B. Consider the same ideal gas within an adiabatically sealed container. Suppose that the ideal gas is initially in an equilibrium state with volume Va and temperature Tr. Suppose that the ideal gas then undergoes a free expansion (i.e., the gas expands against a vacuum) from Va → Vz.

B. Consider the same ideal gas within an adiabatically sealed container. Suppose that the ideal gas is initially in an equilibrium state with volume Va and temperature Tr. Suppose that the ideal gas then undergoes a free expansion (i.e., the gas expands against a vacuum) from Va → Vz.

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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I need help with part A and B
Please answer the question Below.
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
I only need help with part b
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.
i need help with this
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
10b
The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed %3D where R = 8.314 J/(mol-K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-m²/s²). What is the rms speed of O, molecules at 411 K? rms speed: m/s What is the rms speed of He atoms at 411 K? rms speed: m/s
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

Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4 NH₂(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.95 g NH3 reacts with 5.93 g O₂ and produces 0.850 L. N₂ at 295 K and 1.00 bar, how many moles of N₂ can be produced by each reactant? It may be useful to consult the periodic table. NH₂: 0₂: Based on the theoretical yields, which reactant is limiting? NH,(aq) 0₂(g) What is the percent yield of the reaction? percent yield: mol N₂ mol N₂ 28
a cylinder was connected to an open ended U-tube (1 atm) containing some mercury, Hg (density=13.6gcm^-3), and the Hg was displaced 100mm towards the container. What is the pressure of the gas inside the container?