A gas mixture contains 0.600  mol of N2, 0.200  mol of H2, and 0.250  mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 9.00  L vessel at 27.00°C. What is the total pressure of the vessel and the pressure of N2, H2, and CH4 in atm?

A 9.00 L tank at 0.61 °C is filled with 6.67 g of sulfur hexafluoride gas and 5.00 g of dinitrogen monoxide 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 monoxide partial pressure: atm Total pressure in tank: atm

A mixture of gases has 0.3000 mol of CO2, 0.3190 mol of SO2 and 0.3500 mol of water vapor. The total pressure of the mixture is 1.500 atm. What is the partial pressure of SO2 in atm?

A gas mixture contains 1.0 mol neon, 2.0 mol argon, and 3.0 mol krypton in a 10.0 L flask at 0°C. Determine the partial pressure of neon.

A 9.00 L tank at 3.79 °C is filled with 8.94 g of sulfur tetrafluoride gas and 13.3 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. Round each of your answers to 3 significant digits. sulfur tetrafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atm X

A 8.00 L tank at 29.8 °C is filled with 14.1 g of chlorine pentafluoride gas and 17.2 g of boron trifluoride gas. You can assume both gases behave as ideal gase under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas chlorine pentafluoride boron trifluoride mole fraction 0 0 X

A 8.00 L tank at 11.8 °C is filled with 7.85 g of carbon dioxide gas and 3.51 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: 0 x10 carbon dioxide partial pressure: atm mole fraction: 0 boron trifluoride partial pressure: atm Total pressure in tank: atm

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

Suppose that Daniel has a 2.50 L bottle that contains a mixture of O₂, N₂, and CO₂ under a total pressure of 5.30 atm. He knows that the mixture contains 0.210 mol N, and that the partial pressure of CO₂ is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O₂? atm Po,

A 9.00 L tank at 26.4 °C is filled with 4.04 g of dinitrogen difluoride gas and 17.1 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. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm