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4 March, 19:52

A 43.56 gram sample of iron is heated in the presence of excess sulfur. A metal sulfide is formed with a mass of 81.08 g. Determine the empirical formula of the metal sulfide.

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  1. 4 March, 22:25
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    Fe2S3

    Explanation:

    Data obtained from the question include:

    Mass of Fe = 43.56g

    Mass of metal sulfide = 81.08g

    Next we shall determine the mass of sulphur, S in the compound. This is illustrated below:

    Mass of S = Mass of metal sulfide - mass of Fe

    Mass of S = 81.08 - 43.56 = 37.52g

    The empirical formula for the metal sulfide can be obtain as follow:

    Fe = 43.56g

    S = 37.52g

    Divide by their molar mass

    Fe = 43.56/56 = 0.7779

    S = 37.52/32 = 1.1725

    Divide by the smallest

    Fe = 0.7779/0.7779 = 1

    S = 1.1725/0.7779 = 1.5

    Multiply through by 2 to express in whole number

    Fe = 1 x 2 = 2

    S = 1.5 x 2 = 3

    Therefore, the empirical formula for the metal sulfide is Fe2S3
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