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3.3 Yield and atom economy of chemical reactions

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Question 17

Hydrogen chloride is produced at a chemical plant by combining hydrogen with chlorine.

H2+Cl2→2HCl\text{H}_2 + \text{Cl}_2 \rightarrow 2\text{HCl}H2​+Cl2​→2HCl

For one batch, 7.10 tonnes of chlorine entered the reactor. Hydrogen was supplied in excess.

Relative atomic masses: H=1\text{H} = 1H=1, Cl=35.5\text{Cl} = 35.5Cl=35.5.

a.

Use the equation to calculate the greatest possible mass of hydrogen chloride from this batch. Give your answer in tonnes.

[3]
b.

Only 6.57 tonnes of hydrogen chloride entered the storage vessel. Calculate the percentage yield for the batch.

[2]
c.

All the chlorine reacted and no products from unwanted side reactions were detected. Give one reason why less hydrogen chloride reached the storage vessel than the equation predicts.

[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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