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3.2 Use of amount of substance in relation to masses of pure substances

3.2 Use of amount of substance in relation to masses of pure substances

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Question 22

In the industrial Claus process, hydrogen sulfide gas (H2S\text{H}_2\text{S}H2​S) reacts with sulfur dioxide gas (SO2\text{SO}_2SO2​) to produce solid sulfur and water vapour.

The equation for the reaction is:

2H2S(g)+SO2(g)→3S(s)+2H2O(g) 2\text{H}_2\text{S}(\text{g}) + \text{SO}_2(\text{g}) \rightarrow 3\text{S}(\text{s}) + 2\text{H}_2\text{O}(\text{g}) 2H2​S(g)+SO2​(g)→3S(s)+2H2​O(g)

60 cm360\text{ cm}^360 cm3 of H2S\text{H}_2\text{S}H2​S is reacted with 45 cm345\text{ cm}^345 cm3 of SO2\text{SO}_2SO2​.

Calculate the total volume of gases present after the reaction is complete.

All volumes of gases are measured at the same temperature and pressure. Assume the temperature is high enough that water remains in the gas phase.

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3.2 Use of amount of substance in relation to masses of pure substances Questions

  1. GCSE
  2. /Chemistry
  3. /3.2 Use of amount of substance in relation to masses of pure substances

38 exam-style questions on AQA GCSE Chemistry 3.2 Use of amount of substance in relation to masses of pure substances, covering 3.2.1 Moles (HT only), 3.2.2 Amounts of substances in equations (HT only), 3.2.3 Using moles to balance equations (HT only), 3.2.4 Limiting reactants (HT only), and 3.2.5 Concentration of solutions. Each one has a worked solution and a mark scheme showing where the marks go.

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