The pressure exerted by 5 moles of in one litre vessel at using Van der Waals equation is x atm while the pressure is y atm if it behaves ideally in nature. The value of x and y respectively are
(Given, , )
67.43 atm, 131.36 atm
77.21 atm, 134 atm
131.36 atm, 77.21 atm
77.21 atm, 131.36 atm
We have:
V = 1 litre
T = 320K
a = 3.592
b = 0.0427
n = 5
Now, According to Van der Waals equation, we have:
Thus, the pressure is 77.218 atm when the gas shows real gas behaviour.
Now, if the gas behaves like ideal gas, then, we know:
Thus, the pressure is 131.36 atm when the gas behaves ideally.
Therefore, Option(4) is correct