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Use the Van der Waals equation of state to calculate the pressure of p of 2.80 mol of H2S at 481 k in a 4.20 l vessel. Van der Waals constant for H2S is 4.481 atm*l^2 / mol^2, and 0.0434g/mol.
Accepted Answer
The Van der Waals equation of state is given by:
(P + a(n/V)^2)(V - nb) = nRT
Where:
P is the pressure
V is the volume
T is the temperature
n is the number of moles
R is the ideal gas constant (0.0821 L
atm/mol
K)
a and b are Van der Waals constants
Substituting the given values, we have:
(P + 4.481 (2.80/4.20)^2)(4.20 - 0.0434
2.80) = 2.80
0.0821
481
Solving for P, we get:
P = 10.9 atm
Therefore, the pressure of H2S is 10.9 atm.
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