Look at the equations for the reactions that happen at each electrode of an alkaline hydrogen-oxygen fuel cell.
Reaction 1: H2(g)+2OH−(aq)→2H2O(l)+2e−\text{H}_2(\text{g}) + 2\text{OH}^-(\text{aq}) \rightarrow 2\text{H}_2\text{O}(\text{l}) + 2\text{e}^-H2(g)+2OH−(aq)→2H2O(l)+2e−
Reaction 2: O2(g)+2H2O(l)+4e−→4OH−(aq)\text{O}_2(\text{g}) + 2\text{H}_2\text{O}(\text{l}) + 4\text{e}^- \rightarrow 4\text{OH}^-(\text{aq})O2(g)+2H2O(l)+4e−→4OH−(aq)
| Reaction 1 | Reaction 2 | |
|---|---|---|
| A | Reduction because electrons are lost | Oxidation because electrons are gained |
| B | Oxidation because electrons are lost | Reduction because electrons are gained |
| C | Oxidation because electrons are gained | Reduction because electrons are lost |
| D | Reduction because electrons are gained | Oxidation because electrons are lost |
Which row of the table, A, B, C or D, is correct about reactions 1 and 2?
Row A
Row B
Row C
Row D
34 exam-style questions on OCR GCSE Chemistry Electrolysis. Each one has a worked solution and a mark scheme showing where the marks go.