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For the non-zero value of the force of a...

For the non-zero value of the force of attraction between gas molecules, gas equation will be

A

`PV= nRT-(n^(2)a)/(V)`

B

`PV=nRT+nbP`

C

`PV=nRT`

D

`P=(nRT)/(V-B)`

Text Solution

Verified by Experts

The correct Answer is:
A
`(P+(an^(2))/(V^(2))) (V)=nRT or PV= nRT-(n^(2)A)/(V)`
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Knowledge Check

  • For the non-zero values of force of attraction between gas molecules, gas equation will be

    A
    `PV = nRT - (n^2 a)/V`
    B
    `PV = nRT + nbP`
    C
    `PV = nRT`
    D
    `P = (nRT)/(V - b)`

  • For the non-zero values of force of attraction between gas molecules, gas equation will be

    A
    `PV = nRT - (n^2 a)/V`
    B
    `PV = nRT + nbP`
    C
    `PV = nRT`
    D
    `P = (nRT)/(V - b)`

  • For non-zero value of force of attraction between gas molecules gas equation Will be

    A
    `PV =nRT -(n^(2)a)/(V)`
    B
    PV = nRT + nbP
    C
    PV =nRT
    D
    `P=(nRT)/(V-b)`

    • Similar Questions

    Explore conceptually related problems

    van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT For non-zero value of force of attraction between gas moleculer at large volume, gas equation will be :

    The force of attraction between molecules of different substances is

    Statement-1: If the forces of attraction between the molecules suddenly disappear, pressure exerted by the gas will increase. Statement-2: In the absence of the forces of attraction between the molecules, the molecule of the gas will hit the wall of container harder.

    If the assumption that there is no force of attraction between the molecules of a gas is correct, what will be the consequences?

    If the assumption that there is no force of attraction between the molecules of a gas is correct , what will be the consequences ?

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