Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Inorganic Chemistry
869 practice questions
Topics covered
- The Alkali Metals85 practice questions
- The Halogens86 practice questions
- Gases in the Atmosphere86 practice questions
- Reactivity Series163 practice questions
- Extraction and Uses of Metals128 practice questions
- Acids, Alkalis and Titrations83 practice questions
- Acids, Bases and Salt Preparations156 practice questions
- Chemical Tests68 practice questions
Practice questions
171–180 of 374 · Normal
Question 171
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 172
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 173
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 174
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 175
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 176
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 177
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.
Question 178
2 marks · Normal
Answer and see the solution →State the meaning of:
(a)[1 mark]An ore.
(b)[1 mark]A native metal.
Question 179
4 marks · Normal
Answer and see the solution →The list shows three metals in order of reactivity:
Gold Iron Aluminium
(a)[1 mark]Which metal is most likely to be found in the Earth's crust as the uncombined element? Explain your answer.
(b)[1 mark]State one common ore of iron.
(c)[1 mark]Describe the method used to extract iron from its ore.
(d)[1 mark]Explain why aluminium must be extracted by a different method than iron.
Question 180
3 marks · Normal
Answer and see the solution →Explain, using the reactivity series, why gold can be found as a pure metal in the Earth's crust but magnesium cannot.