# Enthalpy and stoichiometry

by Agent M27
Tags: enthalpy, stoichiometry
 P: 171 1. The problem statement, all variables and given/known data The change in internal energy for the combustion of 1.0 mol of octane at a pressure of 1.0 atm is 5084.5 Kj. If the change in enthalpy is 5074.2 Kj, how much work is done during the combustion? Find work in Kj. 2. Relevant equations $$\Delta$$E=$$\Delta$$H + (-P$$\Delta$$V) w=-P$$\Delta$$V 3. The attempt at a solution $$\Delta$$E=5084.5Kj $$\Delta$$H=5074.2Kj 5084.5-5074.2=-1atm($$\Delta$$V) -10.3=$$\Delta$$V w=-(1)(-10.3)=10.3 10.3L*atm x 101.3J=1043.39J $$\frac{1043.39}{1000}$$= 1.04339 Kj This is an online homework set, so when I input the answer it usually will give me a hint if I am close, but I am not getting anything. Can anyone spot my error? Thanks in advance. Joe
 P: 1 I don't know if you have already figured this out, but I thought I'd let you know I found your problem. The way you solved it, your change in volume ended up in kJ/atm when it should be in liters. I just did a track and took 10300J and divided it by 101.3 J to end up with about 101.68 L. 10.3kJ/atm x 1000J/1kJ x 1 Latm/101.3J= 101.68 L. Hopefully that helped if you haven't already figured it out!

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