Calculate the pressure excerted by `5 mol` of `CO_(2)` in `1 L` vessel at `47^(@)C` using van der Waals equation. Also report the pressure of gas if it behaves ideally in nature.
`(a=3.592 atm L^(2) mol^(-2), b=0.0427 L mol^(-1))`

Explanation

Given `n =5, V =1 litre,`
`T =47 + 273 = 320 K`
` a = 3.592, b = 0.0427`
Using van ber Waals equation for n mole
`[P+(n^(2)a)/(V^(2))][V -nb]=nRT`
`[P +(25 ccxx 3.592)/(1)][1 -5 xx 0.0427]=5 xx 0.0821 xx 320`
`P =77.218 atm`
Also if gas behaves ideally, then `PV =nRT`
` P xx 1 =5 xx 0.0821 xx 320 = 131.36` atm .