Calculate the pressure exerted by 0.250 moles of carbon dioxide in 0.275 litres at 100^@C and compare this value with that expected for an ideal gas. (Given : a = 3.59 L^2 " atm " mol^(-2), b = 0.0427 L mol^(-1))

Calculate the pressure exerted by 0.250 moles of carbon dioxide in 0.2

1.	Calculate the pressure exerted by 0.250 moles of carbon dioxide in 0.275 litres at 100^@C and compare this value with that expected for an ideal gas. (Given : a = 3.59 L^2 " atm " mol^(-2), b = 0.0427 L mol^(-1))
Answer» Solution :For n moles of a gas, van der Waals. EQUATION can be written as `(P+(an^2)/V_2)(V - nb) = nRT` Substituting the corresponding values, we have `[P+(3.59 xx (0.250)^2)/((0.275)^2)][0.275 - (0.250 xx 0.0427)]` `= 0.250 xx 0.0821 xx 373` which gives, P = 26 atm. Under similar conditions, for an IDEAL gas `P=(nRT)/V = (0.250 xx 0.0821 xx 375)/(0.275) =27.8` atm, Hence, the PRESSURE exerted by `CO_2` under given conditions is 26 atm. An ideal gas, under similar conditions will EXERT a pressure of 27.8 atm.