Calculate the pressure exerted by 5 mole of `CO_(2)` in one litre vessel at `47^@)C` using van der Waal's equation. Also report the pressure of gas if it behaves ideal in nature. Given that a `=3.592" atm It"^(2)" mol"^(-2), b=0.0427` It/mol. Also if the volume occupled by `CO_(2)` molecules is negligible, then calculate the pressure exerted by one mole of `CO_(2)` gas at 273 K.

Explanation

van der Waals equation
`[P+(n^(2)a)/(V^(2))][V-nb]=nRT`
`n_(CO_(2))=5, V=1" litre, "T=320 K, a=3.592, b=0.0427`
`therefore [P+25xx(3.592)/(1)][1-5xx0.0427]=5xx0.0821xx320`
`therefore P=77.218` atm
For ideal behaviour of gas, PV =nRT
`therefore P xx1=5xx0.0821xx320`
`therefore P=131.36` atm
For one mole `[P+(a)/(V^(2))][V-b]=RT`
`therefore P =(RT)/(V) -(a)/(V^(2))`
`therefore P =(0.0821xx273)/(22.4)-(3.592)/((22.4)^(2))`
`therefore P =0.9922` atm
The volume occupied by 1 mole at 273 K is 22.4 litre if b is negligible.