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100+ Free QCE Chemistry Practice Questions

Pass your QCE Chemistry (Units 3 & 4) External Examination exam on the first try — instant access, no signup required.

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Key Facts: QCE Chemistry Exam

50%

The external examination contributes 50% of the final QCE Chemistry subject result

QCAA Chemistry General senior syllabus

Two papers

The external examination is delivered as Paper 1 and Paper 2, both covering Units 3 and 4

QCAA Chemistry external assessment

20 questions

Paper 1 Section 1 has 20 multiple-choice questions worth 20 marks

QCAA Chemistry Paper 1 question and response book

90 minutes

Each paper allows 90 minutes working time plus 10 minutes perusal

QCAA Chemistry external examination papers

Units 3 and 4

Equilibrium, acids and redox (Unit 3) and structure, synthesis and design (Unit 4)

QCAA Chemistry General senior syllabus

Calculator and data book

A QCAA-approved calculator and the Chemistry formula and data book are permitted

QCAA Chemistry external examination instructions

Year 12

Sat by Year 12 Queensland students as part of the Queensland Certificate of Education

QCAA Chemistry General senior syllabus

100

Free original multiple-choice practice questions here

OpenExamPrep

QCE Chemistry is the QCAA General senior subject sat by Year 12 students in Queensland for the Queensland Certificate of Education. The external examination covers Units 3 and 4 and is worth 50% of the final subject result. It is delivered in two papers: Paper 1 includes a 20-question multiple-choice section (20 marks) plus short response, and Paper 2 is entirely short response with calculations and interpretation. Each paper allows 90 minutes working time plus 10 minutes perusal, and a QCAA-approved calculator and the QCAA Chemistry formula and data book are permitted. This 100-question bank provides original multiple-choice practice across equilibrium, redox and electrochemistry, acids and bases, and organic chemistry.

Sample QCE Chemistry Practice Questions

Try these sample questions to test your QCE Chemistry exam readiness. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1Which statement best describes a system at dynamic chemical equilibrium?
A.The forward and reverse reactions have both stopped
B.The forward and reverse reactions occur at equal rates
C.The concentrations of reactants and products are always equal
D.Only the forward reaction is still occurring
Explanation: At dynamic equilibrium the forward and reverse reactions continue but proceed at equal rates, so the concentrations of reactants and products remain constant over time. The reactions do not stop; they balance.
2For the equilibrium N2(g) + 3H2(g) ⇌ 2NH3(g), which is the correct expression for Kc?
A.[N2][H2]³ / [NH3]²
B.[NH3]² / ([N2][H2]³)
C.[NH3] / ([N2][H2])
D.2[NH3] / ([N2] + 3[H2])
Explanation: Kc is the product concentrations over reactant concentrations, each raised to the power of its coefficient: [NH3]² / ([N2][H2]³). Products go on top and reactants on the bottom.
3A large value of Kc (Kc ≫ 1) for a reaction at a given temperature indicates that at equilibrium:
A.Reactants are favoured
B.Products are favoured
C.The reaction has not started
D.The reaction is at the same point as the start
Explanation: When Kc is much greater than 1, the numerator (products) dominates, so the equilibrium position lies towards the products. A small Kc would favour reactants.
4For the exothermic equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the temperature?
A.The equilibrium shifts towards SO3 and Kc increases
B.The equilibrium shifts towards reactants and Kc decreases
C.The equilibrium shifts towards reactants but Kc is unchanged
D.The equilibrium position and Kc are both unchanged
Explanation: For an exothermic forward reaction, increasing temperature shifts the equilibrium towards the reactants (the endothermic direction), reducing the yield of SO3. Because temperature changes Kc, the value of Kc decreases.
5For the equilibrium N2O4(g) ⇌ 2NO2(g), what happens when the volume of the container is decreased at constant temperature?
A.The equilibrium shifts towards NO2
B.The equilibrium shifts towards N2O4
C.There is no shift because moles of gas are equal
D.Kc increases
Explanation: Decreasing the volume increases the pressure, so the system shifts to the side with fewer moles of gas. The left side has 1 mole (N2O4) versus 2 moles on the right, so the equilibrium shifts towards N2O4.
6Adding an inert gas such as argon to a gaseous equilibrium at constant volume and temperature will:
A.Shift the equilibrium towards the products
B.Shift the equilibrium towards the reactants
C.Not shift the equilibrium position
D.Increase the value of Kc
Explanation: At constant volume, adding an inert gas does not change the partial pressures or concentrations of the reacting species, so it does not change the reaction quotient and the equilibrium position does not shift.
7Adding a catalyst to a system at equilibrium will:
A.Shift the equilibrium towards the products
B.Increase the value of Kc
C.Increase the yield of products
D.Have no effect on the position of equilibrium
Explanation: A catalyst speeds up the forward and reverse reactions equally, so equilibrium is reached faster but the position of equilibrium and the value of Kc are unchanged.
8For H2(g) + I2(g) ⇌ 2HI(g), at equilibrium [H2] = 0.20 M, [I2] = 0.20 M and [HI] = 1.6 M. What is Kc?
A.4.0
B.8.0
C.40
D.64
Explanation: Kc = [HI]² / ([H2][I2]) = (1.6)² / (0.20 × 0.20) = 2.56 / 0.040 = 64. The product concentration is squared because of its coefficient of 2.
9If the reaction quotient Q is less than the equilibrium constant Kc, the reaction will:
A.Proceed in the forward direction to form more products
B.Proceed in the reverse direction to form more reactants
C.Already be at equilibrium
D.Stop completely
Explanation: When Q < Kc, there are relatively too many reactants, so the net reaction proceeds forward, converting reactants to products until Q equals Kc.
10Which change would increase the yield of products for the endothermic equilibrium CaCO3(s) ⇌ CaO(s) + CO2(g)?
A.Decreasing the temperature
B.Adding more CaCO3 solid
C.Removing CO2 gas as it forms
D.Increasing the pressure
Explanation: Removing CO2 as it forms reduces its concentration, so by Le Chatelier's principle the system shifts forward to replace it, increasing the conversion of CaCO3. Solids do not affect the equilibrium position.

