Home
Class 12
CHEMISTRY
Assuming that water vapour is an ideal g...

Assuming that water vapour is an ideal gas, the internal energy change `(DeltaU)` when 1 mol of water is vaporized at 1 bar pressure and `100^(@)`C, (given : molar enthalpy of vaporized of water of 1 bar and 373 K= 41 kJ `mol^(-1)` and `R = 8.314 JK^(-1) mol^(-1)` will beL

A

`4.100 kJ mol^(-1)`

B

`3.7904 kJ mol^(-1)`

C

`37.904 kJ mol^(-1)`

D

`41.00 kJ mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
C
`H_(2)(O)_((l))rarr H_(2)O_((g))`
`Delta H=Delta H+Delta n_(g)RT`
`41=Delta E+1xx8.314xx10^(-3)x373`
`therefore Delta E=37.9 kJ mol^(-1)`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    ALLEN|Exercise EXERCISE -2|100 Videos

  • THERMODYNAMICS

    ALLEN|Exercise EXERCISE -3|108 Videos

  • THERMODYNAMICS

    ALLEN|Exercise EXERCISE -1A|41 Videos

  • TEST PAPERS

    ALLEN|Exercise MATHEMATICS|2 Videos

  • Thermodynamics And Thermo Chemistry

    ALLEN|Exercise All Questions|40 Videos

Similar Questions

Explore conceptually related problems

Assuming that water vapour is an ideal gas, the internal energy change (Delta U) when 1 mol of water is vapourised at 1 bar pressure and 100^(@)C , (Given: Molar enthalpy of vapourization of water at 1 bar and 373K=41 kJ mol^(-1) and R=8.3J mol^(-1)K^(-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) ).

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) ).

The internal energy change (in J) when 90 g of water undergoes complete evaporation at 100^(@)C is ______ . (Given : Delta H_("vap") for water at 373 K = 41 kJ/ mol , R = 8.314 JK^(-1) mol^(-1) )

Calculate the work done (w) and internal energy change ( DeltaU ), when one mole of water at 100^@C vaporises against an atmospheric pressure of 1 atm assuming ideal gas behaviour. Heat of vapourisation of water at 100^@C is 1020 cal mol^(-1) .

The internal energy change for the vapourisation of one mole water at 1 atm and 100°C will be (Enthalpy of vapourization of water is 40.66 kJ

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) .

The kinetic energy of two moles of N_(2) at 27^(@) C is (R = 8.314 J K^(-1) mol^(-1))

What is the entropy change (in JK^(-1) mol^(-1)) when one mole of ice is converted into water at 0^(@)C ? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol^(-1) at 0^(@)C )

The value for DeltaU for the reversible isothermal evaporation of 90 g water at 100^(@)C will be (DeltaH_("evap")" of water "=40.8" kJ mol"^(-1), R=8.314"J K"^(-1)"mol"^(-1))

ALLEN-THERMODYNAMICS -EXERCISE -1B
  1. The bond dissociation energies of X2, Y2 and XY are in the ratio of 1 ...

    Text Solution

    |

  2. The direct conversion of A to B is difficult hence it is carried out b...

    Text Solution

    |

  3. The standard enthalpy of for ation (Delta(f) H^(@)) at 298 K for metha...

    Text Solution

    |

  4. The enthalpy change states for the following processes are listed belo...

    Text Solution

    |

  5. For the process H(2)O(l) (1 "bar", 373 K) rarr H(2)O(g) (1"bar", 373 K...

    Text Solution

    |

  6. In conversion of limestone to lime , CaCO3(s) rarrCaO(s)+CO2(g) the va...

    Text Solution

    |

  7. Assuming that water vapour is an ideal gas, the internal energy change...

    Text Solution

    |

  8. identify the correct statement regarding a spontaneous process:

    Text Solution

    |

  9. Oxidising power of chlorine in aqueous solution can be determined by t...

    Text Solution

    |

  10. Standard entropies of X(2), Y(2) and XY(3) are 60, 40 and 50 JK^(–1) m...

    Text Solution

    |

  11. on the basis of the following thermochemical data [Delta(f) G^(@) H ^...

    Text Solution

    |

  12. In a fuel celll, methanol is used as a fuel and O(2) is used as oxidiz...

    Text Solution

    |

  13. The standard enthalpy of formation of NH3 is -46.0 kJ mol^(-1). If the...

    Text Solution

    |

  14. A system absorbs reversibly 600 J of heat and performs 250 J of work. ...

    Text Solution

    |

  15. For reversible melting of ice at 0^(@)C and 1 atm. Pressure, the value...

    Text Solution

    |

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

    Text Solution

    |

  17. The value of enthalpy change (DeltaH) for the reaction C2H5OH(l) + 3...

    Text Solution

    |

  18. Consider the reaction, 4 N O (2) (g) + O(2) (g) to 2 N(2) O (5) (g) ...

    Text Solution

    |

  19. The incorrect expression among the following is :

    Text Solution

    |

  20. A piston filled with 0.04 mole of an ideal gas expands reversibly from...

    Text Solution

    |