[elfishies]

Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of methane.
(Assume standard state conditions and 298 K for all reactants and products.) *note:its reaction with O2(g) forms the products CO2(g) and H2O(l).*

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What I did:
The balanced equation I got for the combustion of methane is CH4(g)+2O2(g)->CO2(g)+2H2O(l)

Δn = 1-(2+1) = -2 since liquids are neglected
using the Ideal gas law: ΔPV=ΔnRT
ΔPV=(-2)(8.3145)(298) = -4955.442 kJ but the answer turned out to be wrong

Can anyone tell me how to solve this problem? thanks!

[elfishies]

nevermind, i got it!!

[mjc123]

Yes. Did you solve that monatomic ideal gas one?