Suppose you have one container of nitrogen gas (molar mass: 28.0 g/mol) and one container of helium gas (molar mass: 4.00 g/mol). They are separated from each other by a valve that keeps them both from mixing (until
the valve is opened and they mix). Both containers are at 400.0 K. The container of nitrogen Aas is at 400.0 K, and so is the container of helium
gas.
The nitrogen gas container has a pressure of 5.00 atm and a volume of 2.00 L, and the helium gas container has a pressure of 9.00 atm and a
volume of 3.00 L. There are 0.305
mol of nitrogen and 0.823 mol of helium. After the valve is opened, the gases mix and each gas fills the volume of
both containers. What is the partial pressure of the helium gas after this gas mixing? You can assume that the temperature after the mixing is also
400.0 K
Less than 2.00 atm.
Between 2.00 atm and 4.00 atm.
Between 4.00 atm and 6.00 atm.
Between 6.00 atm and 8.00 atm.
More than 8.00 atm.