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Determine the value of DeltaH and DeltaU...

Determine the value of `DeltaH` and `DeltaU` for the reversible isothermal evaporation of `90.0g` of water at `100^(@)C`. Assume that water behaves as an ideal gas and heat of evaporation of water is `540 cal g^(-1) (R = 2.0 cal mol^(-1)K^(-1))`.

Text Solution

Verified by Experts

`{:(,Water,hArr,Vapour,),(Mol e b ef o re evapo ration,90//18=5,,0,):}`
The evaporation of `5 mol e` of water takes place reversibly and isothermally into vapours.
Thus, heat give at constant pressure
`DeltaH=` heat of evaporation `xx` amount evaporated
`DeltaH=540xx90=48600cal`
Also `DeltaH=DeltaU+DeltanRT`
`DeltaU=48600-5xx1xx2xx373`
`=486003730`
`DeltaU=44870cal`
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Determine the value of DeltaH and DeltaU for the reversible isothermal evaporationof 90.0 g of water at 100^(@)C . Assume that water vapour behave as an ideal gas and heat of evaporation of water is 540 cal g^(-1) ( R = 2.0 cal mol^(-1)K^(-1))

Determine the value of DeltaH and DeltaU for the reversible isothermal evaporation of 90.0g of water at 100^(@)C .Assume that water vapour behaves as an ideal gas and heat of evaporation of water is 540 calg^(-)R = 2.0 cal mol^(-1)K^(-1) .

Knowledge Check

  • What is the value of DeltaE for reversible isothermal evaporation of 90 g water at 100^(@) C? Assuming water vapour behaves as an ideal gas, DeltaH_(vap,water) = 540 calsg^(-1)

    A
    `9 xx 10^(3)` cals
    B
    `6 xx 10^(3)` cals
    C
    `4.49` cals
    D
    none of the above

  • What is the value of DeltaE (heat change at constant volume)for reversible isothermal evaporation of 90g water at 100^(@)C Assuming water vapour behaves as an ideal gas and (DeltaH_("vap"))_("water")=540calg^(-1)

    A
    `9xx10^(3)cal`
    B
    `6xx10^(3)cal`
    C
    `4.49cal`
    D
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  • The entropy change accompanying the evaporation of 1 mole of water at 100^(@)C , assuming that the latent heat of vaporisation of water is 540"cal"g^(-1) , in cal/K/mole is

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    B
    25
    C
    26.06
    D
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