. . . A vessel (flask) contains equal moles of each of the following gases: CH4, He and NO₂. The gases are contained in a 10.0 liter flask at room temperature (25.0°C). The flask develops a pinhole leak allowing the gases to escape. Determine which of the following describes the relationship between the partial pressures of each of the gases left in the container after one hour have passed since the the container sprang a leak. PNO2 PCH4 - PHe PNO2PCH4 < PHe PNO2 PCH4> PHe PNO2PCH4> PHe >

The typical human lung has a volume when full of approximately 5.0 L. The partial pressure of oxygen in the atmosphere is 160 mm Hg (1 atm = 760 atm). How many moles of oxygen are in the typical human lung when full? (You can assume the air in the lungs is at a normal human body temperature of 37oC.)

A 1.25 g sample of an unknown gas at 47 ∘C and 1.00 atm is stored in a 2.55 L flask. What is the density of the gas? density:   g/L   What is the molar mass of the gas? molar mass:   g/mol

A mixture of nitrogen and xenon gases, in a 5.99 L flask at 50 °C, contains 2.90 grams of nitrogen and 43.1 grams of xenon. The partial pressure of xenon in the flask is atm and the total pressure in the flask is atm.