A 3.00-L bulb containing neon gas at 3.85 atm is connected to an evacuated 5.00-L flask. The valve connecting the flasks is opened, and the pressure is.

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Presentation transcript:

A 3.00-L bulb containing neon gas at 3.85 atm is connected to an evacuated 5.00-L flask. The valve connecting the flasks is opened, and the pressure is allowed to equilibrate. If the temperature remains constant, what is the final pressure in the system?

How many molecules are present in a sample of hydrogen gas having a volume of 8.56L at 0ºC and 1.5 atm Pressure?

What volume of Oxygen is needed to fully oxidize (rust) our measured block from Richard Serra ’ s 4-5-6? (We will assume the block is solid iron and measures 48 X 60 X 71 inches)

At 1.50 atm pressure and 27ºC, a gas is found to have a density of 1.95g/L. What is the molar mass of the gas?

The atmospheric pressure is 743 mm Hg. If the partial pressure of oxygen is 156 Torr, what is the mol fraction of oxygen in air?

A mixture of 1.00 gram of H 2 and 1.00 gram of He is placed in a 1.00L container at 27˚C. What is the total pressure of the gas?

A sample of nitrogen is present in a container with liquid water present. The sample has a total pressure of 763 mmHg at 27°C. The vapor pressure of water at 27°C is 26.7 mmHg. What is the density of the gas mixture?

A mixture of CH4(g) at atm and O2(g) at atm is present in a 3.00-L container at 28°C. The mixture is ignited by a spark and reacts according to the equation below. What is the total pressure in the container, now at 44°C, after the reaction is complete? The vapor pressure of water at 44°C is mmHg.

A gaseous mixture consists of 50.0% O 2, 25.0% N 2, and 25.0% Cl 2, by weight. At standard temperature and pressure, What is the partial pressure of Cl 2 ?