According to the ideal gas law, a 9.732 mol sample of argon gas in a 0.8289 L container at 499.6 K should exert a pressure of 481.3 atm. What is the percent difference between
the pressure calculated using the van der Waals’ equation and the ideal pressure? For Ar gas, a = 1.345 L’atm/mo12 and b = 3.219×10-2 L/mol.
|Pideal Pvan der Waals |
A 9.722 mol sample of xenon gas is maintained in a 0.7906 L container at 298.7 K. What is the pressure in atm calculated using the van der Waals’ equation for Xe gas under
these conditions? For Xe, a = 4.194 L’atm/mo12 and b = 5.105×10-2 L/mol.
A mixture of neon and methane gases, at a total pressure of 920 mm Hg, contains 6.54 grams of neon and 2.07 grams of methane. What is the partial pressure of each gas in
A mixture of krypton and carbon dioxide gases contains krypton at a partial pressure of 254 mm Hg and carbon dioxide at a partial pressure of 499 mm Hg. What is the mole
fraction of each gas in the mixture?
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