30. A 1.75L container holds 32.5 mol of Xe at 750C. Calculate the pressure of the...
U20 9. Using the van der Waals equation, calculate the pressure for a 1.25 mol sample of xenon contained in a volume of 1.000L at 75°C: a = 4.194 L'atm/mol and b = 0.05105 L/mol for Xe. Compare these results to that predicted by the ideal gas law.
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.
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 10.01 mol sample of xenon gas in a 0.8137 L container at 500.4 K should exert a pressure if 505.1 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 L^2atm/mol^2 and b = 5.105 x 10^-2 L/mol.
According to the ideal gas law, a 0.9249 mol sample of xenon gas in a 1.135 L container at 269.1 K should exert a pressure of 17.99 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Xe gas, a = 4.194 L^2atm/mol^2 and b = 5.105 times 10^-2 L/mol. %
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
Use the References to access important values if needed for this question. According to the ideal gas law, a 0.9428 mol sample of xenon gas in a 1.859 L container at 272.4 K should exert a pressure of 11.34 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 L’atm/mol2 and b = 5.105x10-2 L/mol. Percent difference = 14 Pideal – Pvan der Waals x...
9. Calculate the pressure exerted by 5.00 mol of Co2 in a 1.00 L vessel at 300 K (a) assuming the gas behaves ideally and (b) using the van der Waals equation. (a= 3.610 L'atm/mol, and b = 0.0429 L/mol).
use the van der Waals equation of state to calculate the pressure of 2.30 mol of Xe 481 K in 5.20 L vessel. Use the list of van der Waals constants. P=? Use the ideal gas equation to calculate the pressure under the same conditions. P=?
According to the ideal gas law, a 0.9832 mol sample of carbon dioxide gas in a 1.975 L container at 271.4 K should exert a pressure of 11.09 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For CO2 gas, a = 3.592 L'atm/mol and b=4.267x102 L/mol. Hint: % difference = 100*(P ideal - Pvan der Waals)/P ideal