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3.3 Yield and atom economy of chemical reactions

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Question 7

Iron sulfide is made in a reaction represented by

Fe+S→FeS\text{Fe} + \text{S} \rightarrow \text{FeS}Fe+S→FeS

A batch is started with 11.2 g of iron and 9.60 g of sulfur. The batch produces 14.1 g of iron sulfide.

Relative atomic masses: Fe=56\text{Fe} = 56Fe=56, S=32\text{S} = 32S=32.

a.

Calculate the maximum theoretical mass of iron sulfide, in g\text{g}g, that could be obtained from this batch.

[5]
b.

Calculate the percentage yield for this batch. Give your answer to 3 significant figures.

[2]
c.

Give one reason why the mass of iron sulfide collected is less than the maximum theoretical mass.

[1]
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

104 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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