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6.4 Chemical cells and fuel cells

6.4 Chemical cells and fuel cells

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Question 2
H

A hydrogen-oxygen fuel cell produces 36 g of 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)

Relative atomic masses: H = 1, O = 16. One mole of any gas occupies 24 dm3\mathrm{dm^{3}}dm3 at room temperature and pressure.

What is the total volume of gas (hydrogen plus oxygen), measured at room temperature and pressure, used by the cell?

[1]
A

96 dm396\,\mathrm{dm^{3}}96dm3

B

72 dm372\,\mathrm{dm^{3}}72dm3

C

48 dm348\,\mathrm{dm^{3}}48dm3

D

36 dm336\,\mathrm{dm^{3}}36dm3

Markscheme

6.4 Chemical cells and fuel cells Questions

  1. GCSE
  2. /Chemistry
  3. /6.4 Chemical cells and fuel cells

42 exam-style questions on Edexcel GCSE Chemistry 6.4 Chemical cells and fuel cells, covering 6.4.1 Chemical cells and fuel cells. Each one has a worked solution and a mark scheme showing where the marks go.

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