If the reaction below proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.97 kg SO2 reacts with an excess of CaCO3 and O2?
2 CaCO3(s) + 2 SO2(g) + O2(g) 2 CaSO4(g) + 2 CO2(g)

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  1. first convert the kg of SO2 to grams of SO2 then convert to moles by dividing by its molar mass

    secondly convert between moles of 2SO2 and 2CaSO4 which is a 2/2 ration so no change in moles

    then multiply your moles by CaSO4's molar mass to get grams, then multiply that amount by 96.8% (.968) to get a 96.8% yeild of CaSO4's grams and convert to kg by dividing by 1000

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