Home
Class 11
CHEMISTRY
For the isothermal reversible expansion ...

For the isothermal reversible expansion of an ideal gas

A

`Delta H gt 0 and Delta U= 0`

B

`Delta H gt 0 and Delta U lt 0`

C

`Delta H= 0 and Delta U= 0`

D

`Delta H = 0 and Delta U gt 0`

Text Solution

Verified by Experts

The correct Answer is:
C
Isothermal means `Delta T = 0` If temperature is constant, means `Delta U = 0` as whole energy is used in work done and due to reversible expansion `Delta Η = 0`.
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS AND THERMOCHEMISTRY

    ERRORLESS|Exercise NCERT Based Questions (IInd & IIIrd Law of Thermodynamics and Entropy)|41 Videos

  • THERMODYNAMICS AND THERMOCHEMISTRY

    ERRORLESS|Exercise NCERT Based Questions (Heat of Reaction)|67 Videos

  • THERMODYNAMICS AND THERMOCHEMISTRY

    ERRORLESS|Exercise (Assertion & Reason)|18 Videos

  • THE S-BLOCK ELEMENTS

    ERRORLESS|Exercise Assertion & Reason|10 Videos

Similar Questions

Explore conceptually related problems

Correct relation for isothermal reversible expansion of an ideal gas is DeltaS = 0 DeltaG = - T DeltaS DeltaH != 0 DeltaU != 0

In an isothermal irreversible expansion of an ideal gas as per IUPAC sign convention :

Calculate the work done during isothermal reversible expansion of one mole ideal gas from 10 atm to 1 atm at 300 K .

Calculate Q and w for the isothermal reversible expansion of one mole an ideal gas from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at a constant temperature of 273 K respectively.

Calculate the DeltaH for the isothermal reversible expansion of 1 mole of an ideal gas from initial pressure of 0.1 bar at a constant temperature at 273K .

For an isothermal free expansion of an ideal gas,

Calculate q,w , and DeltaU for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 2.0 bar to a final pressure of 0.2 bar at a constant temperature of 273K .

ERRORLESS-THERMODYNAMICS AND THERMOCHEMISTRY-NCERT Based Questions (First Law of Thermodynamics and Hess Law)
  1. The enthalpy change for a reaction does not depend upon:

    Text Solution

    |

  2. On the basic of thermochemical equations (I),(II)and (III), Find out w...

    Text Solution

    |

  3. The reaction A to B , DeltaH=+24 kJ//"mole". For the reaction B to C, ...

    Text Solution

    |

  4. The enthalpy of neutralization of HCN by NaOH is - 12.13 kJ mol^(-1). ...

    Text Solution

    |

  5. One mole of magnesium in the vapor state absored 1200 kJ mol^(-1) of e...

    Text Solution

    |

  6. For the change,C("diamond") rarr C("graphite"), Delta H = -1.89 kJ , i...

    Text Solution

    |

  7. Given R = 8.314 J K^(-1) "mol"^(-1), the work done during combustion...

    Text Solution

    |

  8. Work done during isothermal expansion of one mole of an ideal gas form...

    Text Solution

    |

  9. An ideal gas expands from 10^(-3) m^(3) to 10^(-2) m^(3) at 300 K agai...

    Text Solution

    |

  10. In an adibatic process, no transfer of heat takes place between system...

    Text Solution

    |

  11. One mole of an ideal gas is allowed to expand reversible and adiabatic...

    Text Solution

    |

  12. One mole of an ideal gas at 250 K is expanded isothermally from an ini...

    Text Solution

    |

  13. To calculate the amount of work done in joules during reversible isoth...

    Text Solution

    |

  14. Two moles of an ideal gas expand spontaneouly into vacuum. The work do...

    Text Solution

    |

  15. Which expression is correct for the work done in adiabatic reversible ...

    Text Solution

    |

  16. The pressure volume work for an ideal gas can be calculated by using t...

    Text Solution

    |

  17. For an ideal gas, which of the following is true

    Text Solution

    |

  18. In an isobaric process, the ratio of heat supplied to the system (dQ) ...

    Text Solution

    |

  19. The entropy change in the isothermal reversible expansion of 2 moles o...

    Text Solution

    |

  20. For the isothermal reversible expansion of an ideal gas

    Text Solution

    |