Question

A 9.800 mol sample of nitrogen gas is maintained in a 0.8166 L container at 301.8 K. What is the pressure in atm calculated using the van der Waals' equation for N2 gas under these conditions? For N2, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol.

Answer 1

P = 359.8 atm

Step-by-step explanation:

The van der Waals' equation relates the properties of a gas, introducing constants "a" and "b" in order to consider gases as real gases. The equation is:

`(P+a.(n^(2) )/(V^(2) ) ).(V-nb)=n.R.T`

where,

P: pressure

a: correction factor for intermolecular forces

V: volume

b: correction factor for molecules' volume

n: moles

R: ideal gas constant

T: absolute temperature

`(P+(1.390L^(2)atm)/(mol^(2)).((9.800mol)^(2))/((0.8166L)^(2))).(0.8166L-9.800mol.(3.910 * 10^(-2)L)/(mol))=9.800mol * (0.08206atm.L)/(mol.K) * 301.8K\\(P + 200.2atm).(0.4334L) = 242.7atm.L\\P=359.8 atm`