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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 1
61%

Nitrogen and hydrogen react to produce ammonia.

The equation for the reversible reaction is:

nitrogen+hydrogen⇌ammonia \text{nitrogen} + \text{hydrogen} \rightleftharpoons \text{ammonia} nitrogen+hydrogen⇌ammonia

The reaction has a maximum theoretical yield of 500 kg500\text{ kg}500 kg of ammonia. A chemical plant actually produces 425 kg425\text{ kg}425 kg of ammonia.

Calculate the percentage yield of ammonia.

Use the equation:

percentage yield=mass of ammonia actually mademaximum theoretical mass of ammonia×100 \text{percentage yield} = \frac{\text{mass of ammonia actually made}}{\text{maximum theoretical mass of ammonia}} \times 100 percentage yield=maximum theoretical mass of ammoniamass of ammonia actually made​×100
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Markscheme

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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