Home
Class 12
CHEMISTRY
Latent heat of vaporisation of water is ...

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

Text Solution

Verified by Experts

The correct Answer is:
A
`DeltaS_(vap)=(DeltaH_(vap))/(T)=(540xx1000)/(373)=1447cal`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • Chemical Thermodynamics and Thermochemistry

    OP TANDON|Exercise Miscellaneous Numerical Examples|22 Videos

  • Chemical Thermodynamics and Thermochemistry

    OP TANDON|Exercise Practice problems|81 Videos

  • Chemical Thermodynamics and Thermochemistry

    OP TANDON|Exercise Solved Example|74 Videos

  • CHEMICAL KINETICS

    OP TANDON|Exercise LINKED COMPRESHENSION TYPE QUESTIONS ( SECTION-VI)|4 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    OP TANDON|Exercise INTEGER|2 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.

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.

Knowledge Check

  • 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)`

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

    A
    `0.513^(@)C`
    B
    `1.026^(@)C`
    C
    `10.26^(@)C`
    D
    `1.832^(@)C`

  • 22320 cal of heat is supplied to 100g of ice at 0^(@)C . If the latent heat of fusion of ice is 80 cal g^(-1) and latent heat of vaporization of water is 540 cal g^(-10 , the final amount of water thus obtained and its temperature respectively are

    A
    `8g, 100^(@)C`
    B
    `100g, 90^(@)C`
    C
    `92g, 100^(@)C`
    D
    `8g, 100^(@)C`

    • Similar Questions

    Explore conceptually related problems

    100 gram of ice at 0^@C is converted into water vapour at 100^@C Calculate the change in entropy.

    1gm water at 100^(@)C is heated to convert into steam at 100^(@)C at 1atm . Find out chage in internal energy of water. It is given that volume of 1gm water at 100^(@)C = 1c c , volume of 1gm steam at 100^(@)C = 167 1 c c . Latent heat of vaporization = 540 cal//g . (Mechanical equivalent of heat J = 4.2J//cal)

    How much heat is required to change 10g ice at 10^(@)C to steam at 100^(@)C ? Latent heat of fusion and vaporisation for H_(2)O are 80 cl g^(-1) and 540 cal g^(-1) , respectively. Specific heat of water is 1cal g^(-1) .

    One mole of ice is melted at 0^(@)C and then is heated to 100^(@)C . What is the difference in entropies of the steam and ice? The heats of vaporisation and fusion are 540 cal g^(-1) and 80 cal g^(-1) respectively. Use the average heat capacity of liquid water as 1cal g^(-1) degree^(-1)

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

    Home
    Profile