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Limestone (CaCO3) is used to remove acidic pollutants from smokestack flue gases. It 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 9.2 X 10^4 kg of coal that is 0.33 mass % sulfur? I need it to be in correct sig figs. So 2 because of the numbers in the question.

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