contestada

Consider 20.0 moles of CO2 in a 1.0 liter container at 300.0 K. What is the pressure predicted by the van der Waals equation? The ideal gas law constant is 0.08206 [L•atm] / [mol•K]. For CO2, the pressure correction constant is 3.658 L2•atm / mol 2, and the volume correction constant is 0.04286 L / mol.

Respuesta :

Answer:

Pressure predicted by van der waals equation is 1984.7 atm

Explanation:

Van der waal gas equation-

[tex](P+\tfrac{n^{2}a}{V^{2}})(V-nb)=nRT[/tex]

Where, P is pressure of gas , n is number of moles of gas, a is pressure correction constant, V is volume of gas, b is volume correction constant , R is gas constant and T is temperature in kelvin scale.

So, plug-in all the given values in the above equation-

[tex][P+\frac{(20.0mol)^{2}\times (3.658L^{2}.atm.mol^{-2})}{(1.0L)^{2}}][1.0L-(20.0mol\times0.04286 L.mol^{-1} )]=(20.0mol)\times (0.08206L.atm.mol^{-1}.K^{-1})\times (300.0K)[/tex]

or, [tex][P+\frac{(20.0mol)^{2}\times (3.658L^{2}.atm.mol^{-2})}{(1.0L)^{2}}][/tex]=[tex]3447.90atm[/tex]

or, P = 1984.7 atm

So, Pressure predicted by van der waals equation is 1984.7 atm