School / IB / CHEMISTRY HL / Reactivity 3: electron transfer (HL) Exam-style + marking analysis
Reactivity 3: electron transfer (HL) Standard electrode potentials, cell EMF and electrolysis calculations using Faraday's law.
16 activities ≈ 32 minutes
Chemistry HL Reactivity 3: electron transfer (HL)
View All Incomplete Complete
Revision Ladder All stages Easy Medium HardSoon
1 Define oxidation and reduction in terms of electron transfer. ✓ Reviewed Easy 2 marks No calculator + 2 Marking analysis: A learner attempts the following task: “Define oxidation and reduction in terms of electron transfer.” Their response addresses only this point: “States that oxidation is the loss of electrons by a species.” Evaluate the response against the complete 2-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Easy 2 marks No calculator + 3 Using standard electrode potentials E°(Cu²⁺/Cu) = +0.34 V and E°(Zn²⁺/Zn) = −0.76 V, calculate E°cell for the reaction Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), stating which half-cell is the cathode. ✓ Reviewed Medium 4 marks Calculator + 4 Marking analysis: A learner attempts the following task: “Using standard electrode potentials E°(Cu²⁺/Cu) = +0.34 V and E°(Zn²⁺/Zn) = −0.76 V, calculate E°cell for the reaction Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), stating which half-cell is the cathode.” Their response addresses only this point: “Identifies the Cu²⁺/Cu half-cell as the cathode, since it has the more positive (less negative) standard electrode potential.” Evaluate the response against the complete 4-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Medium 4 marks Calculator + 5 State how the sign of E°cell indicates whether a redox reaction is spontaneous under standard conditions, and hence state whether the reaction between Zn(s) and Cu²⁺(aq) is spontaneous, given E°cell = +1.10 V. ✓ Reviewed Easy 2 marks No calculator + 6 Marking analysis: A learner attempts the following task: “State how the sign of E°cell indicates whether a redox reaction is spontaneous under standard conditions, and hence state whether the reaction between Zn(s) and Cu²⁺(aq) is spontaneous, given E°cell = +1.10 V.” Their response addresses only this point: “States that a positive E°cell indicates a spontaneous (feasible) reaction under standard conditions, while a negative E°cell indicates a non-spontaneous one.” Evaluate the response against the complete 2-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Easy 2 marks No calculator + 7 A current of 2.00 A is passed through molten lead(II) bromide, PbBr₂(l), for 1930 seconds using inert electrodes. Calculate the number of moles of electrons transferred. (F = 96500 C mol⁻¹) ✓ Reviewed Medium 4 marks Calculator + 8 Marking analysis: A learner attempts the following task: “A current of 2.00 A is passed through molten lead(II) bromide, PbBr₂(l), for 1930 seconds using inert electrodes. Calculate the number of moles of electrons transferred. (F = 96500 C mol⁻¹)” Their response addresses only this point: “States the formula for charge: Q = It.” Evaluate the response against the complete 4-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Medium 4 marks Calculator + 9 Using n(e⁻) = 0.0400 mol from the electrolysis of molten PbBr₂, calculate the mass of lead deposited at the cathode. (Pb²⁺ + 2e⁻ → Pb; Ar(Pb) = 207) ✓ Reviewed Easy 3 marks Calculator + 10 Marking analysis: A learner attempts the following task: “Using n(e⁻) = 0.0400 mol from the electrolysis of molten PbBr₂, calculate the mass of lead deposited at the cathode. (Pb²⁺ + 2e⁻ → Pb; Ar(Pb) = 207)” Their response addresses only this point: “States that 2 moles of electrons are required per mole of Pb deposited, from Pb²⁺ + 2e⁻ → Pb.” Evaluate the response against the complete 3-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Easy 3 marks Calculator + 11 Explain why the standard hydrogen electrode (SHE) is assigned a standard electrode potential of exactly 0.00 V, and outline why this matters for tabulating other electrode potentials. ✓ Reviewed Easy 3 marks No calculator + 12 Marking analysis: A learner attempts the following task: “Explain why the standard hydrogen electrode (SHE) is assigned a standard electrode potential of exactly 0.00 V, and outline why this matters for tabulating other electrode potentials.” Their response addresses only this point: “States that the SHE is an arbitrary but universally agreed reference electrode.” Evaluate the response against the complete 3-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Easy 3 marks No calculator + 13 Aqueous copper(II) sulfate is electrolysed using inert (platinum) electrodes. Identify the products formed at the cathode and the anode, and explain why OH⁻ ions rather than SO₄²⁻ ions are discharged at the anode. ✓ Reviewed Medium 4 marks No calculator + 14 Marking analysis: A learner attempts the following task: “Aqueous copper(II) sulfate is electrolysed using inert (platinum) electrodes. Identify the products formed at the cathode and the anode, and explain why OH⁻ ions rather than SO₄²⁻ ions are discharged at the anode.” Their response addresses only this point: “States that copper metal, Cu(s), is deposited at the cathode, since Cu²⁺ is preferentially reduced over H⁺ (Cu²⁺/Cu has the more positive standard electrode potential).” Evaluate the response against the complete 4-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Medium 4 marks No calculator + 15 Two electrolytic cells are connected in series: one containing molten PbBr₂ and one containing molten AlCl₃, both electrolysed for the same time with the same current. Deduce which cell deposits more moles of metal, Pb or Al, and explain your reasoning. (Pb²⁺ + 2e⁻ → Pb; Al³⁺ + 3e⁻ → Al) ✓ Reviewed Easy 3 marks No calculator + 16 Marking analysis: A learner attempts the following task: “Two electrolytic cells are connected in series: one containing molten PbBr₂ and one containing molten AlCl₃, both electrolysed for the same time with the same current. Deduce which cell deposits more moles of metal, Pb or Al, and explain your reasoning. (Pb²⁺ + 2e⁻ → Pb; Al³⁺ + 3e⁻ → Al)” Their response addresses only this point: “States that cells connected in series carry the same current, so the same quantity of charge (and hence the same number of moles of electrons) passes through both.” Evaluate the response against the complete 3-mark task. Identify what earns credit and state every additional requirement needed for full marks. ✓ Reviewed Marking analysis Easy 3 marks No calculator + Self-assessed 0 / 0
Set total 50
This is a self-study tool, not official marking or a predicted IB grade.
Progress is saved on this device. Sign in to sync across devices. Reset progress
Before you practise
Questions learners ask about this practice Are these official IB questions? No. These are original SubjectScout practice questions for Reactivity 3: electron transfer (HL). They are not official past-paper questions or endorsed material.
What does this Chemistry HL practice page include? It includes selected topic questions, marking points, and feedback prompts designed to help learners practise before requesting teacher support.
Can I request a teacher for this exact topic? Yes. Tell SubjectScout the subject, exact topic, level and deadline, and the team will try to match you with a suitable verified teacher.
Request a teacher for Reactivity 3: electron transfer (HL) Unofficial content under accuracy, provenance, and rights review. Not affiliated with or endorsed by the International Baccalaureate Organization. Official past-paper questions are not reproduced here.
