QCE Chemistry EA preparation strategy: The 2026 guide

Study guide16 min readUpdated 7 Oct 2026

Quick answer

QCE Chemistry EA is two papers (each 90 minutes plus 5 minutes of perusal in 2026, calculator-active; check QCAA for the mark allocation and question types) covering Units 3 and 4; a six-week preparation routine moving from key-knowledge review through calculation drills to full timed papers, with attention to 3 significant figures, units throughout, the show-working convention, and proper use of the data booklet, secures top marks.

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What this guide is for
Paper 1 structure
Paper 2 structure
Question types
Marking criteria
Six-week preparation routine
Key calculation types
Common student errors
Check your knowledge

What this guide is for

QCE Chemistry EA is 50 percent of the subject result. Strong preparation requires familiarity with both papers' formats, the question types, and a structured revision routine. This guide covers all three.

Paper 1 structure

90 minutes plus 5 minutes of perusal. QCAA sets the mark allocation and sections, so check the syllabus for the 2026 format. Papers have typically combined multiple choice with short response.

Tests across Unit 3 and Unit 4 topics. Calculator-active.

Paper 2 structure

90 minutes plus 5 minutes of perusal. Check the syllabus for the 2026 mark allocation and question types.

Items combine short response with data analysis components. QCAA has not confirmed a separate extended-response section for 2026, so treat longer multi-part items as likely rather than certain.

Expect some longer multi-mark items on synthesis pathways, spectroscopy interpretation, or industrial chemistry, but check QCAA's specifications for the real mark values.

Question types

Multiple choice: Knowledge recall, simple calculations, structure identification.
Short response (2-5 marks): Specific calculations, short explanations, balanced equations.
Extended response (8-10 marks): Multi-step calculations, synthesis pathways, multi-part data analysis, comparative analysis.

Marking criteria

QCAA rewards:

Correct chemistry. Equations balanced, formulas correct.
Show working. Even if the final answer is wrong, method marks are available.
Significant figures. Typically 3 sig fig unless specified.
Units. Always include.
Clear communication. Scientific writing in explanations.

Top band requires excellence in all five.

Six-week preparation routine

Weeks 1-2: Review key knowledge. Use QCAA Syllabus as checklist. Map each subject matter point to your notes.
Weeks 3-4: Calculation drills. Practice each type: equilibrium ( $K_c$ , ICE tables), pH (strong, weak, buffer), titration, percentage yield, atom economy.
Week 5: Extended response drills. Practice 8-10 mark items on synthesis pathways, spectroscopy interpretation, multi-step problems.
Week 6: Full timed past papers. Mark against published exemplars.

Key calculation types

A galvanic cell drives the redox extended-response item that appears in most Paper 2 sittings. QCAA's preferred cell-notation convention puts the anode left and cathode right, separated by the salt bridge.

QCAA cell notation lists the anode half-cell on the left, the salt bridge as a double vertical bar, and the cathode half-cell on the right; the standard potential follows from

E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}

Paper 2 commonly pairs an IR spectrum with a proton-NMR spectrum for structural elucidation. The IR pins down the functional group and the NMR pins down the carbon skeleton; together they identify the compound.

IR spectrum of ethanoic acid sketched against the QCAA data booklet ranges; the broad O-H above 2500 paired with the sharp C=O near 1715 cm⁻¹ confirms a carboxylic acid before the NMR is even consulted.

Proton NMR sketch of ethyl ethanoate: the triplet at 1.25 ppm plus quartet at 4.12 ppm signals an ethyl group bonded to oxygen and the lone singlet at 2.05 ppm is the ester methyl with no proton neighbours.

A reaction energy profile underpins both rate-of-reaction items in Paper 1 and the catalyst-comparison extended response in Paper 2. The forward $E_a$ , reverse $E_a$ and $\Delta H$ all read off a single diagram.

The forward

E_a

sets the rate while

\Delta H < 0

sets the thermodynamics; a catalyst lowers

E_a

without altering

\Delta H

Equilibrium constant $K_c$: Equilibrium concentrations divided by reactant concentrations, each raised to stoichiometric coefficient.
pH for strong acid: $\text{pH} = -\log[H^+]$ .
pH for weak acid: Use $K_a$ . $K_a = [H^+][A^-]/[HA]$ . Approximation: $[H^+] = \sqrt{K_a \cdot c}$ for $c >> K_a$ .
Buffer pH: Henderson-Hasselbalch: $\text{pH} = pK_a + \log([A^-]/[HA])$ .
Titration: $c_1 V_1 = c_2 V_2$ for 1:1 stoichiometry; modify for other ratios.
Percentage yield: (actual / theoretical) $\times$ 100 percent.
Atom economy: (Mr of desired product / sum of Mr of all products) $\times$ 100 percent.

