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5.1 Monitoring chemical reactions

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Question 8
F

A chemist reacts 6.0 g of hydrogen with excess nitrogen to make ammonia.

N2+3H2⇌2NH3 \mathrm{N_{2} + 3H_{2} \rightleftharpoons 2NH_{3}} N2​+3H2​⇌2NH3​

The chemist collects 20.4 g of ammonia.

Relative atomic mass (ArA_rAr​): H = 1.0 N = 14.0

What is the percentage yield of ammonia?

[1]
A

29.4%

B

30.0%

C

40.0%

D

60.0%

Markscheme

5.1 Monitoring chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /5.1 Monitoring chemical reactions

57 exam-style questions on OCR GCSE Chemistry 5.1 Monitoring chemical reactions, covering 5.1.1 The technique of titration, 5.1.2 Theoretical mass, percentage yield and atom economy, 5.1.3 Concentration of a solution in mol/dm3, 5.1.4 Concentration calculations and titration results, 5.1.5 Molar gas volume and volumes of gases in reactions, and 5.1.6 Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.

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