Foundation Level (Fail → Pass)

Simple prompts to establish basic understanding.

1. Define an exothermic reaction.

2. Define an endothermic reaction.

3. State whether combustion is exothermic or endothermic.

4. Define enthalpy change (ΔH).

5. Describe how energy is transferred in an exothermic reaction.

6. What happens to the temperature of surroundings in an endothermic process?

7. Draw a simple energy level diagram for an exothermic reaction.

8. Define activation energy.

9. State one example of an endothermic reaction.

10. Define standard conditions (temperature and pressure).

 Intermediate Level (Pass → Credit)

Prompts requiring explanation, reasoning, and calculations.

1. Explain why bond breaking is endothermic and bond forming is exothermic.

2. Use bond energies to calculate ΔH for a reaction.

3. Compare enthalpy of reactants and products in exothermic reactions.

4. Explain Hess’s Law.

5. Draw an energy profile diagram showing activation energy.

6. Describe the difference between ΔHf° and ΔHc°.

7. Explain why some reactions occur spontaneously even if ΔH is positive.

8. Use ΔH = Σ(bonds broken) – Σ(bonds formed) for a given equation.

9. Describe how catalysts affect activation energy.

10. Explain the meaning of standard enthalpy of neutralization.

Advanced Level (Credit → Distinction)

Analytical, multi-step and conceptual prompts.

1. Explain how entropy influences spontaneity of reactions.

2. Derive and interpret the Gibbs free energy equation: ΔG = ΔH – TΔS.

3. Analyse why some endothermic reactions are spontaneous at high temperatures.

4. Compare entropy changes for solid → liquid → gas.

5. Evaluate how temperature affects ΔG for endothermic and exothermic reactions.

6. Explain the thermodynamic significance of equilibrium (ΔG = 0).

7. Discuss how enthalpy and entropy compete in determining spontaneity.

8. Use Gibbs free energy to predict feasibility of chemical processes.

9. Evaluate entropy changes in dissolution, mixing, and expansion of gases.

10. Analyse industrial reaction conditions using enthalpy and entropy considerations.