Calcualte `q, w, DeltaU`, and `DeltaH` for the reversible isothermal expansion of one mole of an ideal gas at `127^(@)C` from a volume of `20dm^(3)` to `40dm^(3)`.

Calcualte `q, w, DeltaU`, and `DeltaH` for the reversible isothermal e

1.	Calcualte `q, w, DeltaU`, and `DeltaH` for the reversible isothermal expansion of one mole of an ideal gas at `127^(@)C` from a volume of `20dm^(3)` to `40dm^(3)`.
Answer» Since the process is isothermal, `DeltaU = DeltaH = 0` From first law of thermodynamics, `DeltaU = q +w = 0` `q =- w` `w =- 2.303 nRT log ((V_(2))/(V_(1)))` `=- 2.303 xx1xx 8.314 xx 400 "log" (40)/(20)` `=- 2.303 xx1xx 8.314 xx 400 xx 0.3010` `=- 2305.3J` (work is done by the system) `q =- w = 2305.3J` (Heat is abosrbed by the system)

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Calcualte `q, w, DeltaU`, and `DeltaH` for the reversible isothermal expansion of one mole of an ideal gas at `127^(@)C` from a volume of `20dm^(3)` to `40dm^(3)`.

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