A sample containing 42.8 g of Ar is enclosed in a container of volume 8.11×10−2 L at 375 K.
Calculate P using the Redlich-Kwong equation of state
the gas is argon
Volume = 8.11 X 10^-2
Temperature = 375 K
Mass = 42.8 , so moles = mass / atomic weight = 42.8 / 40 = 1.07
According to Redlich =kwong equation of state
Vm = molar volume = volume / moles of gas = 8.11X 10^-2 / 1.07 = 7.58 X 10^-2
T = 375 K
Tc = critical temperature = −122.4 °C (150.8 K)
Pc = critical pressure = 48.1 atm (4,870 kPa)
a = 0.42748 R^2 Tc^2.5 / Pc = 0.42748 X (0.0821)^2 (150.8)^2.5 / 48.1 = 5.99 X 10^-5 X 279256.54
a = 16.712
b = 0.08664 RTc / Pc = 0.08664 X 0.0821 X 150.8 / 48.1 = 0.0223
Pressure = (30.7875 / 0.0535 )- (16.712 / 0.0758 X 0.0991 X 19.3649)
Pressure = 575.467 - 144.887 = 430.58 Atm
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