Asked by Tsunayoshi
a.Given the equation: 2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2 What is the actual yield of CO2 if 7.5 mol of O2 gives a percent yield of 80%?
b. The pollutant sulfur dioxide can be removed from the emissions of an industrial plant by the reaction with calcium carbonate and oxygen. 2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2 If this reaction proceeds with a 96.8% yield, how many kilograms of calcium sulfate are formed when 5.24 kg of sulfur dioxide reacts with an excess of calcium carbonate and oxygen gas?
b. The pollutant sulfur dioxide can be removed from the emissions of an industrial plant by the reaction with calcium carbonate and oxygen. 2CaCO3 + 2SO2 + O2 -> 2CaSO4 + 2CO2 If this reaction proceeds with a 96.8% yield, how many kilograms of calcium sulfate are formed when 5.24 kg of sulfur dioxide reacts with an excess of calcium carbonate and oxygen gas?
Answers
Answered by
DrBob222
How much CO2 should you obtain?
That's 7.5 mol O2 x (2 mols CO2/1 mol O2) = 7.5 x 2 = 15 mols CO2 = theoretical yield
Then %yield = (Actual/theoretical)*100
80 = (Actual/15)*100
Actual = ?
That's 7.5 mol O2 x (2 mols CO2/1 mol O2) = 7.5 x 2 = 15 mols CO2 = theoretical yield
Then %yield = (Actual/theoretical)*100
80 = (Actual/15)*100
Actual = ?
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