Question

How many liters of Carbon Dioxide are formed by burning 6011.0 grams of C3H7OH with excess of oxygen gas and is carried out at 20.00 degrees Celsius, and 1.150 atm of pressure.
I know this needs PV=nRT but the burning and excess part is throwing me off. Please help me learn how to do this!
2C3H7OH + 9O2 ==> 6CO2 + 8H2O

mols C3H7OH = grams/molar mass = ?
Using the coefficients in the blanced equation, convert mols C3H7OH to mols CO2.
Now convert mols CO2 to L by
PV = nRT using the conditions of the problem.

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