A tank of volume 1.0 m^3 contains 7.3 moles of nitrogen, 5.2 moles of oxygen, 1.5 moles of helium, and 8.1 moles of carbon dioxide at -75 degrees C. Calculate the partial pressure of each gas in the mixture.

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Beverley SmithLv2

20 Feb 2019

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Mixtures of helium and oxygen are used for scuba diving. For a particular dive, 46 liters of O2 at 25 degrees celsius and 1.0 atm and 12 liters of He at 25 degrees celsius and 1.0 atm are pumped into a tank with a volume of 5.0 liters. Calculate the partial pressure of each gas and the total pressure in the tank at 25 degrees celsius. (Determine moles of each gas first.)

burgundyguinea-pig295

HELP!!! I want to know the step by step process to solve these problems. Italicized and bolded are the answers.

1.) A tank contains 17.00 moles total of carbon dioxide, nitrogen, and oxygen. Calculate the moles of carbon dioxide, if the percent of nitrogen is 44 % and oxygen is 31%. (Hint, convert percent into mole fraction.) 4.2 (4.25) mol Carbon dioxide

2.) A quantity of nitrogen gas originally at 4.60 atm in a 1.20 L container at 23.9 ÂºC is transferred to a 10.0 L container. A quantity of oxygen originally at 3.50 atm and 23.9 ÂºC in a 4.00 L container is transferred to the same 10.0 L container with the ni trogen. Calculate the total pressure of the two gases in the 10.0 L container at 19.7 ÂºC. 1.93 atm

3.) A 50.00 liter tank at - 15.00 Â°C contains 14.00 grams of helium gas and 10.00 grams of nitrogen gas.

a. Determine the total pressure in the tank. P_T = 1.632 atm

b. Determine the partial pressure of each gas. P _He = 1.481 atm PN2 = 0.1512 atm

c. Determine the volume at STP. 86.33 L