[Hazelhaze]

Hello everyone, I'm new to this forum and am in need of a little verification for my final lab report due in a couple days.
Basically, we just filled a 2L coke bottle with Ethanol, and another with Methanol, burned them, and calculated the moles/combustion efficency/percentage yield of water/etc.
I came here for assistance because I noticed my numbers are abnormally high, and I'm wondering if I entered something incorrectly, or if I'm using the wrong formula to determine the actual moles.

We were given the pressure and temperature, and the volume of the coke bottle I put my Ethanol in was 2150 mL.
I also have here that the water vapor leftover from the combustion of ethanol was 1.2 mL.

Using PV = nRT I determined the moles of Ethanol to be 8.78 x 10¹ which seemed high to begin with. Then, I determined the mass to be 4045.824g (?). Here are my calculations.

PV = nRT
= 100.08 kPa ( 2150mL) = n (8.314 kpA-L / mol-k) (297.65 k)
= 101.08(2159) / (8.314)(297.65k) = n
n = 8.78 x 10¹ mol

Then, the molar mass of Ethanol was 46.08 g/mol so I multiplied it by 8. 78 x 10¹ mol to get 4045.824g.

Any assistance on this would be great, as right now I'm just a little puzzled by what I've gone and done wrong. Thanks for your *delete me* =]

[Hazelhaze]

Oh wow. I apologize to this entire forum for having wasted your time with my stupidity =/. I now realize I should of just converted the 2150 mL into liters so that I actually obtain reasonable data for my experiment.

Thanks for taking the time to read this, sorry for wasting it >_<.