About the QCE Chemistry Exam

QCE Chemistry is a QCAA General senior subject taken by Year 12 students in Queensland as part of the Queensland Certificate of Education. The external examination assesses Units 3 and 4: Unit 3 'Equilibrium, acids and redox reactions' covers chemical equilibrium systems, oxidation and reduction (galvanic and electrolytic cells and standard electrode potentials) and acids and bases (pH, Ka, Kb, buffers and titrations); Unit 4 'Structure, synthesis and design' covers the properties and structure of organic materials, chemical synthesis and design, and macromolecules and materials. The external examination is delivered in two papers, with Paper 1 including a 20-question multiple-choice section and Paper 2 being entirely short response with calculations and data interpretation. A QCAA-approved calculator and the QCAA Chemistry formula and data book are permitted.

Assessment

External examination over two papers. Paper 1: Section 1 has 20 multiple-choice questions (20 marks) and Section 2 has short-response questions. Paper 2 is entirely short response (calculations and interpretation). This bank focuses on the multiple-choice content style.

Time Limit

Each paper allows 90 minutes working time plus 10 minutes perusal, totalling about 3 hours of working time for the external examination.

Passing Score

No fixed pass mark. The external examination is worth 50% of the final subject result and is combined with internal assessment for the overall A-to-E grade; there is no single cut score.

Exam Fee

There is no separate per-exam fee paid to QCAA; external examination assessment is part of the student's school enrolment in the QCAA Chemistry General senior subject. (Queensland Curriculum and Assessment Authority (QCAA))

QCE Chemistry Exam Content Outline

17%

Chemical equilibrium systems (Unit 3)

Dynamic equilibrium and reversible reactions, Le Chatelier's principle, writing and calculating the equilibrium constant Kc, the reaction quotient Q, and solubility equilibria including Ksp and the common-ion effect.

17%

Oxidation and reduction (Unit 3)

Assigning oxidation numbers, balancing redox half-equations, galvanic (voltaic) cells, electrolytic cells, the standard electrode potential table, calculating standard cell potential, predicting spontaneity, and electrolysis products.

