For a non-ideal gas,identify the term in the | vedclass

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(C) The van der Waals equation for $n$ moles of a real gas is given by: $\left( P + \frac{an^2}{V^2} \right)(V - nb) = nRT$. For $1$ mole of gas $(n=1

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$\left( P + \frac{a}{V^2} \right)$

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(C) The van der Waals equation for $n$ moles of a real gas is given by: $\left( P + \frac{an^2}{V^2} \right)(V - nb) = nRT$. For $1$ mole of gas $(n=1)$,the equation becomes: $\left( P + \frac{a}{V^2} \right)(V - b) = RT$. In this equation,the term $\frac{a}{V^2}$ accounts for the intermolecular forces of attraction between gas molecules. Therefore,the term representing intermolecular forces is $\left( P + \frac{a}{V^2} \right)$.

For a non-ideal gas,identify the term in the van der Waals equation that represents the intermolecular forces.

Similar Questions

Van der Waals equation for a gas is stated as,
$p = \frac{nRT}{V - nb} - a\left( \frac{n}{V} \right)^2$
This equation reduces to the perfect gas equation,$p = \frac{nRT}{V}$,when:

The van der Waals equation reduces to the ideal gas equation under which of the following conditions?

What is the unit of the Van der Waals constant $a$?

Which of the following formulas is used to calculate the compressibility factor?

Assertion : Greater the value of van der Waal's constant $a$,greater is the liquefaction of gas.
Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.

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