An ideal gas is contained in a cylinder with a pressure of 1429 torr at a temperature of 12.0 C and a volume of 0.370L. The gas is then heated, and the volume is measured to be 1.84 L at a pressure found too be 0.50 atm. What was the final temperature of the gas in C?

What temperature (in °C) did an ideal gas shift to if it was initially at -20.5 °C at 4.62 atm and 35.0 L and the pressure was changed to 2.50 atm and the volume changed to 50.0 L?

A sample of hydrogen gas at a pressure of 1.18 atm and a temperature of 267 °C, occupies a volume of 612 mL. If the gas is heated at constant pressure until its volume is 737 mL, the temperature of the gas sample will be   ____°C.   (Explain well with proper step  by step Answer. ).

The atmospehere in a sealed diving bel contained oxygen and helium. If the gas mixture has 0.200 atm of oxygen and a total pressure of 3.00 atm, calcuate the mass of helium in 1.00 L of the gas mixture at 25.0 C.

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)?

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 temperature (in °C) did an ideal gas shift to if it was initially at -22.00 °C at 4.620 atm and 35.00 L and the pressure was changed to 8.710 atm and the volume changed to 15.00 L?

A certain mass of nitrogen gas occupies a volume of 1.33 L at a pressure of 3.01 atm. At what pressure will the volume of this sample be 3.71 L? Assume constant temperature and ideal behavior.----atm?