12.0 moles of gas are in a 5.00 L tank at 20.5 ∘C . Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol. Express your answer with the appropriate units.
part 1 ,
vander waals equation
(P+an^2/V^2)(V-nb) = nRT
for methane ,
a = 2.300 (L2atm/mol2) , b = 0.043 L/mol
n = no of mol of CH4 gas = 12 mol
V = 5 L
R = 0.0821 l.atm .k-1.mol-1
T = 20.5 c = 293.65 k
(P+(2.3*12^2/5^2))(5-12*0.043) = 12*0.0821*293.65
P = pressure of CH4 gas = 51.27 atm
from ideal gas equation.
PV = nRT
P = pressure of gas = ?
n = no of mol of H2 gas = 12 mol
V = 5 L
R = 0.0821 l.atm.k-1.mol-1
T = 20.5 c = 293.65 k
(P*5) = (12)*0.0821*293.65
P = 57.86 atm
pressure difference = 57.86 - 51.27 = 6.59 atm
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