AQA A-Level Chemistry Paper 1 Sample 2023
This paper tests the core inorganic and physical chemistry content that sets the foundation for the entire A-Level course—the concepts that reappear in every subsequent exam. You'll face realistic questions on atomic structure, bonding, and equilibrium calculations that examiners use to separate the 7-mark students from the 9-mark ones. The 15 questions span three focused topics: structure and bonding fundamentals, energetics and kinetics, and equilibrium shifts, mixing multiple-choice with calculation problems at a difficulty level you'll see in June papers. If you can explain why a certain bond forms over another, calculate an enthalpy change, and predict Le Chatelier shifts, you've cracked the hardest part of Paper 1—and you'll know exactly what to expect in the real exam.
Questions in this quiz
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- Question 1
Sulfur has an atomic number of 16. Which of the following is the correct electron configuration for a sulfur atom in its ground state?
- Question 2
The first ionization energy of magnesium (738 kJ/mol) is lower than that of aluminum (578 kJ/mol) is a false statement. Which of the following best explains why aluminum actually has a lower first ionization energy than magnesium?
- Question 3
Which of the following correctly orders the substances by their melting points from lowest to highest?
- Question 4
The combustion of 1 mole of ethane (C₂H₆) releases 1560 kJ of energy. The enthalpy change for this reaction is:
- Question 5
Use the data below to calculate the enthalpy change for the reaction: C(s) + CO₂(g) → 2CO(g). Reaction 1: C(s) + O₂(g) → CO₂(g) ΔH = -393 kJ/mol. Reaction 2: 2CO(g) + O₂(g) → 2CO₂(g) ΔH = -566 kJ/mol.
- Question 6
The bond dissociation energy of H-H is 436 kJ/mol and H-Cl is 431 kJ/mol. The bond enthalpy for Cl-Cl is 244 kJ/mol. Calculate the enthalpy change for the reaction: H₂(g) + Cl₂(g) → 2HCl(g). (Use: ΔH = Σ(bonds broken) − Σ(bonds formed))
- Question 7
Nitrogen dioxide (NO₂) is a brown gas in equilibrium with dinitrogen tetroxide (N₂O₄), which is colourless. The reaction is: 2NO₂(g) ⇌ N₂O₄(g) ΔH = -58 kJ/mol. When the temperature is increased, the brown colour of the gas mixture becomes darker. This observation is best explained by:
- Question 8
For the gas-phase equilibrium: 2NH₃(g) ⇌ N₂(g) + 3H₂(g), write the correct expression for the equilibrium constant Kc.
- Question 9
A reaction has a very high activation energy. Which of the following statements is true regarding this reaction?
- Question 10
Which of the following statements correctly describes the effect of adding a catalyst to a reversible equilibrium reaction?
- Question 11
For the equilibrium: N₂(g) + 3H₂(g) ⇌ 2NH₃(g), if the pressure on the system is increased at constant temperature, which direction will the equilibrium shift?
- Question 12
The rate of a reaction doubles when the temperature is increased from 25°C to 35°C. The activation energy of this reaction is approximately:
- Question 13
An exothermic reaction with a positive entropy change (ΔS > 0) is thermodynamically feasible at all temperatures. Is this statement true or false?