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CHEM1011 · Chemistry 1a

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Chapter 12 of 12 · CHEM1011

Exam Technique and Final Revision

Week 10 consolidates the whole course for the in-person final exam (40%): how to use the supplied Periodic Table and Data Sheet, how to handle the mix of question styles and lengths, and which Mastery topics — Rydberg spectra, MO diagrams, van 't Hoff and Nernst — appear only here. It maps every syllabus unit back to the assessment that tests it and rehearses the cross-topic links (ΔG° ↔ K ↔ E°cell) that distinguish a strong exam script.

In this chapter

What this chapter covers

01Using the supplied Periodic Table and Data Sheet: constants and equations are given, so the marks are in applying them
02Handling a mix of question styles and lengths under time pressure; budgeting time in proportion to marks
03Mastery-only exam topics: Rydberg equation, MO diagrams and bond order, van 't Hoff, Nernst
04Cross-topic links: equilibrium ↔ acids/bases; thermodynamics ΔG° ↔ K ↔ E°cell (the van 't Hoff bridge)
05IMFs ↔ physical properties ↔ solubility and thermodynamics
06Mapping each of the eight syllabus topics to the component that assesses it
07Rehearsing with the provided mock/practice paper and the tutorial problem sets
08Answer conventions: correct units, log answers to the right decimal places, rounding once at the end

Worked example · free

Cross-topic revision: the equilibrium constant from ΔG°

Q [4 marks]. A reaction has ΔG° = −32.0 kJ mol⁻¹ at 298 K. Using ΔG° = −RT ln K with R = 8.314 J mol⁻¹ K⁻¹, calculate the equilibrium constant K and comment on whether products or reactants are favoured. (4 marks)

+1Rearrange ΔG° = −RT ln K for the constant: ln K = −ΔG°/(RT). Convert ΔG° to joules: −32.0 kJ mol⁻¹ = −32000 J mol⁻¹.
+1Evaluate RT = 8.314 × 298 = 2477 J mol⁻¹.
+1ln K = −(−32000)/2477 = 32000/2477 = 12.9.
+1K = e^12.9 = 4.0 × 10⁵. A large K (≫ 1) means products are strongly favoured, consistent with the negative ΔG°.

ln K = −ΔG°/(RT) = 32000/(8.314 × 298) = 12.9, so K = e^12.9 = 4.0 × 10⁵. K ≫ 1, so the reaction is product-favoured — exactly what a negative ΔG° predicts.

Sia tip — This is the ΔG° ↔ K bridge the exam loves — and it extends to E°cell through ΔG° = −nFE°cell, so all three quantities agree on spontaneity. Convert ΔG° to joules before dividing by RT, and sanity-check the sign: negative ΔG° must give K > 1. Ask Sia to continue the chain and find the E°cell that corresponds to this ΔG° for a two-electron cell.

Glossary

Key terms

Data Sheet: The Periodic Table plus the sheet of constants (Nₐ, R, F, h, c, R_H) and standard equations (pV = nRT, the Rydberg, Nernst, Henderson–Hasselbalch, van 't Hoff and Gibbs relations) provided in the in-term tests and the final exam, so you apply formulas rather than memorise them. It does not carry tables of Ka/pKa or standard reduction potentials — those values are normally given in the question.
Mastery exam topic: Merit-level content assessed only in the 40% final exam — including the Rydberg equation, MO diagrams and bond order, the van 't Hoff equation and the Nernst equation — rather than in the weekly quizzes.
The ΔG°–K–E°cell bridge: The set of links ΔG° = −RT ln K and ΔG° = −nFE°cell that tie thermochemistry, equilibrium and electrochemistry together; the van 't Hoff equation extends this to the temperature dependence of K.
Time-per-mark budgeting: Allocating exam time in proportion to the marks on each question, so a long structured question gets more time than a single multiple-choice item; confirm the total mark count and duration on Moodle.
Cross-topic question: An exam item that spans several topics (e.g. computing K from ΔG°, then E°cell), rewarding students who can move between the thermodynamic, equilibrium and electrochemical descriptions of the same reaction.
Answer conventions: The UNSW marking expectations: state units, give a log answer to as many decimal places as the input has significant figures, treat exact numbers as non-limiting, and round only at the final step.

FAQ

Exam Technique and Final Revision FAQ

What is on the CHEM1011 final exam and how is it structured?

It is a single in-person paper worth 40%, held in the UNSW examination period, spanning all eight topics with a mix of question styles and lengths. It is where the Mastery content is assessed — Rydberg spectra, MO diagrams and bond order, van 't Hoff and Nernst appear here rather than in the weekly quizzes. A Periodic Table and Data Sheet is provided. The exact duration and section structure are released in Week 9, so confirm the details on Moodle and the UNSW exam timetable.

Which topics only appear in the final exam?

The Mastery-flagged material: the Rydberg equation and full energy-level analysis, molecular-orbital diagrams and bond order, the van 't Hoff temperature dependence of K, the Nernst equation and concentration cells, and the deeper treatments of Raoult's law, Hess/Born–Haber cycles and titration/speciation curves. The weekly quizzes and in-term tests stay at Threshold level, so save exam-only practice for these Mastery items.

How should I use the supplied Data Sheet effectively?

Because the constants and standard equations are given, the marks are in choosing the right formula and applying it with correct units — not in recall. Before the exam, practise from the actual sheet so you know exactly what is provided (and what is not, such as specific Ka or E° values you may be given in the question). Then in the exam, quote the relevant equation, substitute with units, and round once at the end following the UNSW answer conventions.

Can Sia help me revise across topics for the final?

Yes. Sia can drill the cross-topic bridges the exam favours — computing K from ΔG° and then E°cell, or moving between IMFs and physical properties — and generate fresh practice in the paper's mix of styles, checking your working step by step. It explains methods and checks reasoning; it does not do graded assessment, and the UNSW academic-integrity policy applies.

Study strategy

Exam move

Revise for the final by mapping, not re-reading: build a one-page grid linking each of the eight topics to the component that tests it, and flag the Mastery-only items (Rydberg, MO diagrams, van 't Hoff, Nernst) for focused exam practice since they never appeared in the weekly quizzes. Rehearse from the actual Data Sheet so you know what is supplied and can go straight to applying formulas with correct units. Prioritise the cross-topic bridges the paper rewards — ΔG° ↔ K ↔ E°cell, equilibrium ↔ acids/bases, IMFs ↔ properties — because being able to move between descriptions of one reaction distinguishes a strong script. Work the provided mock/practice paper under timed conditions, budgeting time in proportion to marks, and drill the answer conventions (units, log decimal places, round once). Keep the standard diagrams (energy levels, VSEPR, MO, titration curves, galvanic cells) exam-ready. Confirm the exam date, duration, room and permitted materials on Moodle and the UNSW exam timetable once released in Week 9. When a cross-topic chain won't connect, ask Sia to walk it end to end.

Working through Exam Technique and Final Revision in CHEM1011? Sia is AskSia’s AI Chemistry tutor — ask any CHEM1011 Exam Technique and Final Revision question and get a clear, step-by-step explanation grounded in how CHEM1011 is taught and assessed. Read this chapter free, then take your hardest questions to Sia.

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