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    6.27g of magnesium carbonate were added to an excess of sulphuric acid. The following reaction occurred:
    MgCO3 + H2SO4 ---> MgSO4 +CO2 +H20

    Calculate the mass of MgSO4 produced assuming a 95% yield.

    Moles of MgCO3 = 0.0744

    I got all the calculations correct but why is it 8.958g x 95% / 100

    Doesnt make sense to me, could someone explain it please?

    So, once you have calculated the mass of MgSO4 from a perfect 100% yield (8.958), you have to take into account that the percentage yield is not 100, but 95%. Therefore, you can either multiply it by 0.95 (95% expressed as a decimal) or by 95, then divide by 100 (which is the same process, just doing it in two steps).
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Updated: January 2, 2013
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