Question

Use the van der Waals equation of state to calculate the pressure of 2.40 mol of H₂S at 499K in a 4.60 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 16.30 L vessel, the pressure of 2.40 mol of H₂S at 499 K is 6.03 atm when calculated using the ideal gas equation and 5.97 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 4.60 L vessel compared to the 16.30 L vessel? 

• The attractive forces between molecules become a greater factor at the higher pressure in the 4.60 L vessel. 

• The attractive forces between molecules become less of a factor at the higher pressure in the 4.60L vessel. 

• The molecular volume is a larger part of the total volume of the 4.60 L vessel. 

• The molecular volume is a smaller part of the total volume of the 4.60L vessel.

Answer 1

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