1) A 9.172 mol sample of argon gas is maintained in a 0.8485 L container at 304.5 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol.
1)
A 9.172 mol sample of argon gas is maintained in a 0.8485 L container at 304.5 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol.
2)
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3)
According to the ideal gas law, a 9.702 mol sample of nitrogen gas in a 0.8232 L container at 500.8 K should exert a pressure of 484.3 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol.
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