16%

Acids and bases (Unit 3)

Brønsted-Lowry acids and bases and conjugate pairs, strong and weak acids, pH and pOH, the acid and base dissociation constants Ka and Kb, buffers, titration curves, equivalence points and choosing indicators.

17%

Properties and structure of organic materials (Unit 4)

Functional groups, IUPAC nomenclature, structural isomers and stereoisomers, intermolecular forces and physical properties, and characteristic reactions of alkanes, alkenes, alcohols, haloalkanes, carboxylic acids, esters and amines.

17%

Chemical synthesis and design (Unit 4)

Multi-step reaction pathways and organic synthesis, percentage yield, atom economy and the principles of green chemistry for designing efficient and sustainable processes.

16%

Macromolecules and materials (Unit 4)

Addition and condensation polymers and their monomers, structure-property relationships of polymers, and biological macromolecules such as proteins and carbohydrates.

How to Pass the QCE Chemistry Exam

What You Need to Know

  • Passing score: No fixed pass mark. The external examination is worth 50% of the final subject result and is combined with internal assessment for the overall A-to-E grade; there is no single cut score.
  • Assessment: External examination over two papers. Paper 1: Section 1 has 20 multiple-choice questions (20 marks) and Section 2 has short-response questions. Paper 2 is entirely short response (calculations and interpretation). This bank focuses on the multiple-choice content style.
  • Time limit: Each paper allows 90 minutes working time plus 10 minutes perusal, totalling about 3 hours of working time for the external examination.
  • Exam fee: There is no separate per-exam fee paid to QCAA; external examination assessment is part of the student's school enrolment in the QCAA Chemistry General senior subject.

Keys to Passing

  • Complete 500+ practice questions
  • Score 80%+ consistently before scheduling
  • Focus on highest-weighted sections
  • Use our AI tutor for tough concepts

QCE Chemistry Study Tips from Top Performers

1Practise writing Kc and Ksp expressions directly from balanced equations, then rehearse the multi-step substitution so you can finish equilibrium calculations within exam time.
2Memorise the rules for assigning oxidation numbers and practise reading the standard electrode potential table both ways, so you can identify the oxidising and reducing agents and calculate cell EMF quickly.
3Drill acid-base calculations: pH from [H+], Ka or Kb from pH, and the assumptions for weak-acid problems, because Paper 2 often asks for working to a set number of decimal places.
4Learn the characteristic reactions and reagents for each organic functional group so you can complete reaction pathways and deduce products and IUPAC names with confidence.
5Use the QCAA Chemistry formula and data book while practising so that on exam day you know exactly where each constant, equation and the potential table is located.
6Work through QCAA past external examination papers under timed conditions and check your answers against the official marking guides to learn the expected level of detail.

Frequently Asked Questions

How is the QCE Chemistry external examination structured?

It is delivered in two papers. Paper 1 has a 20-question multiple-choice section (20 marks) plus a short-response section; Paper 2 is entirely short response with calculations and interpretation. Both papers cover Units 3 and 4.

How much is the external examination worth?

The external examination is worth 50% of the final QCE Chemistry subject result. The remaining 50% comes from internal assessment: the Data Test, Student Experiment and Student Research Investigation.

How long is each Chemistry paper?

Each paper allows 90 minutes of working time plus 10 minutes of perusal, so the external examination totals about three hours of working time across Paper 1 and Paper 2.

Can I use a calculator and a data sheet?

Yes. A QCAA-approved calculator is permitted and the QCAA Chemistry formula and data book is provided, which includes constants, the standard electrode potential table and other data needed for calculations.

What topics does the exam cover?

Units 3 and 4: chemical equilibrium systems, oxidation and reduction and electrochemistry, acids and bases, properties and structure of organic materials, chemical synthesis and design, and macromolecules and materials.

Are these official QCAA questions?

No. These are original OpenExamPrep practice questions modelled on the syllabus and the multiple-choice style of the external examination. QCAA publishes its own past papers and marking guides separately.