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
51–60 of 374 · Normal
Question 51
3 marks · Normal
Answer and see the solution →A student adds chlorine water to 40.0 cm³ of potassium iodide solution and observes the solution turns brown because iodine is produced. Assume the following equation:
The concentration of the potassium iodide solution is 0.20 mol/dm³.
(a)[1 mark]Calculate the number of moles of potassium iodide present in 40.0 cm³ of the solution. Give your answer to 2 significant figures.
(b)[1 mark]Using the equation above, calculate the maximum number of moles of iodine that can be produced from this amount of potassium iodide. Give your answer to 2 significant figures.
(c)[1 mark]State the observation you would expect if bromine water was added to potassium chloride solution instead of chlorine water to potassium iodide solution.
Question 52
2 marks · Normal
Answer and see the solution →Write the ionic equation, with state symbols, for the displacement reaction between bromine water and potassium iodide solution.
Question 53
4 marks · Normal
Answer and see the solution →Chlorine water is added to a solution of potassium bromide.
(a)[1 mark]State what you would see when chlorine water is added to potassium bromide solution.
(b)[2 marks]Explain why this reaction is an example of a redox reaction. Refer to oxidation and reduction in your answer.
(c)[1 mark]Name the oxidising agent in this reaction.
Question 54
3 marks · Normal
Answer and see the solution →Explain, in terms of electron transfer, why iodine does not displace bromine from a solution of potassium bromide. Include references to oxidation and reduction in your answer.
Question 55
4 marks · Normal
Answer and see the solution →The table shows observations from adding different halogen solutions to various potassium halide solutions:
Results of mixing halogen solutions and potassium halide solutions Halogen solution Potassium halide solution Observation Chlorine Potassium iodide Brown solution formed Bromine Potassium chloride No change Iodine Potassium bromide No change Chlorine Potassium bromide Orange solution formed (a)[1 mark]Identify which pairs in the table show a displacement reaction.
(b)[2 marks]For one of the pairs that show a displacement, write the ionic equation for the reaction.
(c)[1 mark]Explain why no change is observed in the reaction between bromine and potassium chloride.
Question 56
1 mark · Normal
Answer and check →Which statement correctly explains why chlorine acts as an oxidising agent in its reaction with bromide ions?
- A.It loses electrons and is oxidised itself.
- B.It gives electrons to bromide ions.
- C.It gains electrons and is reduced.
- D.It forms a brown solution.
Question 57
2 marks · Normal
Answer and see the solution →Complete the ionic equation for the reaction between bromine and sodium iodide solution. Include state symbols.
Question 58
4 marks · Normal
Answer and see the solution →Two students discuss the reaction between chlorine and potassium iodide solution.
(a)[2 marks]Write the ionic equation for this reaction, including state symbols.
(b)[2 marks]Explain, using the meanings of oxidation and reduction, which substance is oxidised and which is reduced in this reaction.
Question 59
3 marks · Normal
Answer and see the solution →Chlorine gas is bubbled through a solution of sodium iodide. Write the balanced ionic equation for this reaction. Show, with working, the steps you use to remove spectator ions from the full ionic equation.
Question 60
2 marks · Normal
Answer and see the solution →State two trends that occur when you go down Group 7 (the halogens) in the Periodic Table.