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
61–70 of 71 · Normal
Question 61
4 marks · Normal
Answer and see the solution →The diagram shows an iron pipeline buried underground with blocks of magnesium attached at intervals.
(a)[2 marks]Explain why the magnesium blocks must be more reactive than iron in order to protect the pipeline from rusting.
(b)[2 marks]Explain what happens to the magnesium during this process.
Question 62
3 marks · Normal
Answer and see the solution →A ship’s iron hull is protected from rusting by sacrificial anodes. Each anode is made from magnesium and has a mass of 6 kg. Over a year, each anode loses 1.5 kg of magnesium.
(a)[1 mark]State one structure, apart from a ship, that is protected by sacrificial anodes.
(b)[2 marks]Calculate the percentage of magnesium lost from each anode in a year.
Question 63
3 marks · Normal
Answer and see the solution →Rusting occurs when iron is exposed to air and water. Ships are often fitted with blocks of zinc on their hulls.
(a)[3 marks]Explain, using the ideas of oxidation and reactivity, how these zinc blocks prevent the iron hull from rusting.
Question 64
4 marks · Normal
Answer and see the solution →A scientist is choosing a metal to protect an iron water tank from rusting. She tests three metals (A, B, and C), each attached to iron and left in moist air. The results are shown below.
Results: Rusting of iron with different metals attached Metal attached Observation after 1 month A Iron is rusted; attached metal is not corroded B Iron is shiny; attached metal is heavily corroded C Iron is rusted; attached metal is also rusted (a)[2 marks]Which metal, A, B, or C, acts as a sacrificial anode for iron? Explain your answer.
(b)[2 marks]Explain, using the observations, why the chosen metal must be more reactive than iron.
Question 65
1 mark · Normal
Answer and check →Which structure is commonly protected using sacrificial anodes made of zinc or magnesium?
- A.Aluminium can
- B.Underground oil pipeline
- C.Plastic water bottle
- D.Glass window
Question 66
2 marks · Normal
Answer and see the solution →State what is meant by a sacrificial anode, and name a metal commonly used as one to protect iron.
Question 67
4 marks · Normal
Answer and see the solution →A section of an underwater steel bridge has several aluminium blocks attached to it.
(a)[2 marks]Explain why aluminium is able to protect the steel from rusting by sacrificial protection.
(b)[2 marks]Describe what happens to the aluminium blocks over time and why they are eventually replaced.
Question 68
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 69
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 70
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.