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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 1

Magnesium oxide is produced by burning magnesium in oxygen gas.

The equation for the reaction is:

2Mg+O2→2MgO 2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO} 2Mg+O2​→2MgO

Calculate the volume of oxygen gas needed to react completely with 6.0 g6.0\text{ g}6.0 g of magnesium.

You should calculate:

  • the number of moles of magnesium used
  • the number of moles of oxygen gas that react with 6.0 g6.0\text{ g}6.0 g of magnesium
  • the volume of oxygen gas needed.

Relative atomic mass (ArA_rAr​): Mg=24\text{Mg} = 24Mg=24

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

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Markscheme

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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