Volume of 2 moles of `CO_(2)` gas at `27^(@)C` is 0.001 `m^(3)`. What will be the pressure of this gas (i) according to van der waals equation and (ii) according to ideal gas equation?
[Given `a(CO_(2))=0.364" "N*m^(4)*mol^(-2) and b(CO_(2))=4.27xx10^(-5)m^(3)*mol^(-1)`]

Explanation

(i) `(P+(n^(2)a)/(V^(2)))(V-nb)=nRT`
or, `(P+(2^(2)+0.364N*m^(4))/(10^(-6)m^(6)))(10^(-3)-2xx4.27xx10^(-5))m^(3)`
`=2xx0.0821x300L*atm` ,brgt or, `(P+1.456xx10^(6)N*m^(-2))(9.146xx10^(-4)m^(3))`
`=2xx0.0821xx300xx10^(-3)m^(3)*atm`
or, `P+1.456xx10^(6)xx10^(-5)atm=53.859atm`
`therefore P=39.299 atm`
(ii) PV=nRT
or, `P=(2xx0.0821xx300)/(0.001m^(3))L*atm=59260(L*atm)/(m^(3))=59.26atm`