Calculate the pressure exerted by 10 moles of neon gas in a 5 L container at `27^(@)C`, using the ideal gas equation.

Explanation

(a) For an ideal gas , PV = n RT
`P = (nRT)/(V) = (10 "mol" xx 0.082 L "atm" K^(-1) mol^(-1) xx 300 K)/(5L) = 49.26` atm
(b) For a van der Waals gas , P = `(n RT)/(V - nb) - (n^(2) a)/(V^(2))`
P = `(10 "mol" xx 0.0821 L "atm" K^(-1) mol^(-1) xx 300 K)/((5L) - (10 "mol" xx 0.0171 L "mol"^(-1))) - ((10 mol)^(2) (0.21 L^(2) "atm" mol^(-2)))/((5L)^(2))`
= 51.004 atm - 0.84 atm = 50.16 atm