A 10.21 mol sample of argon gas is maintained in a 0.7564 L container at 296.9 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219*10-2 L/mol.

The pressure in atm calculated using the van der Waals' equation, is 337.2atm

Explanation:

This is the Van der Waals equation for real gases:

(P + a/v²) (v-b) = R. T

where P is pressure

v is Volume/mol

R is the gas constant and T, T° in K

a y b are constant for each gas, so those values are data, from the statement.

[P + 1.345 L²atm/mol² / (0.7564L/10.21mol) ² ] (0.7564L/10.21mol - 3.219*10-2 L/mol) = 0.082 L. atm/mol. K. 296.9K

[P + 1.345 L²atm/mol² / 5.48X10⁻³ L²/mol²] (0.074 L/mol - 3.219*10-2 L/mol) = 0.082 L. atm/mol. K. 296.9K

(P + 245.05 atm) (0.04181L/mol) = 0.082 L. atm/mol. K. 296.9K

(P + 245.05 atm) (0.04181L/mol) = 24.34 L. atm/mol

0.04181L/mol. P + 10.24 L. atm/mol = 24.34 L. atm/mol

0.04181L/mol. P = 24.34 L. atm/mol - 10.24 L. atm/mol

0.04181L/mol. P = 14.1 L. atm/mol

P = 14.1 L. atm/mol / 0.04181 mol/L

P = 337.2 atm