One mole of carbon-dioxide was found to occupy a volume of 1.32 litre at `48^(@) `C and at a pressure of 16.4 atm. Calculate the pressure of the gas that would have been expected to behave ideally and non-ideally.

Explanation

`[a = 3.59` atm `dm^(6) mol^(-2)], [b = 4.27 xx 10^(-2) dm^(3) mol^(-1)` and R = `0.082 dm^(3)` atm `deg^(-1) mol^(-1)`]
V = 1.32 lit
T = `48 + 273 = 321 K`
R = `0.082 dm^(3)` atm `K^(-1).mol^(-1)`
(n = 1 mole)
For ideal behaviour , PV = RT
`P = (RT)/(V) = (0.082 xx 321)/(1.32)`
`P_("ideal") = 19.94` atm
For real behaviour , `P = (RT)/(V - b) - (a)/(V^(2)) ( n = 1 ` mole)
For ideal behaviour ,
For ideal behaviour ,
`PV = RT`
`P = (RT)/(V) = (0.082 xx 321)/(1.32)`
` P_("ideal") = 19.94` atm
For real behaviour ,
`P = (RT)/(V -b) = (a)/(V^(2)) (n = 1`mole)
`P = ((0.082 xx 321)/(1.32 - 0.0427)) - ((3.59)/((1.32)^(2)))`
= `20.6 - 2.06`
`P_("real") = 18.54` atm