1. A 9.157 mol sample of methane gas is maintained in a 0.8013 L container at 30

Question

1. A 9.157 mol sample of methane gas is maintained in a 0.8013 L container at 302.7 K. What is the pressure in atm calculated using the van der Waals' equation for CH4 gas under these conditions? For CH4, a = 2.253L2atm/mol2 and b = 4.278×10-2 L/mol.

2. According to the ideal gas law, a 1.018mol sample of oxygen gas in a 1.037 L container at 273.7 K should exert a pressure of 22.05 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For O2 gas, a = 1.360L2atm/mol2 and b = 3.183×10-2 L/mol.

Explanation / Answer

Ans 1

van der Waals' equation

[P + a(n/V)2] x (V - nb) = nRT

[P + 2.253*(9.157/0.8013)2] x (0.8013 - 9.157*4.278*10^-2) = 9.157*0.0821*302.7

(P + 294.22) x (0.4095) = 227.566

P + 294.22 = 555.718

P = 261.498 atm

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