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3.3 Yield and atom economy of chemical reactions

3.3 Yield and atom economy of chemical reactions

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Question 10

Hydrogen gas can be produced industrially by the steam reforming of methane.

The equation for the reaction is:

CH4+H2O→CO+3H2 CH_4 + H_2O \rightarrow CO + 3H_2 CH4​+H2​O→CO+3H2​

Calculate the percentage atom economy for the production of hydrogen from this reaction.

Give your answer to 3 significant figures.

Use the equation:

Percentage atom economy=Total relative formula mass of desired productTotal relative formula mass of all reactants×100 \text{Percentage atom economy} = \frac{\text{Total relative formula mass of desired product}}{\text{Total relative formula mass of all reactants}} \times 100 Percentage atom economy=Total relative formula mass of all reactantsTotal relative formula mass of desired product​×100

Relative atomic masses (ArA_rAr​):

  • C=12C = 12C=12
  • H=1H = 1H=1
  • O=16O = 16O=16
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3.3 Yield and atom economy of chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /3.3 Yield and atom economy of chemical reactions

31 exam-style questions on AQA GCSE Chemistry 3.3 Yield and atom economy of chemical reactions, covering 3.3.1 Percentage yield and 3.3.2 Atom economy. Each one has a worked solution and a mark scheme showing where the marks go.

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