Home
Class 12
CHEMISTRY
The latent heat of vaporisation of water...

The latent heat of vaporisation of water at `100 ^(@)C` is `540 cal g^(-1)`. Calculate the entropy increase when one mole of water at `100^(@)C` is evaporated

A

`26 cal K^(-1) mol^(-1)`

B

`1.82 cal K^(-1) mol^(-1)`

C

`367 cal K^(-1) mol^(-1)`

D

`540xx18 cal K^(-1) mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
A
`DeltaS=(DeltaH_(vap))/(T)=(540xx18)/(373)`
`=26 cal K^(-1) mol^(-1)`
`(DeltaH_(vap) "for" 1 "mole"=540xx18)`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • CHEMICAL KINETICS

    DINESH PUBLICATION|Exercise Additional Numerical Problems For Practice|16 Videos

  • CHEMISTRY IN EVERY DAY LIFE

    DINESH PUBLICATION|Exercise Unit test-9|50 Videos

Similar Questions

Explore conceptually related problems

Boiling point of an aqueous solution is 100.1^(@)C . Latent heat of fusion and latent heat of vaporisation of water are "80 cal g"^(-1) and "540 cal g"^(-1) respectively. Calculate the freezing point of the solution.

One moles of strem is compressed reversibly of water at boiling point 100^(@)C . The heat of vapourisation of water at 100^(@)C and 1atm is 540cal g^(-1) . Calculate DeltaU and DeltaH .

Knowledge Check

  • Latent heat of vaporisation of water is 540cal g^(-1) at 100^(@)C calculate the entropy change when 1000 g water is converted to steam at 100^(@)C

    A
    1447 cal
    B
    2447 cal
    C
    3447 cal
    D
    4447 cal

  • Latent heat of fusion of ice is 0.333 kJ g^(-1) . The increase in entropy when 1 mole water melts at 0^(@)C will be

    A
    `21.96 kJ ^(-1) mol^(-1)`
    B
    `21.98 kcal K ^(-1) mol^(-1)`
    C
    `21.96 J K ^(-1) mol^(-1)`
    D
    `21.98 cal K ^(-1) mol^(-1)`

  • The work done by the system in the conversion of 1 mol of water at 100 ^(@)C and 760 torr to steam is -3.1 kJ . Calculate the DeltaE for the conversion (Latent heat of vaporisation of water is 40.65 kJ mol^(-1) )

    A
    `43.75 kJ`
    B
    `101.35 kJ`
    C
    `37.55 kJ`
    D
    `-40.65 kJ`

    • Similar Questions

    Explore conceptually related problems

    What is the amount of heat required (in calories) to convert 10 g of ice at -10^(@)C into steam at 100^(@)C ? Given that latent heat of vaporization of water is "540 cal g"^(-1) , latent heat of fusion of ice is "80 cal g"^(-1) , the specific heat capacity of water and ice are "1 cal g"^(-1).^(@)C^(-1) and "0.5 cal g"^(-1).^(@)C^(-1) respectively.

    The volume of steam produced by 1g of water at 100^(@)C is 1650 cm^(3) . Calculate the change in internal energy during the change of state. Given J= 4.2xx10^(7) erg . cal.^(-1), d= 981 cm^(s-2) . Latent heat of stream = 540 cal. G^(-1)

    The latent heat of vaporisation of water is 9700 "Cal/mole" and if the b.p.is 100^(@)C , ebullioscopic constant of water is

    Entropy of vaporisation of water at 100^(@)C , if molar heat of vaporisation is 9710 cal mol^(-1) will be

    Entropy of vaporisation of water at 100^(@)C , if molar heat of vaporisation is 8710 cal mol^(-1) will be

    Home
    Profile