A student adds different metal powders to copper(II) sulfate solution and measures the temperature rise. The same mass of metal, the same volume of solution and the same concentration are used each time.
Write the ionic equation for the reaction between magnesium and copper(II) ions. Include state symbols.
Explain, in terms of electrons, why this reaction is a redox reaction.
Identify the spectator ion in this reaction.
The table shows the results.
| Metal | Temperature rise / °C |
|---|---|
| iron | 3.5 |
| magnesium | 12.0 |
| silver | 0.0 |
| zinc | 6.5 |
Use the results to put the four metals in order of reactivity. Start with the most reactive.
Explain why there is no temperature rise with silver.
Write the half equation for the change that happens to zinc atoms when zinc is added to copper(II) sulfate solution.
45 exam-style questions on Edexcel GCSE Chemistry 5.1 Obtaining and using metals, covering 5.1.1 The reactivity series of metals, 5.1.2 Displacement reactions as redox reactions, 5.1.3 Extracting metals from ores by reduction, 5.1.4 Biological methods of metal extraction, 5.1.5 Resistance to oxidation and recycling metals, and 5.1.6 Life cycle assessment. Each one has a worked solution and a mark scheme showing where the marks go.