Home
Class 11
CHEMISTRY
Calculate the entropy change when 3.6g o...

Calculate the entropy change when `3.6g` of liquid water is completely converted into vapour at `100^(@)C` . The molar heat of vaporization is `40.85KJ mol^(-1)` .

A

`6.08JK^(-1)`

B

`109.5JK^(-1)`

C

`21.89JK^(-1)`

D

`-21.89JK^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
`DeltaH_(vap)=40850Jmol^(-1),T_(b)=373K`
`DeltaS_("vap")=(DeltaH_("vap"))/(T_(b))=(40850Jmol^(-1))/(373K)=109.5K^(-1)mol^(-1)`
`DeltaS_(vap)` per gram `=(109.5JK^(-1)mol^(-1))/(18gmol^(-1))=6.-083JK^(-1)g^(-1)`
Entropy change for `3.6g` water `=6.083JK^(-1)g^(-1)xx3.6g`
`=21.89JK^(-1)`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS

    A2Z|Exercise Heat Capacity And Calorimetry|13 Videos

  • CHEMICAL THERMODYNAMICS

    A2Z|Exercise Section B - Assertion Reasoning|17 Videos

  • CHEMICAL THERMODYNAMICS

    A2Z|Exercise Work, Internal Energy And Enthalpy|76 Videos

  • CHEMICAL EQUILIBRIUM

    A2Z|Exercise Section D - Chapter End Test|30 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY OF PROPERTIES

    A2Z|Exercise Section D - Chapter End Test|30 Videos

Similar Questions

Explore conceptually related problems

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

90 g of water spilled out from a vessel in the room on the floor. Assuming that water vapour behaving as an ideal gas, calculate the internal energy change when the spilled water undergoes complete evaporation at 100^(@)C . (Given the molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ mol^(-1) ).

Calculate the entropy change when one mole of water at 373 K is converted into steam. Latent heat of vaporisation of water (DeltaH_(v)) is 40.7 xx 10^(3) J mol^(-1)

Calculate the entropy change (DeltaS) when 1 mol of ice at 0^(@)C is converted into water at 0^(@)C . Heat of fusion of ice at 0^(@)C is 1436 cal per mol.

Calculate the entropy change involved in the vaporisation of water at 373 K to vapours at the same temperature(Latent heat of vaporisation = 2.275 kJ/g).

What is DeltaU when 2.0 mole of liquid water vaporise at 100^(@)C ? The heat of vaporistaion , DeltaH vap. of water at 100^(@)C is 40.66 kJ mol^(-1) .

Knowledge Check

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

    A
    `20 cal mol^(-1)K^(-1)`
    B
    `26 cal mol^(-1)K^(-1)`
    C
    `24 cal mol^(-1)K^(-1)`
    D
    `28 cal mol^(-1)K^(-1)`

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

    A
    `20 cal mol^(-1) K^(-1)`
    B
    `23.36 cal mol^(-1) K^(-1)`
    C
    `24 cal mol^(-1) K^(-1)`
    D
    `28.0 cal mol^(-1) K^(-1)`

  • Calculate the ebullioscopic constant for water. The heat of vaporization is 40.685 kJ mol^(-1)

    A
    `0.512 K kg mol^(-1)`
    B
    `1.86 K kg mol^(-1)`
    C
    `5.12 K kg mol^(-1)`
    D
    `3.56 K kg mol^(-1)`
    • A2Z-CHEMICAL THERMODYNAMICS-Entropy, Gibb'S Energy And Spontaneity Of Process
    1. Calculate the entropy change when 3.6g of liquid water is completely c...

      Text Solution

      |

    2. In an irreversible process taking place at constant P and T in which o...

      Text Solution

      |

    3. The correct relationship between free energy change in a reaction and ...

      Text Solution

      |

    4. Predict which of the following reaction (s) has a positive entropy cha...

      Text Solution

      |

    5. Maxing of non-reacting gases is generally accompanied by

      Text Solution

      |

    6. A particular state of system is arrived at starting from a given state...

      Text Solution

      |

    7. For a spontaneous reaction, DeltaG, equilibrium constant (K) and E(cel...

      Text Solution

      |

    8. For the water gas reaction C(s) + H(2)O(g) hArr CO(g) + H(2)(g) At 1...

      Text Solution

      |

    9. At 500K , for an isobaric pracess. DeltaS(system)=-10(KJ)/(molK) and...

      Text Solution

      |

    10. Identify the correct statement regarding a spontaneous process:

      Text Solution

      |

    11. Standard entropt of X(2) , Y(2) and XY(3) are 60, 40 and 50JK^(-1)mol...

      Text Solution

      |

    12. If liquids A and B from an ideal solution,

      Text Solution

      |

    13. Which reaction, with the following value of DeltaH and DeltaS at 350K ...

      Text Solution

      |

    14. The incorrect expression among the following is

      Text Solution

      |

    15. Which of the following reactions is associated with the most negative ...

      Text Solution

      |

    16. For the reaction in the plant cells 6CO(2)(g)+12H(2)O(l)rarrC(6)H(12...

      Text Solution

      |

    17. The entropy change involved in the isothermal reversible expansion of ...

      Text Solution

      |

    18. In view of the signs of Delta(r)G^(0) for the following reactions Pb...

      Text Solution

      |

    19. Two moles of an ideal gas is expanded irreversibly and isothermally at...

      Text Solution

      |

    20. A spontaneous change is one in which a system under goes

      Text Solution

      |