**Van der Waals Equation vs. Ideal Gas Equation: Analysis of Pressure for SO₂**In this exercise, you are asked to calculate the pressure of sulfur dioxide (SO₂) using two different equations of state: the van der Waals equation and the ideal gas equation.1. **Van der Waals Equation Calculation** - **Variables Given:** - \( n = 3.70 \, \text{mol} \) - \( T = 499 \, \text{K} \) - \( V = 3.50 \, \text{L} \) - Use the van der Waals equation of state with constants to calculate the pressure \( P \). - **Calculation Box:** You will need to enter the calculated pressure value here: \( P = \underline{\hspace{3cm}} \, \text{atm} \)2. **Ideal Gas Equation Calculation** - Calculate the pressure using the ideal gas equation under the same conditions. - **Calculation Box:** Enter the calculated pressure value here: \( P = \underline{\hspace{3cm}} \, \text{atm} \)3. **Comparison of Calculations** - When applying these equations in a 15.50 L vessel: - Using the **ideal gas equation**, the pressure is 9.77 atm. - Using the **van der Waals equation**, the pressure is 9.52 atm.4. **Conceptual Question** - Consider why the percent difference in calculated pressures is greater in a 3.50 L vessel compared to a 15.50 L vessel. - **Options to Consider:** - The attractive forces between molecules become less of a factor at the higher pressure in the 3.50 L vessel. - The molecular volume is a larger part of the total volume of the 3.50 L vessel. - The attractive forces between molecules become a greater factor at the higher pressure in the 3.50 L vessel. - The molecular volume is a smaller part of the total volume of the 3.50 L vessel.Select the option that best explains the observed difference.**Note:** The van der Waals equation adjusts for intermolecular forces and finite molecular size, providing a more accurate representation than the ideal gas law under certain conditions, particularly at high pressure or low volume.

Given : Moles of gas SO2 = n = 3.70 mol Temperature = T = 499 K Volume of vessel = V = 3.50 L We…

Use the van der Waals equation of state to calculate the pressure of 3.70 mol of SO, at 499K in a 3.50 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm In a 15.50 L vessel, the pressure of 3.70 mol of SO, at 499 K is 9.77 atm when calculated using the ideal gas equation and 9.52 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 3.50 L vessel compared to the 15.50 L vessel? The attractive forces between molecules become less of a factor at the higher pressure in the 3.50L vessel. The molecular volume is a larger part of the total volume of the 3.50 L vessel. O The attractive forces between molecules become a greater factor at the higher pressure in the 3.50 L vessel. The molecular volume is a smaller part of the total volume of the 3.50L vessel. O O

Use the van der Waals equation of state to calculate the pressure of 3.70 mol of SO, at 499K in a 3.50 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm In a 15.50 L vessel, the pressure of 3.70 mol of SO, at 499 K is 9.77 atm when calculated using the ideal gas equation and 9.52 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 3.50 L vessel compared to the 15.50 L vessel? The attractive forces between molecules become less of a factor at the higher pressure in the 3.50L vessel. The molecular volume is a larger part of the total volume of the 3.50 L vessel. O The attractive forces between molecules become a greater factor at the higher pressure in the 3.50 L vessel. The molecular volume is a smaller part of the total volume of the 3.50L vessel. O O

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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