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Deviation of real gases from ideal behav...

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is
`Z=(pV)/(nRT)`
The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at `0^(@)C` and 100 atm pressure is found to be 0.5. The van der Waals gas equation is
`(p(an^(2))/(V^(2)))(V-nb)=nRT`
What is the value of Z for an ideal gas?

Text Solution

AI Generated Solution

To find the value of the compressibility factor \( Z \) for an ideal gas, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding the Compressibility Factor (Z)**: The compressibility factor \( Z \) is defined as: \[ Z = \frac{PV}{nRT} ...
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Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the volume of the gas?

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the significance of van der Waals constant 'a'?

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT Calculate the value of 'a' assuming volume of molecules to be negligible.

Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT For gases like H_(2) and He , which show only positive deviation from ideal behaviour, the compressibility factor is greater than 1. Is the statement true or false?

The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb) = nRT

The unit of the van der Waals gas equation parameter 'a' in (P+(an^(2))/(V^(2)))(V-nb)=nRT is :

Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are

Knowledge Check

  • Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are

    A
    `L^(2)atm^(-1), L`
    B
    `atm L^(-2), L^(-1)`
    C
    `L^(2) atm^(-1) mol^(-2), L mol^(-1)`
    D
    `atm L^(2)mol^(-2), L mol^(-1)`

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

    A
    Equal to 1
    B
    Equal to 0
    C
    Always greater than 1
    D
    Initially less than 1 and then becomes greater than 1 at high pressures

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

    A
    Equal to 1
    B
    Equal to 0
    C
    Always greater than 1
    D
    Initially less than 1 and then becomes greater than 1 at high pressures