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Two mole of ideal diatomic gas (C("v,m")...

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

Text Solution

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The correct Answer is:
`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`
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2 moles of an ideal diatomic gas (C_(V)=5//2R) at 300 K, 5 atm expanded irreversibly and adiabatically to a final pressure of 2 atm against a constant pressure of 1 atm. (1) Calculate final temperature q, w, DeltaH&DeltaU (2) Calculate corresponding values if the above process is carried out reversibly.

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  • One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas :

    A
    270 K
    B
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    C
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    D
    200 K

  • One mole of a ideal gas (C_(v,m)=5/2R) at 300 K and 5 at m is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is:

    A
    270K
    B
    273K
    C
    248.5K
    D
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  • One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

    A
    270 K
    B
    273 K
    C
    248.5 K
    D
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