(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. %
(chp.13) According to the ideal gas law, a 1.010 mol sample of krypton gas in a...
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. ____%
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...
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 0.9935 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 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 10.13 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.
According to the ideal gas law, a 10.65 mol sample of krypton gas in a 0.8201 L container at 496.1 K should exert a pressure of 528.7 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 LPatm/mol? and b 3.978x102 L/mol. Pideal-Poan der Woals Percent difference x 100 Pnal+Pn der Waals 2 %
According to the ideal gas law, a 0.9988 mol sample of xenon gas in a 1.401 L container at 267.4 K should exert a pressure of 15.64 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L2atm/mol2 and b = 5.105×10-2 L/mol. %
According to the ideal gas law, a 1.001 mol sample of argon gas in a 1.589 L container at 270.1 K should exert a pressure of 13.96 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 L2atm/mol2 and b = 3.219×10-2 L/mol.
According to the ideal gas law, a 1.099 mol sample of nitrogen gas in a 1.520 L container at 271.3 K should exert a pressure of 16.10 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.