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3.3 Yield and atom economy of chemical reactions

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Question 11
H

Carbon disulfide is made by reacting methane with sulfur.

CH4+2S→CS2+2H2S\text{CH}_4 + 2\text{S} \rightarrow \text{CS}_2 + 2\text{H}_2\text{S}CH4​+2S→CS2​+2H2​S

Relative atomic masses: H=1\text{H} = 1H=1, C=12\text{C} = 12C=12, S=32\text{S} = 32S=32.

a.

Calculate the percentage atom economy for the production of carbon disulfide.

[3]
b.

The hydrogen sulfide made in this reaction is used to make sulfuric acid. Explain how this affects the proportion of the reactants that is wasted.

[2]
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

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

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