Exam-style practice (harder): Chemistry multiple choice
14 harder, exam-style VCE Chemistry Units 3 and 4 multiple-choice questions: calorimetry, galvanic and electrolytic cells, equilibrium, rates, isomers, reaction pathways, NMR, titration, HPLC and food chemistry. Each is tagged with its question type and every distractor's error explained. Original practice questions, not from any VCAA exam.
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Why this set is harder than our topic quizzes
Our topic quizzes check facts and definitions. VCE Chemistry multiple choice mostly asks you to calculate, predict or interpret: a calorimetry result, a cell voltage, a shift in equilibrium, a structure from an NMR spectrum. Each wrong option is the answer you reach by making one specific slip.
These 14 questions follow that pattern. They are original practice questions written by ExamExplained, not taken from any VCAA examination. Each explanation begins with a Type tag and names the slip behind every wrong option.
For every calculation, write the equation or relationship first (n = Q / F, Kc expression, q = mcΔT) and carry units through. Then look for your answer. Most distractors come from a missing step: a charge of 2, a dilution factor, an efficiency.
The question types
| Type | What it looks like | Typical trap |
|---|---|---|
| Calculation | Calorimetry, Faraday's laws, Kc, titration, energy from fuels | Moles for concentrations, minutes for seconds, dilution not reversed, efficiency applied the wrong way |
| Data interpretation | Electrochemical series, equilibrium changes, NMR, HPLC calibration | Adding potentials, matching splitting without checking shifts, retention time used as a measure of amount |
| Concept application | Galvanic cells, catalysts, isomers, reaction pathways, glycaemic index | Electron flow through the salt bridge, catalysts "shifting" equilibrium, counting ethers as alcohols |
Question map
| Q | Type | Study design area |
|---|---|---|
| 1 | Calculation | Unit 3 AoS 1: solution calorimetry |
| 2 | Concept application | Unit 3 AoS 1: galvanic cells |
| 3 | Calculation | Unit 3 AoS 2: electrolysis and Faraday's laws |
| 4 | Data interpretation | Unit 3 AoS 1: electrochemical series and cell voltage |
| 5 | Calculation | Unit 3 AoS 2: equilibrium constant |
| 6 | Concept application | Unit 3 AoS 2: catalysts and Maxwell-Boltzmann |
| 7 | Data interpretation | Unit 3 AoS 2: Le Chatelier's principle |
| 8 | Concept application | Unit 4 AoS 1: structural isomers |
| 9 | Concept application | Unit 4 AoS 1: organic reaction pathways |
| 10 | Data interpretation | Unit 4 AoS 2: ¹H NMR |
| 11 | Calculation | Unit 4 AoS 2: volumetric analysis |
| 12 | Data interpretation | Unit 4 AoS 2: HPLC and calibration |
| 13 | Concept application | Unit 4 AoS 2: glycaemic index |
| 14 | Calculation | Unit 3 AoS 1: energy from fuels |
Five checks that catch most distractors
- Charge in Faraday calculations. Divide moles of electrons by the number of electrons in the half-equation.
- Cell voltage is a difference. E°(cathode) minus E°(anode), never multiplied by coefficients.
- Only temperature changes Kc. Concentration, pressure, volume and catalysts do not.
- Chemical shift before splitting. Two esters can share a singlet, quartet and triplet; the shifts tell them apart.
- Reverse every dilution. Titration and calibration results give the diluted concentration first.
Thinking electrons move through the salt bridge. The salt bridge carries ions to balance charge; electrons only travel through the external circuit.
What to do next
- Revise Unit 3 in the Unit 3 deep dive and practise energetics calculations.
- Revise Unit 4 in the Unit 4 deep dive.
- Then complete a VCAA past examination and check it against the examination report.
Sources & how we know this
- chemistry
- vce-chemistry
- multiple-choice
- exam-technique
- practice-questions
- units-3-4