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 andtemperature 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 numericalvalue of b is 0.0320.Use the van der Waals equation to calculate the pressure of asample of argon at -110.0 °C with a molar volume of 2.98 L/molRound your answer to the correct number of significant digits.atmUse the Ideal Gas Law to calculate the pressure of the samesample under the same conditions. Round your answer to thecorrect number of significant digits.atmx10§

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Answered: The van der Waals equation of state was…

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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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- |(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. Ar What are the units of a? 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. Oat ||atm Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 4.03 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. atm
Water vapor is a polar gas molecule. Because of this it has fairly strong interactions with itself in the gas phase that can make it behave less like an ideal gas that other gases under similar conditions. What is the difference between the calculated pressures found using the ideal gas law and found using the van der Waals gas equation for 1 mole of water vapor at -100°C in a 1.00L container. (van der Waals constants for water are a = 5.464 L2 atm mol-2, b = 0.03049 L mol-1) i atm
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+a- (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. For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. | atm Use the van der Waals equation to calculate the pressure of a sample of water at 445.0 °C with a molar volume of 2.47 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 APR 49 X W 24 : MacBook Air DD 80 DO0 O00 888 F9 F10 F7 F8 F5 F6 F2 F3 F4
[References) Use the References to access important values if needed for this question. According to the ideal gas law, a 0.9550 mol sample of carbon dioxide gas in a 1.558 L container at 268.2 K should exert a pressure of 13.49 atm. What is the percent difference between the pressure calculated using the van der Waal equation and the ideal pressure? For CO, gas, a = 3.592 L2atm/mol? and b = 4.267x10-2 L/mol. Pideal - Puan der Waols Peal +Pean der Wade Percent difference = x 100
Assuming that a 800 mg gas occupying a volume of 1,100 ml at a pressure of 1,600 mmHg and a temperature of 75 deg. C is behaving like an ideal gas. What is the molecular weight of the gas?
Please do not round off sig figs in calculations until final answer. Thank you.
A 9.00 L tank at 18.1 °C is filled with 3.17 g of dinitrogen monoxide gas and 8.90 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas dinitrogen monoxide carbon monoxide mole fraction
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: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? 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 ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 195.0 °C with a molar volume of 4.12 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 O
Give some application and importance of the Ideal Gas Laws.
A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. ol. mole fraction: x10 chlorine pentafluoride Ar ? partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm
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

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