5) Ideal and real (van der Waals) gas. The sample of xenon gas with mass of 131 g is placed in a vessel of volume 1.0 L. a) Assuming perfect gas behavior, calculate its pressure; b) assuming it behaves as a van der Waals gas, calculate its pressure.

5) Ideal and real (van der Waals) gas. The sample of xenon gas with mass of 131 g is placed in a vessel of volume 1.0 L. a) Assuming perfect gas behavior, calculate its pressure; b) assuming it behaves as a van der Waals gas, calculate its pressure.

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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Answer part a and b
In general, real gases behave most ideally at _____(highORlow) temperatures and _____(highORlow) pressures.The behavior of real gases can be described using the van der Waals equation[P + (n2a/V2)](V-nb) = nRT The values of a and b are given below for the two real gases xenon and neon.The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the largest is _______(xenon OR neon)The gas that would be expected to behave most like an ideal gas at high pressures is _______(xenon OR neon.) gas a (L2atm/mol2) b (L/mol) Xe 4.19 5.11×10-2 Ne 0.211 1.71×10-2
Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 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 Under these conditions, would you expect HI or CCl, to deviate more from ideal behavior? Why? CCl because it occupies a larger volume and it has smaller dispersion forces between molecules. HI because it occupies a smaller volume and it has smaller dispersion forces between molecules. HI because it occupies a larger volume and it has smaller dispersion forces between molecules. CCI, because it occupies a larger volume and it has greater dispersion forces between molecules. HI because it occupies a smaller volume and it has greater dispersion forces between molecules. CCI, because it occupies a smaller volume and it has greater dispersion forces between molecules.
Please do not round off sig figs in calculations until final answer. Thank you.
What are the units of a? What are the units of b? For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 55.0 °C with a molar volume of 0.515 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm Explanation Check
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: p+a n #2²7) (V- (V-nb)=nRT The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. What are the units of b? For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 1.92 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. 1 0 П atm atm x10 H X ロ・ロ S
Real gases differ in characteristics from ideal gases. O True False
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: n (p+₁ +²2) (v- (V-nb)=nRT The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. What are the units of b? For ethane the numerical value of a is 5.507 and the numerical value of b is 0.0651. Use the van der Waals equation to calculate the pressure of a sample of ethane at 105.0 °C with a molar volume of 5.27 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. 0 0 atm atm x10 DO X ロ・ロ

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature I for gases better than the Ideal Gas Law does: 72 (V-nb)= nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For argon the numerical value of a is 1.337 and the numerical value of b is 0.0320. Use the van der Waals equation to calculate the pressure of a sample of argon at -110.0 °C with a molar volume of 2.98 L/mol Round your answer to the correct number of significant digits. atm Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. atm x10 §