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 70% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 66000 kg coal that is 0.44 mass % sulfur?