**Instructions: Calculating Pressure Using Gas Equations**1. **Van der Waals Equation:** - Calculate the pressure \( P \) of 2.10 mol of \( \text{NH}_3 \) at 487 K in a 3.50 L vessel. - Use the provided [list of van der Waals constants](#) to assist in your calculation. \[ P = \_\_\_\_\_ \, \text{atm} \]2. **Ideal Gas Equation:** - Use the ideal gas equation to calculate the pressure \( P \) under the same conditions. \[ P = \_\_\_\_\_ \, \text{atm} \] - Text boxes are provided to enter the calculated pressures. - The van der Waals equation adjusts the ideal gas law for interactions between molecules and the volumes occupied by them, providing a more accurate calculation for real gases.- The ideal gas equation is a simplified model assuming no intermolecular forces and that the gases occupy no volume. ## Van der Waals ConstantsThe table below lists the Van der Waals constants for various gases. These constants are used in the Van der Waals equation, which is an equation of state for gases. The equation accounts for the volume occupied by gas molecules and the attractive forces between them, which are not considered in the ideal gas law.### Table: Van der Waals Constants| Gas | \( a \) (bar \(\cdot\) L\(^2\)/mol\(^2\)) | \( a \) (atm \(\cdot\) L\(^2\)/mol\(^2\)) | \( b \) (L/mol) ||------|---------------------------------------|---------------------------------------|-----------------|| CH\(_4\) | 2.303 | 2.273 | 0.0431 || CO\(_2\) | 3.658 | 3.610 | 0.0429 || Cl\(_2\) | 6.343 | 6.260 | 0.0542 || NH\(_3\) | 4.225 | 4.170 | 0.0371 || H\(_2\)O | 5.537 | 5.465 | 0.0305 || Xe | 4.192 | 4.137 | 0.0516 || CCl\(_4\) | 20.01 | 19.75 | 0.1281 || O\(_2\) | 1.382 | 1.360 | 0.0318 || N\(_2\) | 1.370 | 1.351 | 0.0387 || Kr | 5.193 | 5.152 | 0.0320 || Ar | 1.355 | 1.336 | 0.0320 || CO | 1.472 | 1.452 | 0.0395 || H\(_2\)S | 4.544 | 4.417 | 0.0436 || NO | 1.414

Van der Waal Equation: P = nRTV-nb-an2V2 where P = Pressure, V = Volume, n= no. of moles T =…

Use the van der Waals equation of state to calculate the pressure P of 2.10 mol of NH, at 487 K in a 3.50 L vessel. Use this list of van der Waals constants. P = atm Use the ideal gas equation to calculate the pressure P under the same conditions. atm P =

Use the van der Waals equation of state to calculate the pressure P of 2.10 mol of NH, at 487 K in a 3.50 L vessel. Use this list of van der Waals constants. P = atm Use the ideal gas equation to calculate the pressure P under the same conditions. atm P =

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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