4.7


and

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Alicia Lin 2F
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Joined: Wed Sep 18, 2019 12:17 am

4.7

Postby Alicia Lin 2F » Thu Jan 30, 2020 10:28 pm

(a) Calculate the work that must be done against the atmosphere for the expansion of the gaseous products in the combustion of 1.00 mol C6H6(l) at 25°C and 1.00 bar.

I'm not really sure which work equation to use for this question.

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Re: 4.7

Postby Chem_Mod » Thu Jan 30, 2020 10:43 pm

The best one is to use w = -P(deltaV). However, we are not given change in volume, so you must calculate it using the Ideal gas law, in which PV = nRT. You can rearrange the equation to say V = nRT/P, but since we want the change in volume, we can say delta V = deltan(RT/P). I chose change in moles of gas because that is the quickest route (for 1 mol of C6H6 that is burned, what is the net change in moles of gas?). Substitute your unknowns into the work equation, and you will see that P cancels out, leaving you with work = -(delta n)RT.


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