Common student errors

Significant figures: Use 3 sig fig unless data has different precision.
Units missing: Every numerical answer needs units.
Wrong $K_a$ from data booklet: Check the table carefully.
Markovnikov direction confusion: H goes to the carbon with more hydrogens; X to the more substituted carbon.
Catastrophic error compounding: Don't double-down on a wrong approach. If your equation gives nonsense (negative concentration, pH above 14), recheck.
Calculator-style data analysis: Always interpret the numbers chemically.

Check your knowledge

A mix of recall, short-response calculation, and EA-style extended-response questions covering Unit 3 and Unit 4 subject matter. Answer all under timed conditions (about 1 minute per mark), then check against the solutions block. Three significant figures and units throughout.

Give the IUPAC name and identify the functional-group class for each of: (a) $CH_3CH_2CH(OH)CH_3$ , (b) $CH_3CH_2COOCH_3$ , (c) $CH_3CH_2CH_2NH_2$ , (d) $CH_3COCH_2CH_3$ . (4 marks)
Calculate the mass of $CO_2$ produced when 5.40 g of butane is burned completely in excess oxygen. $M_r(C_4H_{10}) = 58.14$ ; $M_r(CO_2) = 44.01$ . (3 marks)
25.0 g of nitrogen and 6.00 g of hydrogen are placed in a 10.0 L vessel and allowed to react to form ammonia. After equilibrium is established 12.0 g of ammonia is present. Identify the limiting reagent and calculate the percentage yield. $M_r(N_2) = 28.02$ ; $M_r(H_2) = 2.016$ ; $M_r(NH_3) = 17.03$ . (4 marks)
State whether each species is a Bronsted-Lowry acid, base or amphiprotic, and write the equation for its reaction with water: (a) $HSO_4^-$ , (b) $NH_3$ , (c) $HCO_3^-$ . (3 marks)
A galvanic cell is constructed at 25 degrees C with a copper half-cell ( $Cu^{2+}/Cu$ , $E^{\circ} = +0.34$ V) and a silver half-cell ( $Ag^+/Ag$ , $E^{\circ} = +0.80$ V). (a) Write the overall cell equation. (b) Calculate $E^{\circ}_{\text{cell}}$ . (c) Identify the cathode. (3 marks)
Predict the major product of each reaction and name it: (a) propene + HBr; (b) butan-2-ol heated with acidified $K_2Cr_2O_7$ under reflux; (c) ethanoic acid + propan-1-ol in concentrated $H_2SO_4$ . (3 marks)
The Haber process is operated at the Gladstone industrial complex to produce ammonia: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ , $\Delta H = -92$ kJ mol $^{-1}$ . (a) Predict and justify the effect on the yield of ammonia of (i) increasing temperature, (ii) increasing pressure, (iii) adding an iron catalyst. (b) The industrial conditions used are around 450 degrees C and 200 atm with an iron catalyst. Justify why these conditions are chosen even though theory predicts a higher yield at lower temperature. (5 marks)
A student at a Mount Isa school constructs an electrochemical cell to investigate the relative activity of three metals (M1, M2, M3) by measuring cell potentials against a standard zinc half-cell ( $E^{\circ}(Zn^{2+}/Zn) = -0.76$ V). The measured potentials (M as cathode, Zn as anode) are M1 +1.10 V, M2 +0.34 V, M3 -0.42 V. (a) Calculate the standard reduction potential of each metal. (b) Rank the three metals from strongest to weakest oxidising agent in their ionic form. (c) Predict, with justification, whether a spontaneous reaction occurs when M3 is placed in a 1.0 M solution of M1 $^{n+}$ . (d) Identify a Queensland mining context where reduction-potential ranking matters and explain its relevance in one sentence. (5 marks)

