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3.2 Use of amount of substance in relation to masses of pure substances

3.2 Use of amount of substance in relation to masses of pure substances

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Question 2

Iron reacts with chlorine gas to produce iron(III) chloride.

The balanced equation for the reaction is:

2Fe(s)+3Cl2(g)→2FeCl3(s) 2\text{Fe(s)} + 3\text{Cl}_2\text{(g)} \rightarrow 2\text{FeCl}_3\text{(s)} 2Fe(s)+3Cl2​(g)→2FeCl3​(s)

Calculate the volume of chlorine gas needed to react completely with 11.2 g11.2\text{ g}11.2 g of iron.

You should calculate:

  • the number of moles of iron used
  • the number of moles of chlorine gas that react with 11.2 g11.2\text{ g}11.2 g of iron
  • the volume of chlorine gas needed.

Relative atomic mass (ArA_rAr​): Fe=56\text{Fe} = 56Fe=56

The volume of 1 mole of gas = 24 dm324\text{ dm}^324 dm3

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3.2 Use of amount of substance in relation to masses of pure substances Questions

  1. GCSE
  2. /Chemistry
  3. /3.2 Use of amount of substance in relation to masses of pure substances

38 exam-style questions on AQA GCSE Chemistry 3.2 Use of amount of substance in relation to masses of pure substances, covering 3.2.1 Moles (HT only), 3.2.2 Amounts of substances in equations (HT only), 3.2.3 Using moles to balance equations (HT only), 3.2.4 Limiting reactants (HT only), and 3.2.5 Concentration of solutions. Each one has a worked solution and a mark scheme showing where the marks go.

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