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Upon decomposition, one sample of magnesium fluoride produced 1.65kg of magnesium and 2.58kg of fluorine. A second sample produce 1.38kg of magnesium. How much fluorine (in grams) did the second sample produce?

  • chemistry -

    The ratio of Mg to F is constant.

    f2 / m2 = f1 / m1

    To find the second mass of fluorine (f2),
    rearrange and substitute appropriate values.

  • chemistry -

    F/Mg = 2.58/1.65
    So, given 1.28kg Mg, we should have

    1.28*(2.58/1.65) = 2.00kg F

  • chemistry -

    You need to create an identity to solve for the mass of fluorine:

    1.65 kg of Mg=2.58 kg of F


    1.38 kg of Mg=x kg of F


    x kg of F/1.38kg of Mg=2.58 kg of F/1.65 kg of Mg

    Solve for x kg of F,

    x kg of F=(2.58 kg of F/1.65 kg of Mg)*1.38kg of Mg

    x kg of F=2.157Kg of F

    2.157 kg of F*(10^3g/1kg )=2.16 x 10^3 g of F or 2,160 g of F

    Answer contains 3 sig figs.

  • chemistry -


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