The value of van der Waals constant `a` for the gases `O_(2)`, `N_(2)`, `NH_(3)`, and `CH_(4)` are `1.360`, `1.390`, `4.170`, and `2.253 L^(2) atm mol^(-2)`, respectively. The gas which can most easily be liquefied is

Options

A. `O_(2)`
B. `N_(2)`
C. `NH_(3)`
D. `CH_(4)`

Explanation

`(P+(an^(2))/(V^(2)))(V-nb)=nRT`
The van der Waals constant `a` is used in pressure correction, and its value depends upon the intermolarcular forces between the gas molecules The larger the value of `a` for a gas, the more easily that gas can be liquefied.