Two mole of ideal diatomic gas `(C_(v.m)= 5//2 R)` at 300 K and 5 atm expanded irreversibly to a final pressue of 2atm against a constant pressue of 1

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Two mole of ideal diatomic gas `(C_(v.m)= 5//2 R)` at 300 K and 5 atm expanded irreversibly to a final pressue of 2atm against a constant pressue of 1

Two mole of ideal diatomic gas `(C_(v.m)= 5//2 R)` at 300 K and 5 atm expanded irreversibly
to a final pressue of 2atm against a constant pressue of 1 atm . Calculate q,w,`DeltaH` & `DeltaU`.

Monjur Alahi

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2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Salim Ahmed Kawsar

Correct Answer - `DeltaU = w = - 1247.1 ; DeltaH = - 1745.94J`
` w =nC_(V) (T_(2)- T_(1)) =- P_("ext")[(nRT_(2))/(P_(2))(nRT_(1))/(P_(1))]`
`T_(2) = 370 K`
`w= nC_(V) (T_(2)- T_(1)) =- 1247.1 J`
`q=0`
`DeltaU = w`
`DeltaH = DeltaU + nRDeltaT =- 1745.94J`

5 views Answered 2023-02-05 15:29