A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 640. mL at a pressure of 1.00 atm, and it weighs 0.712 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 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. mole fraction: х10 sulfur tetrafluoride partial pressure: | atm ? mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm

A sample of an unknown compound is vaporized at  100.°C . The gas produced has a volume of  1330.mL  at a pressure of  1.00atm , and it weighs  4.52g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits.

A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 1850. mL at a pressure of 1.00 atm, and it weighs 1.95 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits. g mol x10 X

A 9.00 L tank at 2.1 °C is filled with 7.71 g of boron trifluoride gas and 9.11 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. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: carbon dioxide 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 3.00 atm. key carbon hydrogen nitrogen sulfur oxygen chlorine 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. gas mole fraction partial pressure x10 N₂ 02 atm ☐ ☑ 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 lowered from 23.0°C⁢ to −19.0°C, and at the same time the pressure is changed. If the initial pressure was 6.3atm and the volume increased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits.

A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 2130. mL at a pressure of 1.00 atm, and it weighs 6.27 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. g x10 mol

A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 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. ol. mole fraction: x10 chlorine pentafluoride Ar ? partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

A sample of an unknown compound is vaporized at 150. °C. The gas produced has a volume of 2330. mL at a pressure of 1.00 atm, and it weighs 6.37 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. g mol x10 ×