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4FeS2 + 11O2 > 2Fe2O3 + 8SO2

Given 75.0 grams of iron (IV) sulfide, how many grams of sulfur dioxide are produced?

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  1. Today, 01:39
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    80.13g of SO2

    Explanation:

    4FeS2 + 11O2 - > 2Fe2O3 + 8SO2

    Molar Mass of FeS2 = 55.8 + (2x32) = 119.8g/mol

    Mass of FeS2 from the balanced equation = 4 x 119.8 = 479.2

    Molar Mass of SO2 = 32 + (16x2) = 32 + 32 = 64g/mol

    Mass of SO2 from the balanced equation = 8 x 64 = 512g

    From the equation,

    479.2g of FeS2 produced 512g of SO2.

    Therefore, 75g of FeS2 will produce = (75 x 512) / 479.2 = 80.13g of SO2
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