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5.1 Monitoring chemical reactions

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Question 23

Hydrogen reacts with oxygen to produce liquid water.

2H2(g)+O2(g)→2H2O(l) \mathrm{2H_{2}(g) + O_{2}(g) \rightarrow 2H_{2}O(l)} 2H2​(g)+O2​(g)→2H2​O(l)

Measurements show that the reaction consumes 0.840 dm3\mathrm{dm^{3}}dm3 of oxygen at room temperature and pressure.

One mole of any gas occupies 24 dm3\mathrm{dm^{3}}dm3 at room temperature and pressure.

Relative atomic mass (ArA_rAr​): H = 1.0

What mass of hydrogen reacted?

[1]
A

0.0350 g

B

0.0700 g

C

0.140 g

D

0.280 g

Markscheme

5.1 Monitoring chemical reactions Questions

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

152 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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