Iron powder reacts with dilute sulfuric acid. Fe(s) + H₂SO₄(aq) → FeSO₄(aq) + H₂(g) (a) The graph shows the volume of hydrogen gas produced at 20°C as the reaction proceeds. [Figure 3.1]

1. (a)(i)State how long it takes from the start of the experiment to collect 18cm³ of hydrogen gas.[1]
2. (a)(ii)The experiment is repeated at 30°C. All other conditions are the same. Draw a line on the grid to show how the volume of hydrogen gas produced changes with time when the reaction is done at 30°C.[2]
3. (b)(i)Describe and explain, using ideas about collisions between particles, how the rate of the reaction changes when the temperature of the reaction mixture is increased. All other conditions are the same.[2]
4. (b)(ii)Describe and explain, using ideas about collisions between particles, how the rate of the reaction changes when larger pieces of iron are used. All other conditions are the same.[2]
5. (c)Calculate the maximum volume, in dm³, of hydrogen formed when 3.36g of iron react with excess dilute sulfuric acid at room temperature and pressure. Give your answer to three significant figures. maximum volume =[2]
6. (d)Concentrated sulfuric acid is an oxidising agent. Describe a test for oxidising agents. test observations[2]

This question uses a diagram from the original paper, which isn't shown here. Open the full paper from the past papers archive to see it.