Asked by Kenneth
A o.8378g sample of calcium oxalate is heated to 1000°C.(a) calculate the moles of CaO remaining after ignition .(b)calculate the millimoles of CO evolved. (C) Calculate the weight of CO2 produced.
Answers
Answered by
DrBob222
Stepwise:
CaC2O4 (s) → CaCO3 s + CO (g)
CaCO3(s) ==> CaO(s) + CO2(g)
Total reaction:
CaC2O4 ==> CaO + CO + CO2
mols CaC2O4 = grams/molar mass = 0.8378/128 = 0.00654
Notice 1 mol CaC2O4 produces 1 mjol CO2 and 1 mol CO so
0.00654 mola CaC2O4 will produce 0.00654 mols CO and 0.00654 mols CO2.
mllimols CO = mols CO x 1000 = ?
mass CO2 = mols CO2 x molar mass CO2 = ?
CaC2O4 (s) → CaCO3 s + CO (g)
CaCO3(s) ==> CaO(s) + CO2(g)
Total reaction:
CaC2O4 ==> CaO + CO + CO2
mols CaC2O4 = grams/molar mass = 0.8378/128 = 0.00654
Notice 1 mol CaC2O4 produces 1 mjol CO2 and 1 mol CO so
0.00654 mola CaC2O4 will produce 0.00654 mols CO and 0.00654 mols CO2.
mllimols CO = mols CO x 1000 = ?
mass CO2 = mols CO2 x molar mass CO2 = ?
Answered by
Manuel John
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