A 1.55-mol sample of nitrogen gas is maintained in a 0.730-L container at 292 K. Calculate the pressure of the gas using both the ideal gas law and the van der Waals equation (van der Waals constants for N2 are a = 1.39 L2atm/mol2 and b = 3.91×10-2 L/mol).
Pideal gas equation = ______ atm
Pvan der Waals =_____ atm
1)
Given:
V = 0.73 L
n = 1.55 mol
T = 292.0 K
use:
P * V = n*R*T
P * 0.73 L = 1.55 mol* 0.08206 atm.L/mol.K * 292 K
P = 50.9 atm
Answer: 50.9 atm
2)
Given:
V = 0.73 L
n = 1.55 mol
R = 0.08206 atm.L/mol.K
T = 292.0 K
a = 1.39 atm.L^2/mol^2
b = 0.0391 L/mol
use:
(P+an^2/V^2)*(V-nb) = n*R*T
(P + 1.39*1.55^2/0.73^2)*(0.73-1.55*0.0391) = 1.55*0.08206*292.0
(P + 6.2666)*(0.6694) = 37.1404
P + 6.2666 = 55.4835
P = 49.2 atm
Answer: 49.2 atm
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