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6 November, 16:44

1. Starting with 9.3 moles of O2, how many moles of H2S will be needed and how many moles of SO2 will

be produced in the following reaction? SHOW YOUR WORK!

2 H2S + 3 O2 - > 2 SO2 + 2 H2O

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  1. 6 November, 17:12
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    6.2 moles of H₂S of moles are needed.

    6.2 moles of SO₂ are produced.

    Explanation:

    Reaction: 2 H₂S + 3 O₂ → 2SO₂ + 2H₂O

    2 moles of hydrogen sulfide can react to 3 moles of oxygen in order to produce 2 moles of sulfur dioxide and 2 moles of water.

    We propose the following rule of three:

    If 3 moles of oxygen need 2 moles of H₂S to react

    Then, 9.3 moles of O₂ will react with (9.3. 2) / 3 = 6.2 moles of H₂S

    3 moles of O₂ can produce 2 moles of SO₂

    So, 9.3 moles will produce (9.3. 2) / 3 = 6.2 moles of SO₂

    If we take account the 6.2 moles of H₂S (the value we obtained), we get the same answer: 6.2 moles of SO₂. This is because ratio is 2:2
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