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9 October, 17:23

Acrylonitrile (C3H3N) Is The Starting Material For Many Synthetic Carpets And Fabrics. It Is Produced By The Following Reaction: 2C3H6 (g) + 2NH3 (g) + 3O2 (g) = 2C3H3N (g) + 6H2O (g) If 15.0 G C3H6, 10.0 G O2, And 5.00 G NH3 Are Reacted, What mass of the acrylonitrile can be produced assuming 100% yield?

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  1. 9 October, 20:03
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    11.072 g

    Explanation:

    2 C3H6 (g) + 2NH3 (g) + 3O2 (g) = 2C3H3N (g) + 6H2O (g)

    molar mass of Acrylonitrile (C3H3N) = 53.06 g/mol

    molar mass of C3H6 = 42.08 g/mol =

    molar mass of NH3 = 17.031 g/mol

    molar mass of O2 = 15.999 g/mol

    mole of C3H6 = 15 g / 42.08 g/mol = 0.3565 mol

    mole of NH3 = 5 g / 17.031 g/mol = 0.294 mol

    mole of O2 = 10 g / (15.999 x 2g/mol) = 0.313

    finding the limiting reagent be comparing the mole

    2 mole of C3H6 react with 2 mole of NH3 and 3 mole of O2 to yield 2 mole of C3H3N

    0.209 mole of C3H6 react with 0.209 mole of NH3 and 0.313 oxygen

    mass of Acrylonitrile (C3H3N) = 53.06 g/mol * 0.209 mol = 11.072 g
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