Asked by Amy
Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is
2C4H10(g) + 13O2(g)-> 8CO2(g)+ 10H2O(l)
At 1.00 atm and 23 degrees Celcius, what is the volume of carbon dioxide formed by the combustion of 1.80g of butane?
2C4H10(g) + 13O2(g)-> 8CO2(g)+ 10H2O(l)
At 1.00 atm and 23 degrees Celcius, what is the volume of carbon dioxide formed by the combustion of 1.80g of butane?
Answers
Answered by
DrBob222
mols butane = grams/molar mass.
Using the coefficients in the balanced equation, convert mols butane to mols CO2.
Use PV = nRT to solve for V of CO2 at the conditions listed in the problem. Remember T must be in kelvin, P in atm and V will be in L.
Using the coefficients in the balanced equation, convert mols butane to mols CO2.
Use PV = nRT to solve for V of CO2 at the conditions listed in the problem. Remember T must be in kelvin, P in atm and V will be in L.
Answered by
Anonymous
1.67 L
Answered by
khia
your all wrong
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