What volume will a sample of nitrogen occupy at STP (standard temperature and pressure) if it occupies a volume of 650. mL at 82.00 oC and 420. mmHg of pressure? (Hint: first solve for moles in PV=nRT. Then, using PV=nRT again, solve for volume using calculated moles and STP values.)

Molar mass ?

What would be the volume of 3.90 moles of an ideal gas, at STP?  What is the pressure of this gas, if the temperature was increased from 0 degC to 53.5 degC as it stays in a constant volume container?

2. Calculate the pressure of a sample of gas collected over water at 25°C if the atmospheric pressure is 0.948 atm. 1 atm = 760 mm Hg.

A sample of hydrogen gas occupies a volume of 9.21 L at 51.0°C and 0.780 atm. If it is desired to decrease the volume of the gas sample to 7.91 L, while decreasing its pressure to 0.566 atm, the temperature of the gas sample at the new volume and pressure must be °C.

A sample of hydrogen gas has a volume of 6.04 L at 47°C and 1.32 atm. What would be the volume of this gas sample at STP? (STP (standard temperature and pressure) is used as a reference point for the molar volume of an ideal gas. In the USA, most chemists, most general chemistry texts, and OWL use STP = 0°C, 1 bar, where the molar volume = 22.7 L/mol.) Volume =  L

If a sample of Xenon gas occupies a volume of 31.0L at 17.0°C, at what temperature, in °C, will it occupy a volume of 7.0L if the pressure remains constant? (Hint: Convert ° to K)

4. In a laparoscopic surgery, carbon dioxide gas is used to inflate the abdomen to separate the internal organs and the abdominal wall. If the CO2 injected into the abdomen produces a pressure of 17 mmHg and a volume of 2.9 L at 26°C, how many moles of CO2 were used? How many grams? 5. What is the total pressure, in millimeters of mercury, of a gas mixture containing krypton gas at 0.45 atm and neon gas at 650 mmHg?

4. A glass container was initially charged with 2.00 moles of a gas sample at 3.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 28.1 °C, so the final pressure in the container was reduced to 0.998 atm. Assume the volume stayed the same. How many moles of the gas sample are present at the end?

What is the final temperature of a gas (in °C) that starts at a pressure of (4.51x10^2) mm Hg, a volume of (8.400x10^0) L, and a temperature of (3.270x10^1)°C and is changed to a pressure of (7.3000x10^2) mm Hg and a volume of (6.9000x10^0) L?