Question

The van der Waals equation for one mole of $C{O}_2$ gas at low pressure will be :

• A. $[P+\frac{a}{V^2}]V=RT$
• B. $P(V-b)=RT-\frac{a}{V^2}$
• C. $P=\frac{RT}{V-b}$
• D. $P=[\frac{RT}{V-b}-\frac{a}{V^2}]$

Answer 1

The correct option is A $[P+\frac{a}{V^2}]V=RT$

At low pressure, volume correction for 1 mole of gas is negligible,
$b=0$

and van der Waals equation becomes

$[P+\frac{a}{V^2}]V=RT$

So, the correct option is $A$