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Calculateq, W, DeltaU and DeltaH for the...

Calculate`q, W, DeltaU` and `DeltaH` for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of `1.0` bar to a final pressure of `0.1` bar at a constant temperature of `273K.`

Text Solution

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For isothermal reversible expansion, `w=-2.303 nRT log (P_(1)/P_(2))`
`=-2.303 xx 1 xx 8.314 xx 273 xx log (1.0/0.1)`
`=-5227.2` J
At constant temperature, for expansion `DeltaT =0`, therefore `DeltaE=0`
Also, `DeltaE = 1 xx C_(v) xx DeltaT=0`. (for 1 mol)
`DeltaE = q+w`
`therefore q=-W = 5227.2` J
Also, when temeprature is constant, `P_(1)V_(1) = P_(2)V_(2)`
`DeltaH = DeltaE + Delta(PV)`
`therefore DeltaH=0`
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Calculate q, W, DeltaU and DeltaH for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0bar to a final pressure of 0.1bar at a constant temperature of 273K .

Calculate Q,W,DeltaE and DeltaH for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of1.0 bar to a final pressure of0.1 bar at a constant temperature of273 K.

Knowledge Check

  • Calculate Q and w for the isothermal reversible expansion of one mole an ideal gas from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at a constant temperature of 273 K respectively.

    A
    5.22kJ, -5.22 kJ
    B
    `-5.22 kJ, 5.22 kJ`
    C
    27.3 kJ, -27.3 kJ
    D
    `-27.3 kJ, 27.3 kJ`

  • 1 mole of an ideal gas is expanded from an initial pressure of 1 bar to final pressure of 0.1 bar at constant temperature of 273 K. Predict which of the following is not true?

    A
    `Delta`E = 0
    B
    `Delta`H = 0
    C
    PV is constant
    D
    `Delta S larr 0`

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