glass container was containing 1.50 moles of a gas sample at 5.00 atm and 21.7 °C was heated to 33.1°C. During the heating some gas escapes its container

If 3.23 g Ar are added to 4.22 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of the resulting gaseous mixture? Ptotal = atm

A glass container was initially charged with 2.35 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. How many moles of the gas sample are present at the end?

If 1.52 g Ar are added to 3.41 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of the resulting gaseous mixture? Ptotal = atm

A glass container was initially charged with 2.40 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. How many moles of the gas sample are present at the end?

An ideal gas in a sealed container has an initial volume of 2.65 L. At constant pressure, it is cooled to 24.00 'C, where its final volume is 1.75 L. What was the initial temperature? °C T =

You have a 3.00-liter container filled with N₂ at 25 °C and 3.35 atm pressure connected to a 2.00-liter container filled with Ar at 25 °C and 2.75 atm pressure. A stopcock connecting the containers is opened and the gases are allowed to equilibrate between the two containers. What is the final pressure (in atm) in the two containers if the temperature remains at 25 °C? Assume ideal behavior.

Container A holds 752 mL of ideal gas at 2.30 atm. Container B holds 124mL of ideal gas at 4.70 atm. If the gases are allowed to mix together, what is the partial pressure of each gas in the total volume?

Container A holds 757 mL of an ideal gas at 2.10 atm. Container B holds 114 mL of a different ideal gas at 4.30 atm.  If the gases are allowed to mix together, what is the resulting pressure?

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?