Hey, I was wondering if anyone here could solve this chemistry problem, because I got pretty far on it, but now I’m stuck. %|

Anyway, it’s for extra credit, and my chemistry professor said I could use ANY source…

Okay, here it is:

A cylinder contains 3.00 g of liquid octane(C8H18 and an initial O2 pressure of 1.00 atm. The cylinder is fitted with a piston and initially occupies a volume of 10.00 L at 298 Kelvin. The octane is completely consumed by the reaction. Approximate that the piston is massless and frictionless and that the cylinder neither absorbs or releases heat. Calculate the final volume occupied by the cylinder.

Okay, so I am just assuming that this is an ideal gas, using PV=nRT and such, and I’ve already figured out the initial and final states of the stuff. Here it is:

Initial Volume: 10.00 L

Initial Pressure: 1 atm

Initial Temp: 298 K

Initial # of mols of gas: 0.409 mol

The balanced reaction: C8H18(liquid) + 25/2O2(gas) --> 8CO2(gas) + 9H2O(gas)

Final number of mols of stuff:

O2: 0.0802

CO2: 0.2104

H2O: 0.2367

I can’t seem to figure out how to get the final heat, though…

Anyway, If you think you can solve it, please, try!