Internal energy

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Internal energy

Postby Stevin1H » Thu Mar 14, 2019 1:16 am

Can someone explain the concept behind when the change in internal energy would be equal to 0?

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Re: Internal energy

Postby Karishma_1G » Thu Mar 14, 2019 1:31 am

Delta U for an isothermal reversible expansion is zero. These types of reactions usually take place in a heat reservoir. The energy that is lost when the system does work is replaced by heat energy from the surroundings. Therefore q and w are equal in magnitude and opposite in sign; q is positive since heat is coming into the system and w is negative since work is being done by the system. So when you add q and w to get delta U, it is zero.

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Re: Internal energy

Postby CHEM 14B Lover » Thu Mar 14, 2019 2:31 pm

"The energy lost as work is replaced by heat"; but you say these reactions normally happen in a heat bath? What if there isn't a heat bath? Would it simply not be isothermal reversible?

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