Van der Waals Constants a (atm · L 2 /mol 2 ) Gas a (bar · L 2 /mol 2 ) a (atm ·

Question

Van der Waals Constants

a

(atm·L2/mol2)

Gas a
(bar·L2/mol2)

a

(atm·L2/mol2)

b (L/mol) CH4 2.303 2.273 0.0431 CO2 3.658 3.610 0.0429 Cl2 6.343 6.260 0.0542 NH3 4.225 4.170 0.0371 H2O 5.537 5.465 0.0305 Xe 4.192 4.137 0.0516 7/6/2016 11:55 PM 6.3/10 Calculator-l Gradebook Print Periodic Table Question 24 of 25 Map Sapling Learning Use the van der Waals equation of state to calculate the pressure of 2.70 mol of CH4 at 457 K in a 4.10-L vessel. Van der Waals constants can be found here. Number P= atm Use the ideal gas equation to calculate the pressure under the same conditions. Number P= atm Previous Give Up &View; Solution Check AnswerNextExit Hint

Explanation / Answer

Answer:-

P=(R*T/(V-b)) - a/(V)2

P is pressure (atm)
V is Volume (in Liters) 4.10 L
n is the number of moles 2.70 moles
R is a constant (0.08206)
T is Temperature (in kelvin) 457 K

Now P=(R*T/(V-b)) - a/(V)2

P = (0.08206*457 / (4.10-0.0431)) - (2.273/(4.10)2

P =(37.50/4.05) -(0.1352) =9.2592-0.1352 = 9.1240 atm

P= 9.1240 atm

The ideal gas law is PV=nRT.
P is pressure (atm)
V is Volume (in Liters)
n is the number of moles
R is a constant (0.08206)
T is Temperature (in kelvin)

P=nRT/V = 2.70*0.08206*457 / 4.10

P=24.69 atm

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