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21 May, 10:40

how many grams of iron will be required to release all the antimony from 10 grams of antimony trisulfide? iron 2 sulfide is also formed

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  1. 21 May, 13:11
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    mass of Fe = 4.86 g

    Explanation:

    Balanced chemical equation

    Sb₂S₃ + 3Fe → 2Sb + 3FeS

    Given data from eq.

    moles of iron = 3 mol

    mas of iron = ?

    moles of antimony trisulfide = 1 mol

    mass of antimony trisulfide = 10 g

    Solution

    1st we will find out the mole ratio of Sb₂S₃ and Fe from balanced chemical equation

    Sb₂S₃ : Fe

    1 : 3

    Now we find out number of moles of citric acid Sb₂S₃ from the given mass

    moles = mass / molar mass

    moles = 10 g / 339.7 g/mol

    moles = 0.029 mol

    Now we find out moles (x) of iron needed for 0.029 mol of antimony trisulfide

    from the balanced chemical equation the mole ratios are:

    1 : 3

    0.029 : x

    Cross multiply these ratios

    3 * 0.029 = 1x

    0.087 = 1 x

    x = 0.087 mol

    Now we will find out the mass of iron

    mass = moles * molar mass

    mass of Fe = 0.087 mol * 55.845 g/mol

    mass of Fe = 4.86 g
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