In the van der Waals equation for real gases, | vedclass

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

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$P + \frac{a}{V_m^2}$

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(B) The van der Waals equation for $n$ moles of a real gas is given by $(P + \frac{an^2}{V^2})(V - nb) = nRT$.For $1$ mole of gas,it is $(P + \frac{a}{V_m^2})(V_m - b) = RT$.Here,the term $\frac{a}{V_m^2}$ represents the pressure correction factor,which accounts for the intermolecular forces of attraction between gas molecules.Therefore,the term representing intermolecular forces is $P + \frac{a}{V_m^2}$.

In the van der Waals equation for real gases,which of the following terms represents the correction for intermolecular forces?

Similar Questions

In the van der Waals equation,which of the following will have the highest value of '$a$'?

If the compressibility factor $Z < 1$ at $STP$,what will be the molar volume?

Compressibility factor,$Z$,of a gas is given as $Z = \frac{pV}{nRT}$.
$(i)$ What is the value of $Z$ for an ideal gas?
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The compressibility factor $(Z)$ of a gas is less than unity at $STP$,then:

If $Z$ is a compressibility factor,the van der Waals equation at low pressure can be written as:

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