Solutions

Q1: (a) Butan-2-ol; secondary alcohol. (b) Methyl propanoate; ester. (c) Propan-1-amine; primary amine. (d) Butan-2-one; ketone.
Q2: Step 1: $n(C_4H_{10}) = 5.40 / 58.14 = 0.0929$ mol. Step 2: balanced equation $2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O$ ; mole ratio $C_4H_{10}:CO_2 = 1:4$ . Step 3: $n(CO_2) = 4 \times 0.0929 = 0.372$ mol. Step 4: $m(CO_2) = 0.372 \times 44.01 = 16.4$ g. The mass of $CO_2$ produced is 16.4 g.
Q3: Step 1: moles available: $n(N_2) = 25.0 / 28.02 = 0.892$ mol; $n(H_2) = 6.00 / 2.016 = 2.976$ mol. Step 2: for $N_2 + 3H_2 \rightarrow 2NH_3$ , $H_2$ required to consume all $N_2 = 3 \times 0.892 = 2.68$ mol; $H_2$ available 2.976 mol, so $N_2$ is the limiting reagent. Step 3: theoretical $n(NH_3) = 2 \times 0.892 = 1.784$ mol; theoretical mass $= 1.784 \times 17.03 = 30.4$ g. Step 4: actual $n(NH_3) = 12.0 / 17.03 = 0.7046$ mol; percentage yield $= (0.7046 / 1.784) \times 100 = 39.5$ percent. The limiting reagent is $N_2$ and the percentage yield is 39.5 percent.
Q4: (a) Amphiprotic: $HSO_4^- + H_2O \rightarrow SO_4^{2-} + H_3O^+$ (acid) and $HSO_4^- + H_2O \rightarrow H_2SO_4 + OH^-$ (base, very minor). (b) Base: $NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-$ . (c) Amphiprotic: $HCO_3^- + H_2O \rightleftharpoons CO_3^{2-} + H_3O^+$ (acid) and $HCO_3^- + H_2O \rightleftharpoons H_2CO_3 + OH^-$ (base, dominant in aqueous solution).
Q5: (a) $Cu_{(s)} + 2Ag^+_{(aq)} \rightarrow Cu^{2+}_{(aq)} + 2Ag_{(s)}$ . (b) $E^{\circ}_{\text{cell}} = E^{\circ}_{\text{cathode}} - E^{\circ}_{\text{anode}} = +0.80 - (+0.34) = +0.46$ V. (c) The silver electrode is the cathode (higher reduction potential, reduction occurs there).
Q6: (a) 2-bromopropane (Markovnikov: H to the $CH_2$ carbon, Br to the more substituted central carbon). (b) Butan-2-one (secondary alcohol oxidises to ketone; reflux prevents loss of volatile product). (c) Propyl ethanoate plus water (Fischer esterification; concentrated $H_2SO_4$ is catalyst and dehydrating agent).
Q7: (a) (i) Increasing temperature shifts equilibrium in the endothermic (reverse) direction since the forward reaction is exothermic; yield of $NH_3$ decreases and $K_c$ decreases. (ii) Increasing pressure shifts equilibrium to the side with fewer moles of gas (4 mol reactants to 2 mol products), increasing $NH_3$ yield; $K_c$ unchanged. (iii) Iron catalyst does not shift the equilibrium position or alter $K_c$ ; it increases the rate at which equilibrium is established. (b) 450 degrees C and 200 atm are a compromise: theory predicts higher yield at lower temperature, but the rate is impractically slow below about 400 degrees C even with the iron catalyst. Higher pressures than 200 atm increase yield but escalate plant construction cost and risk. The Gladstone-style continuous process recycles unreacted $N_2$ and $H_2$ , so a moderate single-pass yield (around 15 percent) at higher rate is more economical than a higher yield at uneconomic rate.
Q8: Step 1: $E^{\circ}_{\text{cell}} = E^{\circ}_{\text{cathode}} - E^{\circ}_{\text{anode}}$ , so $E^{\circ}(M^{n+}/M) = E^{\circ}_{\text{cell}} + E^{\circ}(Zn^{2+}/Zn) = E^{\circ}_{\text{cell}} - 0.76$ . (a) $E^{\circ}(M1) = +1.10 - 0.76 = +0.34$ V; $E^{\circ}(M2) = +0.34 - 0.76 = -0.42$ V; $E^{\circ}(M3) = -0.42 - 0.76 = -1.18$ V. (b) Strongest oxidising agent first: $M1^{n+}$ ( $+0.34$ V) > $M2^{n+}$ ( $-0.42$ V) > $M3^{n+}$ ( $-1.18$ V). (c) M3 in $M1^{n+}$ solution: $E^{\circ}_{\text{cell}} = +0.34 - (-1.18) = +1.52$ V; positive, so the reaction is spontaneous and M3 will displace M1 from solution. (d) Mount Isa copper-lead-zinc ore processing relies on selective reduction: zinc metal displaces copper from copper sulfate leach solution because $E^{\circ}(Cu^{2+}/Cu) > E^{\circ}(Zn^{2+}/Zn)$ , allowing copper recovery before zinc electrowinning.

Sources & how we know this

Chemistry General senior syllabus 2025 — QCAA