The problem states: Two small containers of equal volume, 100 cm^3, each contain helium gas at 0 degrees C and 1.00 atm pressure. The two containers are joined by a small open tube of negligible volume, allowing gas to flow from one container to the other. What common pressure will exist in the two containers if the temperature of one container is raised to 100 degrees C while the other is kept at 0 degrees C.
I know I should use PV=nRT but I am having trouble with how to set the pressures equal.
The Attempt at a Solution
I used n=PV/RT to find the number of moles of Helium gas in each container = 4.4646*10^-6 mol He
I then tried to use: n1T1=n2T2 to find the number of moles of He on the side of the container that was heated to 100 degrees C, but am stuck here.
*Would the pressure rise the same amount if both sides of the container were heated to 50 degrees C?