Home
Class 11
CHEMISTRY
The ideal gas behaviour has been express...

The ideal gas behaviour has been expressed in terms of ideal gas equation `PV =nRT` Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor `Z = (Z =(PV)/(nRT))` Usually when `Z gt1` repulsive forces among molecules predominates and when `Z lt1` attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of `Z` for 1 mole of gas at critical conditions is `(3)/(8)`
The gas which always shows predominative repulsive forces .

A

`He`

B

`Ne`

C

`Ar`

D

`Kr`

Text Solution

Verified by Experts

For he `Z gt 1` repulsive forces predominates .
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • GASEOUS STATE

    P BAHADUR|Exercise passage -3|1 Videos

  • GASEOUS STATE

    P BAHADUR|Exercise passage -4|1 Videos

  • GASEOUS STATE

    P BAHADUR|Exercise Exercise 7 passage -1|1 Videos

  • CHEMICAL EQUILIBRIUM

    P BAHADUR|Exercise Exercise|134 Videos

  • IONIC EQUILIBRIUM

    P BAHADUR|Exercise Exercise|85 Videos

Similar Questions

Explore conceptually related problems

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The compressibility factor SO_(20 is 0.711 then .

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The ratio of Z at Boyle's temperature and at critical conditions for 1 mole of a given gas is .

Knowledge Check

  • In the gas equation, PV = nRT

    A
    V denotes volume of one mole
    B
    n is the number of molecules of a gas
    C
    n moles of gas have volume V
    D
    P is pressure of gas when only one mole of gas is present

  • Gas deviates from ideal gas nature because molecules

    A
    are colourless
    B
    attract each other
    C
    contain covalent bond
    D
    show Brownian movement

  • Gas deviates from ideal gas nature because molecules

    A
    are colourless
    B
    attract each other
    C
    contain covalent bond
    D
    show Brownian movement

    • Similar Questions

    Explore conceptually related problems

    The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The numerical value of Z is greater than 1 for gases usually at .

    The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The numerical value of 'Z' for gases within Boyle's temperature range is .

    For an ideal gas, the value of compressibility factor Z(=(pVm)/(RT)) is

    For H_(2) gas the compressibility factor Z=PV/nRT is

    For H_(2) gas the compressibility factor Z=PV/nRT is

    Home
    Profile