Use 1 decimal point for all atomic weights (X.X). For the following oxygen, nitrogen, and helium mixture, determine the partial pressure of helium if the gas is 11 g of oxygen, 22 g of nitrogen, and 33 g of helium at a total pressure of 101.3 kPa. ------?   kPa

A 9.00 L tank at 26.5 °C is filled with 3.97 g of carbon monoxide gas and 7.00 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. carbon monoxide sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank 0 atm 0 0. alm atm 0.P X

Please answer all the parts of the following question

A 5.00 L tank at 18.8 °C is filled with 3.00 g of sulfur hexafluoride gas and 3.26 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: sulfur hexafluoride partial pressure: Datm mole fraction: carbon dioxide partial pressure: atm Total pressure in tank: atm O

According to Charles’s law, the volume of a gas is directly related to its temperature in kelvins at constant pressure and the number of moles. In your initial post to the discussion, respond to the following prompts: What if there was an inverse relationship between the temperature and the volume? How do you think the world might be different? How would this change our day-to-day lives? Pick one of the following questions and try to answer it using one of the laws you learned in this module: How do spray cans work? Why do you need to fill up your tires with air on a cold day? Why do soda cans explode? When you inhale, your diaphragm increases in volume. How does this allow you to breathe? How does a syringe fill? How does filling a basketball with air increase its volume?

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

Use 1 decimal point for all atomic weights (X.X). For the following oxygen, nitrogen, and helium mixture, determine the partial pressure of nitrogen if the gas is 101 g of oxygen, 286 g of nitrogen, and 502 g of helium at a total pressure of 400.0 kPa.   ?  kPa?   I put 29.6, then 30 kPa both wrong... ....but don't know why... here is my work O=101/32=3.16, N=286/28=10.21, H=502/4=125.5 Total mol: 138.87  O 3.16/138.87=0.023 N: 10.21/138.87=0.074 H: 125.5/138.87= 0.90 0.074  (N) * 400 kPa= 29.6 kPa

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