A tank is filled with 8.97 moles O2(g), 2.82 moles N2(g), and 2.3 moles of Ar,...
A tank is filled with 8.97 moles O2(g), 2.82 moles N2(g), and 2.3 moles of Ar, giving a final take pressure of 6.35 atm. What is the partial pressure of agron gas in the tank?
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A tank is filled with 8.97 moles O2(g), 2.82 moles N2(g), and
2.3 moles of Ar,...
a rigid oxygen tank with 150 grans of O2 was inflated with more O2 from 3.5...
a rigid oxygen tank with 150 grans of O2 was inflated with more O2 from 3.5 atm to 15 atm at a constant orwssure. Find the final moles and grams od O2 in the tank N2(g) was collected over water in a volume id 16.2 mL at 25*C under atmospherix pressure of 780 Torr. partial pressure if water is P(H2O,25*C)= 24 Torr. Find mols of N2 1. A rigid oxygen tank with 150 grams of O2 was inflated with more...
1. A container is filled with 16.0 g of O2 and 14.0 g of N2. a....
1. A container is filled with 16.0 g of O2 and 14.0 g of N2. a. What is the volume of the container at STP? b. What is the partial pressure of the O2 gas? c. What is the mole fraction of N2 in the mixture? 2. Look carefully at the following reaction: N2(g) + 3H2(g) -> 2NH3(g) How will the enthalpy change (H) compared to the internal energy change (E) for this reaction? That is, will H be equal...
A 5.00 L tank at 24.6 °C is filled with 2.30 g of carbon dioxide gas...
A 5.00 L tank at 24.6 °C is filled with 2.30 g of carbon dioxide gas and 3.32 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. Be sure your answers have the correct number of significant digits. mole fraction: carbon dioxide partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 9.00 L tank at 21.4 °C is filled with 6.62 g of dinitrogen difluoride gas...
A 9.00 L tank at 21.4 °C is filled with 6.62 g of dinitrogen difluoride gas and 16.5 g of sulfur tetrafluoride 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: 3 dinitrogen difluoride partial pressure: atm Х ? mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure...
A 10.00 L tank at 23.2 degrees Celsius is filled with 15.8 g of dinitrogen monoxide...
A 10.00 L tank at 23.2 degrees Celsius is filled with 15.8 g of dinitrogen monoxide gas and 4.94 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. What is the mole fraction and partial pressure for dinitrogen monoxide? Mole fraction: ? Partial pressure: ? atm What is the mole fraction and partial pressure for sulfur tetrafluoride? Mole fraction:? Partial pressure: ? atm What is the total pressure in the tank? Round...
A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas...
A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas and 10.1 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. Be sure your answers have the correct number of significant digits. mole fraction: chlorine pentafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 6.00 L tank at 2.56 °C is filled with 5.50 g of sulfur hexafluoride gas...
A 6.00 L tank at 2.56 °C is filled with 5.50 g of sulfur hexafluoride gas and 13.0 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. Be sure your answers have the correct number of significant digits. mole fraction: sulfur hexafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 8.00 L tank at 1.88 °C is filled with 2.53 g of dinitrogen difluoride gas...
A 8.00 L tank at 1.88 °C is filled with 2.53 g of dinitrogen difluoride gas and 5.50 g of chlorine pentafluoride 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: dinitrogen difluoride partial pressure: atmx ? mole fraction: chlorine pentafluoride partial pressure: | atm Total...
A 8.00 L tank at 10.2 °C is filled with 8.47 g of chlorine pentafluoride gas...
A 8.00 L tank at 10.2 °C is filled with 8.47 g of chlorine pentafluoride gas and 12.1 g of carbon dioxide 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: chlorine pentafluoride partial pressure: | atm x 6 ? mole fraction: carbon dioxide partial pressure:...
A 5.000 L tank at 11.2 °C is filled with 3.68 g of dinitrogen difluoride gas...
A 5.000 L tank at 11.2 °C is filled with 3.68 g of dinitrogen difluoride gas and 12.7 g of chlorine pentafluoride 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 וים dinitrogen difluoride partial pressure: atm mole fraction chlorine pentafluoride partial pressure: atim Total pressure in tank...
A 5.00 L tank at 24.6 °C is filled with 2.30 g of carbon dioxide gas and 3.32 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. Be sure your answers have the correct number of significant digits. mole fraction: carbon dioxide partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 9.00 L tank at 21.4 °C is filled with 6.62 g of dinitrogen difluoride gas and 16.5 g of sulfur tetrafluoride 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: 3 dinitrogen difluoride partial pressure: atm Х ? mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure...
A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas and 10.1 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. Be sure your answers have the correct number of significant digits. mole fraction: chlorine pentafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 6.00 L tank at 2.56 °C is filled with 5.50 g of sulfur hexafluoride gas and 13.0 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. Be sure your answers have the correct number of significant digits. mole fraction: sulfur hexafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...
A 8.00 L tank at 1.88 °C is filled with 2.53 g of dinitrogen difluoride gas and 5.50 g of chlorine pentafluoride 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: dinitrogen difluoride partial pressure: atmx ? mole fraction: chlorine pentafluoride partial pressure: | atm Total...
A 8.00 L tank at 10.2 °C is filled with 8.47 g of chlorine pentafluoride gas and 12.1 g of carbon dioxide 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: chlorine pentafluoride partial pressure: | atm x 6 ? mole fraction: carbon dioxide partial pressure:...
A 5.000 L tank at 11.2 °C is filled with 3.68 g of dinitrogen difluoride gas and 12.7 g of chlorine pentafluoride 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 וים dinitrogen difluoride partial pressure: atm mole fraction chlorine pentafluoride partial pressure: atim Total pressure in tank...
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