According to the ideal gas law, a 10.12 mol sample of krypton gas in a 0.8350 L container at 495.1 K should exert a pressure of 492.4 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L²atm/mol? and b = 3.978×10² L/mol. [Pideal – Pvan der Waals| x 100 Percent difference Pideal+P der Waals van

According to the ideal gas law, a 10.12 mol sample of krypton gas in a 0.8350 L container at 495.1 K should exert a pressure of 492.4 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L²atm/mol? and b = 3.978×10² L/mol. [Pideal – Pvan der Waals| x 100 Percent difference Pideal+P der Waals van

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter10: Gases And Their Properties

Section: Chapter Questions

Problem 53PS: In the text, it is stated that the pressure of 4.00 mol of Cl2 in a 4.00-L tank at 100.0 C should be...

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In the text, it is stated that the pressure of 4.00 mol of Cl2 in a 4.00-L tank at 100.0 C should be 26.0 atm if calculated using the van der Waals equation. Verify this result, and compare it with the pressure predicted by the ideal gas law.
You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?
A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?
Butyl mercaptan, C4H9SH, has a very bad odor and is among the compounds added to natural gas to help detect a leak of otherwise odorless natural gas. In an experiment, you burn 95.0 mg of C4H9SH and collect the product gases (SO2, CO2, and H2O) in a 5.25-L flask at 25 C. What is the total gas pressure in the flask, and what is the partial pressure of each of the product gases?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
59 During a collision, automobile air bags are inflated by the N2 gas formed by the explosive decomposition of sodium azide, NaN3: 2NaN32Na+3N2 What mass of sodium azide would be needed to inflate a 30.0-L bag to a pressure of 1.40 atm at 25 C?