Final 2011 Question 1B Combustion of Methane


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Alex Nguyen 3I
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Final 2011 Question 1B Combustion of Methane

Postby Alex Nguyen 3I » Wed Mar 09, 2016 9:46 pm

Suppose 1.00 mol of methane is combusted irreversibly at constant room temperature (25 degrees C). Calculate the work associated with this process.

In the solution, it indicates the process as:
CH4(g) + 2O2(g) --> 2H2O(l) + CO2(g)
and that delta n(gas) = -2.00

Isn't H2O water vapor (gas) not liquid? If not, can someone explain why it's a liquid?

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Re: Final 2011 Question 1B Combustion of Methane

Postby Chem_Mod » Wed Mar 09, 2016 11:28 pm

It's because you're at room temperature.


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