Question

# For ethane, C2H6, the van der Waals constants are a = 5.435x10−1 Pa.m6/mol−2 and b =...

For ethane, C2H6, the van der Waals constants are a = 5.435x10−1 Pa.m6/mol−2 and b = 6.51x10−5 m3/mol

Calculate the pressure exerted by 1.0 mole of ethane and the compression factor Z:

In a 20 L container at 300K as an ideal gas

P = _______________ __________ Z = ___________

In a 20 L container at 300K as a van der Waals gas

P = _______________ __________ Z = ___________

In an 100. mL container at 900 K as an ideal gas

P = _______________ __________ Z = ___________

In an 100. mL container at 900K as a van der Waals gas

P = _______________ __________ Z = ___________

In a 20 L container at 300K as an ideal gas
P*V = n*R*T
P*20 = 0.0821*300
P = 1.23 atm = 1.246*5 pa

Z= P*V/(N*R*T)
= 1.23*20/(1*0.0821*300)
= 1

In a 20 L container at 300K as a van der Waals gas
V = 20 L = 0.02 m^3
(P+ an^2/V^2)(V-nb)=n*R*t
(P+ 0.05435 / 0.02^2) (0.02-6.51*10^-5) = 8.314*300
(P +135.875) (0.0199) = 2494.2
P = 1.252*10^5 Pa

Z = P real * Vreal/R*T
= (1.252*10^5 + 135.875)*0.0199/(2494.2)
=1

I am allowed to give only 4 answers

You can follow same process to fill teh rest 4

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