A 8.00 L tank at 12.6 °C is filled with 3.51 g of carbon monoxide gas and 12.1 g of boron trifluoride 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. carbon monoxide boron trifluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm 10 X

A 8.00 L tank at 12.6 °C is filled with 3.51 g of carbon monoxide gas and 12.1 g of boron trifluoride 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. carbon monoxide boron trifluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm 10 X

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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A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?
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?
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.)
Describe the factors responsible for the deviation of the behavior of real gases from that of an ideal gas.
In the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.
Referring to exercises 1.6 and 1.7, does it matter if the pressure difference is caused by an ideal gas or a non-ideal gas? Explain your answer.