predict equilibrium shifts in multi-step reactions with coupled equilibria.

7. Explain how partial pressures are used in Kp calculations.

8. Analyse why Haber process conditions represent a compromise between yield and rate.

9. Compare homogeneous and heterogeneous equilibria.

10. Calculate equilibrium concentrations using ICE tables for a given system.