Work and ideal gas law


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WYacob_2C
Posts: 102
Joined: Sat Jul 20, 2019 12:16 am

Work and ideal gas law

Postby WYacob_2C » Sat Feb 01, 2020 1:33 am

Can someone explain the relationship between work and the ideal gas law? I believe a problem was done in class where work was found using the ideal gas law. Thank you in advance.

Anika Chakrabarti 1A
Posts: 102
Joined: Sat Aug 24, 2019 12:17 am

Re: Work and ideal gas law

Postby Anika Chakrabarti 1A » Sat Feb 01, 2020 9:10 am

The ideal gas law is PV = nRT, and work is equal to -P(change in V). So, if you know the number of moles and the temperature of a reaction, you can solve for work using the idea that work = -nRT. I think there was an example of this in Friday's lecture.

Alex Chen 2L
Posts: 86
Joined: Wed Sep 18, 2019 12:21 am

Re: Work and ideal gas law

Postby Alex Chen 2L » Sun Feb 02, 2020 2:10 pm

In the example we did in class, we had an exothermic reaction with ΔH = -50kJ occuring in an open beaker producing net 8 moles of gas at 25C, and we had to calculate the change in internal energy. Since ΔU = ΔH - PΔV, we had to use the ideal gas law to calculate PΔV, setting it equal to ΔnRT since the volume and number of moles of gas changed. You would then get PΔV equal to 20 kJ and therefore ΔU = -50 - 20 = -70 kJ.

Ashley Wang 4G
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Joined: Wed Sep 11, 2019 12:16 am

Re: Work and ideal gas law

Postby Ashley Wang 4G » Sun Feb 02, 2020 8:03 pm

Work = -P ∆V when the external pressure is constant.
By the ideal gas law, PV = nRT, and P∆V = ∆(nRT)
So any work done under constant pressure = - ∆(nRT), where the change in volume can result from a change in the number of moles of gas (∆n) or a change in the temperature (∆T).

005384106
Posts: 101
Joined: Sat Aug 24, 2019 12:16 am

Re: Work and ideal gas law

Postby 005384106 » Tue Feb 04, 2020 9:33 pm

How do I know when I need to use the ideal gas law?


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