Asked by Mary
What is the volume of the oxygen produced when 1.00L carbon dioxide reacts with 20.0 g of Na2O2 based on the following unbalanced reaction at 25C and 2.00 bar?
Na2O2 + CO2 -> O2 + Na2CO3
R = 0.083145 L bar K-1 mol-1
I got 1.57L but the answer is 500mL
Na2O2 + CO2 -> O2 + Na2CO3
R = 0.083145 L bar K-1 mol-1
I got 1.57L but the answer is 500mL
Answers
Answered by
DrBob222
It would have been so much easier if you had shown your work; then I could have found your error.
First, you didn't balanced the equation.
2Na2O2 + 2CO2 ==> O2 + 2Na2CO3
mols Na2O2 = grams/molar mass = ? I have approx 0.3 but that's just an estimate.
Use PV = nRT and solve for mols CO2. I have approx 0.04, again an estimates as are all of the other numbers I quote.
Did you calculate that CO2 was the limiting reagent. It is.
Using the coefficients in the balanced equation, convert mols CO2 to mols O2. I get approx 0.02
Then use PV = nRT and calculate volume. I get 0.5L which is 500 cc.
First, you didn't balanced the equation.
2Na2O2 + 2CO2 ==> O2 + 2Na2CO3
mols Na2O2 = grams/molar mass = ? I have approx 0.3 but that's just an estimate.
Use PV = nRT and solve for mols CO2. I have approx 0.04, again an estimates as are all of the other numbers I quote.
Did you calculate that CO2 was the limiting reagent. It is.
Using the coefficients in the balanced equation, convert mols CO2 to mols O2. I get approx 0.02
Then use PV = nRT and calculate volume. I get 0.5L which is 500 cc.
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