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    Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 74.7% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 90000 kg coal that is 0.42 mass % sulfur?

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    mass of Sulfur =90000*(0.42/100) = 378 kg

    CaO + SO2 --> CaS


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