Use the van der Waals equation of state to calculate the pressure of 2.30 mol of CCI, at 455K in a 5.80 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = 4.94 Incorrect Use the ideal gas equation to calculate the pressure under the same conditions. P = 15.05 In a 16.80 L vessel, the pressure of 2.30 mol of CC14 at 455 K is 5.11 atm when calculated using the ideal gas equation and 4.83 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 5.80 L vessel compared to the 16.80 L vessel? The molecular volume is a smaller part of the total volume of the 5.80L vessel. The molecular volume is a larger part of the total volume of the 5.80 L vessel. The attractive forces between molecules become a greater factor at the higher pressure in the 5.80 L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 5.80L vessel. atm atm
Use the van der Waals equation of state to calculate the pressure of 2.30 mol of CCI, at 455K in a 5.80 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = 4.94 Incorrect Use the ideal gas equation to calculate the pressure under the same conditions. P = 15.05 In a 16.80 L vessel, the pressure of 2.30 mol of CC14 at 455 K is 5.11 atm when calculated using the ideal gas equation and 4.83 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 5.80 L vessel compared to the 16.80 L vessel? The molecular volume is a smaller part of the total volume of the 5.80L vessel. The molecular volume is a larger part of the total volume of the 5.80 L vessel. The attractive forces between molecules become a greater factor at the higher pressure in the 5.80 L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 5.80L vessel. atm atm
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Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.127QP: A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000...
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Use the van der Waals equation of state to calculate the pressure of 2.30 mol of CC14 at 455K in a 5.80 L vessel. Van der Waals
constants can be found in the van der Waals constants table.
P =
4.94
Incorrect
Use the ideal gas equation to calculate the pressure under the same conditions.
P =
15.05
In a 16.80 L vessel, the pressure of 2.30 mol of CCl4 at 455 K is 5.11 atm when calculated using the ideal gas equation and
4.83 atm when calculated using the van der Waals equation of state.
Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the
5.80 L vessel compared to the 16.80 L vessel?
The molecular volume is a smaller part of the total volume of the 5.80L vessel.
The molecular volume is a larger part of the total volume of the 5.80 L vessel.
The attractive forces between molecules become a greater factor at the higher pressure in the 5.80 L vessel.
The attractive forces between molecules become less of a factor at the higher pressure in the 5.80L vessel.
atm
atm
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