A student added 1 g of four different metals to separate samples of copper sulfate solution. The starting temperature of the solution was 20.0 ∘C20.0\ ^\circ\text{C}20.0 ∘C each time.
Table: The highest temperature reached when 1 g of each metal was added to 50 cm3 of copper sulfate solution at a starting temperature of 20.0 ∘C20.0\ ^\circ\text{C}20.0 ∘C
| Metal | Highest temperature reached in ∘C^\circ\text{C}∘C |
|---|---|
| Magnesium | 46.5 |
| Zinc | 32.0 |
| Iron | 25.5 |
| Copper | 20.0 |
Calculate the temperature rise for zinc.
Give the metal that produced the smallest temperature rise, and give a reason for your answer.
All of the reactions that took place were exothermic. Explain what this tells you about the energy stored in the products compared with the energy stored in the reactants.
85 exam-style questions on AQA GCSE Chemistry 5.1 Exothermic and endothermic reactions, covering 5.1.1 Energy transfer during exothermic and endothermic reactions, 5.1.2 Reaction profiles, and 5.1.3 The energy change of reactions. Each one has a worked solution and a mark scheme showing where the marks go.