Work through the list without notes. If you cannot do a statement, follow its link, then come back. Guide = study guide; Practice = practice questions.
Understanding
- I can explain what a standard reduction potential measures and why the hydrogen half-cell is set at 0.00 V. (Guide: “Standard reduction potentials”)
- I can say which of two half-reactions runs as the reduction in a galvanic cell by comparing their E° values. (Guide: Figure 1; Practice Q1, Q4)
- I can explain that a positive E°cell means a thermodynamically favoured reaction, and a negative E°cell means an applied potential is needed. (Guide: “The sign of E°cell”; Practice Q3)
- I can explain why E° does not change when an equation is multiplied, but ΔG° does. (Guide: “Do not multiply E° by coefficients”; Practice Q6)
Calculation
- I can calculate E°cell = E°(cathode) − E°(anode) without multiplying by coefficients or changing a sign twice. (Guide: Worked example 1; Practice Q1)
- I can find n from the electrons that cancel in a balanced overall equation. (Guide: Worked example 1; Practice Q2)
- I can calculate ΔG° from E° with ΔG° = −nFE° and give the answer in kJ mol⁻¹ with the correct sign. (Practice Q2, Q4)
- I can work backwards from ΔG° or a measured cell potential to an unknown reduction potential. (Guide: Worked example 3; Practice Q5)
Reasoning
- I can use E° and ΔG° together to decide whether a proposed redox reaction is thermodynamically favoured. (Guide: Worked example 2; Practice Q5(c))
- I can explain why recharging a cell needs an applied potential larger than the cell’s own E°. (Practice Q7)
- I can state that a favourable E° tells me nothing about how fast a reaction goes. (Guide: “Common misconceptions”)
All ticked? Move on to Topic 9.10, Cell Potential Under Nonstandard Conditions, or return to the course roadmap.