A 10.13 mol sample of krypton gas is maintained in a 0.7517 L container at 297.2 K. What is the pressure in atm calculated using the van der Waals' equation for Kr gas under these conditions? For Kr, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol.
A 10.13 mol sample of krypton gas is maintained in a 0.7517 L container at 297.2...
A 9.450 mol sample of krypton gas is maintained in a 0.8100 L container at 300.1 K. What is the pressure in atm calculated using the van der Waals' equation for Kr gas under these conditions? For Kr, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. atm
A 10.33 mol sample of krypton gas is maintained in a 0.7797 L container at 301.0 K. What is the pressure in atm calculated using the van der Waals' equation for Kr gas under these conditions? For Kr, a = 2.318 L’atm/mol and b = 3.978x10-2 L/mol. atm
According to the ideal gas law, a 10.74 mol sample of krypton gas in a 0.8444 L container at 498.7 K should exert a pressure of 520.5 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. ____%
(chp.13) According to the ideal gas law, a 1.010 mol sample of krypton gas in a 1.123 L container at 269.7 K should exert a pressure of 19.90 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. %
According to the ideal gas law, a 1.066 mol sample of krypton gas in a 1.927 L container at 272.4 K should exert a pressure of 12.37 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. ___% Hint: % difference = 100×(P ideal - Pvan der Waals) / P ideal
According to the ideal gas law, a 0.9054 mol sample of krypton gas in a 1.023 L container at 274.0 K should exert a pressure of 19.90 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. % According to the ideal gas law, a 9.344 mol sample of oxygen gas in a 0.8267 L container at 500.1...
A 9.262 mol sample of xenon gas is maintained in a 0.8496 L container at 299.3 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 L2atm/mol2 and b = 5.105×10-2 L/mol.
A 9.386 mol sample of methane gas is maintained in a 0.7854 L container at 302.4 K. What is the pressure in atm calculated using the van der Waals' equation for CH4 gas under these conditions? For CH4, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol.
According to the ideal gas law, a 0.9935 mol sample of krypton gas in a 1.258 L container at 265.4 K should exert a pressure of 17.20 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Kr gas, a - 2.318 L'atm/mol- and b= 3.978*10-2 L/mol. Hint: % difference = 100*(P ideal - Pvan der Waals) /P ideal
A 1.55-mol sample of nitrogen gas is maintained in a 0.730-L container at 292 K. Calculate the pressure of the gas using both the ideal gas law and the van der Waals equation (van der Waals constants for N2 are a = 1.39 L2atm/mol2 and b = 3.91×10-2 L/mol). Pideal gas equation = ______ atm Pvan der Waals =_____ atm