A complete revision and exam practice pack for SC9c Moles, covering C4.8H–C4.11H. This is entirely Higher-tier content.

Topic Mastery Sheet (PDF) - a comprehensive student reference introducing the mole as the chemist’s counting unit: one mole of any substance contains 6.02 × 10²³ particles (the Avogadro constant) and has a mass equal to its Mr in grams. The three core relationships are presented in a clear formula table: n = m/Mr (moles from mass), N = n × Nₐ (particles from moles), and the combined form for particles directly from mass. Five fully worked examples. The limiting reactant section explains the concept clearly: the reactant that runs out first limits the amount of product formed; the other is in excess. The key method - convert both reactants to moles, compare relative to the mole ratio - is applied to the Zn/CuSO₄ experiment (zinc: 0.05 mol; CuSO₄: 0.0627 mol; 1:1 ratio → zinc is limiting → max Cu = 3.175 g) and to KOH/HNO₃ (0.1 mol KOH limits vs 0.15 mol HNO₃). The stretch section connects to A-level molar concentration (mol dm⁻³) and titration calculations.

Student Exam Practice Sheet (PDF + DOCX) - five questions (15 marks), all Higher tier: mole definition and moles of water in 27 g, three separate mole calculations (mass, molecules and moles from particle count), the full Zn + CuSO₄ limiting reactant analysis (four parts), KOH + HNO₃ limiting reactant and mass of KNO₃, and determining the balanced equation from the NaCl + AgNO₃ experimental data.

Teacher Answer Key (PDF + DOCX) - full worked mark scheme with all numerical answers and reasoning for the limiting reactant and stoichiometry questions.

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