A gas mixture has partial pressures of 52.55 mmHg H2, 159.74 mmHg N2, and 362.99 mmHg  O2. What is the mole fraction of O2 in the mixture? Report your answer with two decimals.

A gas mixture contains an unknown amount of NO and 0.1343 mol of CO. How many moles of NO are there, if the total pressure is 904.99 mm Hg and the partial pressure of NO is 389.73 mm Hg?

Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1100. torr, key carbon hydrogen nitrogen sulfur охудen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr ? O2 torr

A 8.00 L tank at 21.1 °C is filled with 11.6 g of chlorine pentafluoride gas and 12.6 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: x10 chlorine pentafluoride partial pressure: ? atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm

A 10.00 L tank at -7.6 °C is filled with 5.09 g of chlorine pentafluoride gas and 16.3 g of dinitrogen difluoride 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 chlorine pentafluoride dinitrogen difluoride mole fraction 0 10 X S

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 0.060 kPa. gas N₂ carbon mole fraction Ú nitrogen oxygen key partial pressure kPa kPa Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 2 significant digits. You may assume each gas behaves as an ideal gas. 0 hydrogen x10 sulfur chlorine X

Chlorine pentafluoride gas is collected at -17.0 °C in an evacuated flask with a measured volume of 50.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.330 atm . Calculate the mass and number of moles of chlorine pentafluoride gas that were collected. Round your answer to 3 significant digits. mass: g x10 mole: || mol

A 9.00 L tank at 1.5 °C is filled with 3.22 g of carbon monoxide gas and 16.7 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. Be sure your answers have the correct number of significant digits. carbon monoxide chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm x10 × Ś 0:39 0 E

A 6.00 L tank at 6.04 °C is filled with 18.4 g of sulfur hexafluoride gas and 2.89 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: Ox10 sulfur hexafluoride partial pressure: atm mole fraction: carbon dioxide partial pressure: atm Total pressure in tank: atm

For many purposes we can treat ammonia  NH3  as an ideal gas at temperatures above its boiling point of  −33.°C .   Suppose the temperature of a sample of ammonia gas is raised from  −14.0°C  to  −1.0°C , and at the same time the pressure is increased by  15.0% .       Does the volume of the sample increase, decrease, or stay the same?   increase decrease stays the same       If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent. %