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5.1 Monitoring chemical reactions

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Question 4

An iron sample is added to excess dilute hydrochloric acid. The iron reacts according to the equation:

Fe+2HCl→FeCl2+H2 \mathrm{Fe + 2HCl \rightarrow FeCl_{2} + H_{2}} Fe+2HCl→FeCl2​+H2​

The reaction produces 0.840 dm3\mathrm{dm^{3}}dm3 of hydrogen 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​): Fe = 55.8

What mass of iron has reacted?

[1]
A

0.977 g

B

1.95 g

C

3.91 g

D

0.0350 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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