Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Reactivity Series
163 practice questions
Topics covered
- Displacement reactions involving metal oxides20 practice questions
- Oxidation and reduction19 practice questions
- Displacement reactions involving solutions of salts19 practice questions
- Reactions of metals with water18 practice questions
- Reactions of metals with dilute acids19 practice questions
- Making predictions using the reactivity series19 practice questions
- Preventing rusting by galvanising21 practice questions
- Preventing rusting by using sacrificial protection18 practice questions
Practice questions
151–160 of 163
Question 151
2 marks · Hard
Answer and see the solution →Explain why a block of copper cannot be used as a sacrificial anode to protect iron from rusting.
Question 152
5 marks · Hard
Answer and see the solution →An engineer is tasked with protecting an iron pipeline buried underground using the method of sacrificial protection.
(a)[2 marks]Explain why sacrificial anodes must be made of a metal more reactive than iron.
(b)[2 marks]The engineer is considering aluminium, tin, and silver as possible metals for sacrificial anodes. Aluminium is above iron in the reactivity series, tin is just below iron, and silver is far below iron. Which of these metals could be used as sacrificial anodes for the pipeline? Justify your choice.
(c)[1 mark]Describe what happens to the chosen sacrificial anode metal over time.
Question 153
2 marks · Hard
Answer and see the solution →State one example of a structure (not previously listed in examples) that can be protected from rusting using sacrificial anodes, and name a suitable metal that could be used as the sacrificial anode for this structure.
Question 154
5 marks · Easy
Answer and see the solution →(a)[1 mark]The reactivity series below shows the order of metals from most to least reactive. Potassium, Sodium, Lithium, Calcium, Magnesium, Zinc, Iron, Copper.
Arrange the following three metals in order of reactivity, from most reactive to least reactive: magnesium, copper, iron.
(b)[1 mark]Iron(III) oxide reacts with aluminium powder when heated.
Write a word equation for this reaction.
(c)[2 marks]Explain which substance is oxidised and which substance is reduced in this reaction, in terms of oxygen transfer.
(d)[1 mark]In the reaction above, which metal is displaced from its oxide?
Question 155
5 marks · Easy
Answer and see the solution →(a)[1 mark]State what is meant by a displacement reaction involving a metal oxide.
(b)[2 marks]When carbon is heated with iron(III) oxide, the following reaction occurs:
Identify which substance is reduced in this reaction and explain your answer in terms of oxygen transfer.
(c)[1 mark]Name one use of carbon as a reducing agent in industry.
(d)[1 mark]Explain why carbon cannot be used to extract magnesium from magnesium oxide.
Question 156
5 marks · Easy
Answer and see the solution →A student heats a mixture of powdered aluminium and iron(III) oxide. The following reaction occurs:
(a)[2 marks]Use the reactivity series to explain why this reaction occurs. Identify which metal is displaced and why.
(b)[3 marks]In terms of electron transfer, describe what happens to aluminium and what happens to iron(III) oxide in the reaction above. Use your answer to part (a) to help you.
Question 157
6 marks · Normal
Answer and see the solution →This question is about metals reacting with both solutions of salts and with water.
(a)[1 mark]State the general equation for the reaction of a metal with cold water.
(b)Iron does not react with cold water, but does react with copper(II) sulfate solution.
(i)[2 marks]Write the ionic equation for the reaction between iron and copper(II) sulfate solution.
(ii)[1 mark]Give a reason why iron reacts with copper(II) sulfate solution but not with cold water.
(c)[2 marks]Potassium reacts vigorously with cold water. Complete the ionic equation for this reaction and identify the gas produced:
Question 158
6 marks · Normal
Answer and see the solution →Some metals react with dilute hydrochloric acid at different rates. The reactivity series can be used to predict how metals behave in these reactions.
(a)[1 mark]A student adds small pieces of magnesium, iron, and copper to separate test tubes containing dilute hydrochloric acid. State the trend in reactivity observed for these three metals with dilute acids.
(b)[1 mark]Give one observation the student would make when magnesium reacts with dilute hydrochloric acid.
(c)[2 marks]Results for the reaction of metals with dilute hydrochloric acid Metal Temperature change / °C Magnesium 21 Zinc 7 Iron 4 Copper 0 Using the data in the table, identify the most reactive and the least reactive metal.
(d)[2 marks]A new, unfamiliar metal 9 is found to react with dilute hydrochloric acid and produces a temperature change greater than zinc but less than magnesium. Predict, using the reactivity series, where 9 would be placed relative to magnesium and zinc. Explain your answer.
Question 159
6 marks · Normal
Answer and see the solution →A student investigates how three different metals react with dilute sulfuric acid. The student uses equal moles of each metal under the same conditions.
(a)[1 mark]Temperature change when metals react with dilute sulfuric acid Metal Temperature change / °C Zinc 9 Iron 5 Copper 0 Use the data to arrange the three metals from most reactive to least reactive with dilute sulfuric acid.
(b)[2 marks]Write a balanced chemical equation (with state symbols) for the reaction between zinc and dilute sulfuric acid.
(c)[2 marks]Explain why the student must use the same number of moles, rather than the same mass, of each metal to fairly compare their reactivity.
(d)[1 mark]A metal called cobalt is placed between iron and copper in the reactivity series. Predict whether cobalt will react with dilute sulfuric acid under the same conditions. Give a reason for your answer.
Question 160
6 marks · Normal
Answer and see the solution →A student investigates the reaction between metals and dilute hydrochloric acid. She uses 0.010 mol of each metal and measures the temperature change during the reaction. Her results are shown below:
Temperature changes when metals react with dilute hydrochloric acid. Metal Initial temperature / C Maximum temperature / C Magnesium 20 42 Zinc 20 28 Iron 20 24 Copper 20 20 Another metal, chromium, is placed between iron and zinc in the reactivity series.
(a)[2 marks]Calculate the temperature rise for each metal. Complete the table below.
Add the temperature rise for each metal. Metal Temperature rise / C Magnesium Zinc Iron Copper (b)[2 marks]Based on your answers to part a, describe and explain the trend in reactivity of these metals with dilute hydrochloric acid.
(c)[2 marks]Predict the temperature rise the student would expect if she repeated the experiment using 0.010 mol of chromium. Explain your answer.