MISSED THIS? Watch KCV: Mixtures of Gases and Partial Pressures, IWE: Partial Pressures and Mole Fractions; Read Section 6.6. You can click on the Review link to access the section in your eText. Composition of Dry Air Gas Percent by Volume (%) Nitrogen (N₂) Oxygen (O₂) Argon (Ar) Carbon dioxide (CO₂) 0.04 78 21 0.9 ▼ Part A What is the mole fraction of oxygen gas in air? (See table for the composition of dry air.) Express the fraction to two significant figures. X = 0.21 Submit ✔ Correct According to Avogadro's law the amount and the volume are directly proportional, so the mole fraction equals the volume fraction. The volume percent of oxygen in air is 21% (see the table below); therefore, the mole fraction is 0.21. Part B Previous Answers Vair 13 = Gas Nitrogen (N₂) Oxygen (O₂) Argon (Ar) Carbon dioxide (CO₂) Percent by volume (%) www. ? 78 21 0.9 What volume of air contains 17.6 g of oxygen gas at 273 K and 1.00 atm? Express your answer using two significant figures. 195] ΑΣΦ 0.04 L

Dinitrogen monoxide gas is collected at 28.0 °C in an evacuated flask with a measured volume of 30.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.290 atm. Calculate the mass and number of moles of dinitrogen monoxide gas that were collected. Be sure your answer has the correct number of significant digits. mass: g dlo mole: |mol I Don't Know Submit O 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

A 6.00 L tank at -2.4 °C is filled with 2.01 g of sulfur tetrafluoride gas and 6.11 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas sulfur tetrafluoride sulfur hexafluoride mole fraction 0 0 X Ś 0 000 13 Ar

A 7.00 L tank at 12.4 °C is filled with 19.4 g of sulfur tetrafluoride gas and 10.3 g of dinitrogen difluoride gas. You can assume both gases behar gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction sulfur tetrafluoride dinitrogen difluoride

A 9.00 L tank at 6.02 °C is filled with 8.81 g of sulfur hexafluoride gas and 10.5 g of dinitrogen difluoride 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. mole fraction: sulfur hexafluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 0.150 kPa. gas N₂ 0₂ carbon nitrogen kPa oxygen mole fraction partial pressure kPa key Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. hydrogen x10 sulfur chlorine × Ś

A 6.00 L tank at 7.53 °C is filled with 5.91 g of sulfur hexafluoride gas and 7.97 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. mole fraction: sulfur hexafluoride partial pressure: ? atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm