Use the van der Waals equation of state to calculate the pressure of 3.90 mol of Kr at 467 K in a 3.80 L vessel. Van der Waals constants can be found in the van der Waals constants table.   Use the ideal gas equation to calculate the pressure under the same conditions.   In a 16.80 L vessel, the pressure of 3.90 mol of Kr at 467 K is 8.90atm when calculated using the ideal gas equation and 8.64 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 3.80 L compared to the  16.80 L vessel?

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Chapter5: The Gaseous State
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Problem 5.103QP: Calculate the molar volume of ethane at 1.00 atm and 0C and at 10.0 atm and 0C, using the van der...
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Use the van der Waals equation of state to calculate the pressure of 3.90 mol of Kr at 467 K in a 3.80 L vessel. Van der Waals constants can be found in the van der Waals constants table.

 

Use the ideal gas equation to calculate the pressure under the same conditions.

 

In a 16.80 L vessel, the pressure of 3.90 mol of Kr at 467 K is 8.90atm when calculated using the ideal gas equation and 8.64 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 3.80 L compared to the  16.80 L vessel?

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