A 5.00 L lank al 2.19 °C IS leu with 5.75 g Ol gas anu g Ol Tur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditi Calculate the mole fraction and partial pressure of each gas, and the total pressure in th tank. Round each of your answers to 3 significant digits. mole fraction: chlorine pentafluoride partial pressure: atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm

A 5.00 L lank al 2.19 °C IS leu with 5.75 g Ol gas anu g Ol Tur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditi Calculate the mole fraction and partial pressure of each gas, and the total pressure in th tank. Round each of your answers to 3 significant digits. mole fraction: chlorine pentafluoride partial pressure: atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.93PAE: 93 The complete combustion of octane can be used as a model for the burning of gasoline:...

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93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.
A mixture of N2 and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 15.00 atm? Assume ideal gas behavior.
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.
Butane, C4H10, is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.857 atm and 22C. Give the answer in grams per liter
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