A 10.42 mol sample of methane gas is maintained in a 0.8003 L container at 302.3 K. What is the pressure in atm calculated using the van der Waals' equation fora 2.253 L2atm/mol2 and b = 4.278x102 L/mol.CH4 gas under these conditions? For CH4atm

The vander Waals’ equation is given as

Answered: A 10.42 mol sample of methane gas is…

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. 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. atm Use the van der Waals equation to calculate the pressure of a
Calculate the pressure (in atm) of a 5.30 mol sample of nitrogen gas at 200.0 K in a 2.00 L container using the van der Waals equation. For nitrogen, a = 1.39 L²･atm/mol² and b = 0.0391 L/mol.
Calculate the pressure (in atm) of a 4.50 mol sample of ammonia gas at 350.0 K in a 3.00 L container using the van der Waals equation. For ammonia, a = 4.17 L²･atm/mol² and b = 0.03712 L/mol.
For molar masses, use 35.45 for chlorine and 1.008 for hydrogen. It will make a difference if you use a periodic table that has different ones. Given the Van der Waals constants for hydrogen chloride, below, calculate the pressure in atmospheres of 2.19 kilograms of hydrogen chloride gas in a 25.0 L container at 18°C. a(HCl) = 3.65 L^2 atm/mol^2 b(HCl) = 0.0406 L/mol a. 42.5 atm b. 6422 atm c. 377 atm d. 0.057 atm e. -17.1 atm
What would be the pressure (in atm) of a 5.00 mol sample of Cl₂ at 400.0 K in a 2.00 L container found using the van der Waals equation? For Cl₂, a = 6.49 L²･atm/mol² and b = 0.0652 L/mol.
Calculate the pressure of a 14.6 L container with 60.6 moles of hydrogen, at -14.5 degree C, assuming ideal conditions, and then calculate it assuming the gas is not behaving ideally. Compare the two values, and determine explain if the ideal gas law is appropriate to determine the pressure under these conditions. The van der waal constants for hydrogen are a=0.244(atm*L2 )/mol2 and b=0.0266 L/mol.
A 10.12 mol sample of argon gas is maintained in a 0.8094 L container at 304.4 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol. atm
Calculate the pressure (in atm) of a 2.10 mol sample of ammonia gas at 350.0 K in a 3.00 L container using the van der Waals equation. For ammonia, a = 4.17 L².atm/mol² and b = 0.03712 L/mol.
Calculate the pressure (in atm) of a 2.70 mol sample of ammonia gas at 350.0 K in a 3.00 L container using the van der Waals equation. For ammonia, a = 4.17 L²･atm/mol² and b = 0.03712 L/mol.
Suppose 10.05 mol of Ar gas are pumped into a 1.16 L container at 293.15 K Calculate an estimate of the gas pressure one might observe based on the van der Waals equation, Pobs.a = 1.34 L2 · atm/mol2, b = 0.0322 L/mol.
A sample of an ideal gas has a volume of 2.35 L2.35 L at 289 K289 K and 1.14 atm.1.14 atm. Calculate the pressure when the volume is 1.40 L1.40 L and the temperature is 3.00×102 K.
A10.12 mol sample of krypton gas is maintained in a 0.8044 L container at 301.1 K What is the pressure in atm calculated using the van der Waals' equation for Kr gas under these conditions? For Kr, a 2.318 L'atm/mol2 and b = 3.978x10-2 L/mol. atm

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A 10.42 mol sample of methane gas is maintained in a 0.8003 L container at 302.3 K. What is the pressure in atm calculated using the van der Waals' equation for a 2.253 L2atm/mol2 and b = 4.278x102 L/mol. CH4 gas under these conditions? For CH4 atm