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5.1 Monitoring chemical reactions

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Question 22
H

A student mixes 20 cm3\mathrm{cm^{3}}cm3 of methane with 100 cm3\mathrm{cm^{3}}cm3 of oxygen. The methane burns completely.

CH4(g)+2O2(g)→CO2(g)+2H2O(l) \mathrm{CH_{4}(g) + 2O_{2}(g) \rightarrow CO_{2}(g) + 2H_{2}O(l)} CH4​(g)+2O2​(g)→CO2​(g)+2H2​O(l)

All volumes are measured at room temperature and pressure.

What is the total volume of gas left at the end of the reaction?

[1]
A

20 cm3\mathrm{cm^{3}}cm3

B

60 cm3\mathrm{cm^{3}}cm3

C

80 cm3\mathrm{cm^{3}}cm3

D

120 cm3\mathrm{cm^{3}}cm3

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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