Question

Which of the following is/are correct for a gas obeying Van der Waals equation?

• A. A gas having negligible size and reasonable intermolecular force follows $(P+\frac{a}{V_m^2})\left(V_m\right)=RT$
• B. A gas having negligible intermolecular force and reasonable size follows: $Z=1-\frac{Pb}{RT}$
• C. A gas having negligible size and negligible intermolecular force follows: $P{V}_m=RT$
• D. At boyle's temperature, gas follows $P{V}_m=RT$ at all pressure

Answer 1

Answer: (A), (C)

The correct options are
A A gas having negligible size and reasonable intermolecular force follows $(P+\frac{a}{V_m^2})\left(V_m\right)=RT$
C A gas having negligible size and negligible intermolecular force follows: $P{V}_m=RT$

The equation of state for a gas having negligible volume and reasonable intermolecular forces is $(P+\frac{a}{V^{2}m})\left(V_m\right)=RT.$.
The equation of state for a gas having negligible volume and negligible intermolecular forces is $P{V}_m=RT$.
The second equation can be obtained from first equation by substituting $a=0$.
The first equation can be obtained from Van der Waals equation of state $(p+\frac{a}{V_m^2})(V_m-b)=Rt$ by substituting $b=0$.