2. A sample of molecular nitrogen gas, N2, occupies 3.0 L at a pressure of 3.0 atm. What volume will it occupy when the pressure is changed to 0.50 atm and the temperature remains constant?

A sample of xenon gas occupies a volume of 7.22 L at 52.0°C and 0.710 atm. If it is desired to increase the volume of the gas sample to 8.89 L, while increasing its pressure to 0.963 atm, the temperature of the gas sample at the new volume and pressure must be °C.

A gas which is very important when considering the environmental impacts of pollution is sulfur dioxide (SO2). Consider a sample of SO2 with volume 4.24 L at a pressure of 4.5 atm. If the pressure is changed to 4 atm, what will be the final volume of the gas (in mL)? Assume temperature stays constant

A 17.017.0 L sample of ideal gas has a pressure of 25.025.0 atm at a certain temperature. At the same temperature, what volume would this gas occupy at a pressure of 9.309.30 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

45.0 L of an ideal gas at 288 K and 3.50 atm are heated to 373 K with a new pressure of 8.20 atm. What is the new volume (in L)?

A sample of krypton gas has a volume of 5.78 L and a pressure of 2.92 atm, under a constant temperature of 300 K. What is the new volume, if the pressure is decreased to 1.75 atm?

A sample of nitrogen gas occupies 9.20 L at 0.595 atm. If the pressure is increased to 2.15 atm at constant temperature, what is the newly occupied volume?

3. A certain mass of magnesium is reacted with 6M HCl. The hydrogen gas liberated is collected by displacing 200 mL of water. The pressure of the gas and the atmospheric pressure are equalized. The atmospheric pressure is 762 mmHg. The temperature of the experiment is 27°C. How many moles of hydrogen have been liberated, and what is the mass of the magnesium that reacted?

A certain mass of nitrogen gas occupies a volume of 6.63 L6.63 L at a pressure of 6.08 atm.6.08 atm. At what pressure will the volume of this sample be 9.01 L?9.01 L? Assume constant temperature and ideal behavior.