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A 10.0 L tank at 22.1 °C is filled with 4.97 g of boron trifluoride gas and 7.95 g of sulfur hexafluoride 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. Be sure your answers have the correct number of significant digits. mole fraction: boron trifluoride partial pressure: |atm X. mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

A 10.0 L tank at 22.1 °C is filled with 4.97 g of boron trifluoride gas and 7.95 g of sulfur hexafluoride 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. Be sure your answers have the correct number of significant digits. mole fraction: boron trifluoride partial pressure: |atm X. mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

Chemistry
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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**Calculating Partial Pressure in a Gas Mixture** A 10.0 L tank at 22.1 °C is filled with 4.97 g of boron trifluoride gas and 7.95 g of sulfur hexafluoride 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. Be sure your answers have the correct number of significant digits. | **Component** | **Mole Fraction** | **Partial Pressure (atm)** | |---------------------|-------------------|----------------------------| | Boron trifluoride | | | | Sulfur hexafluoride | | | | **Total pressure in tank:** | | | To perform these calculations, you'll need to use the ideal gas law and understand mole fractions. Remember, mole fractions are the ratio of the number of moles of one particular gas to the total number of moles of gas in the mixture. **Tools Available:** - A calculator interface for performing calculations - Input fields to fill in your answers Make sure to use proper significant figures based on the input data provided. If you require additional help in solving this problem, please refer to the "Explanation" section or check your answers using the "Check" function.
Transcribed Image Text:**Calculating Partial Pressure in a Gas Mixture** A 10.0 L tank at 22.1 °C is filled with 4.97 g of boron trifluoride gas and 7.95 g of sulfur hexafluoride 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. Be sure your answers have the correct number of significant digits. | **Component** | **Mole Fraction** | **Partial Pressure (atm)** | |---------------------|-------------------|----------------------------| | Boron trifluoride | | | | Sulfur hexafluoride | | | | **Total pressure in tank:** | | | To perform these calculations, you'll need to use the ideal gas law and understand mole fractions. Remember, mole fractions are the ratio of the number of moles of one particular gas to the total number of moles of gas in the mixture. **Tools Available:** - A calculator interface for performing calculations - Input fields to fill in your answers Make sure to use proper significant figures based on the input data provided. If you require additional help in solving this problem, please refer to the "Explanation" section or check your answers using the "Check" function.
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