>>11688069This thread is full of retards.
Ideally, lets assume that the system is perfectly sealed and the the outside of containers 2 and 3 are under 100 degrees C and that container 1 is 150 degrees C. In this ideal scenario, eventually all the water in cup 1 will have evaporated and condensed into cups 2 and 3 equally.
The water vapor will be pulled from cup 1 into 2 and 3 evenly, as a gas will evenly expand to fill its container. As the gas condenses, it will result in a drop of vapor pressure in cups 2 and 3 and assuming they are identical in design and environment, this will happen equally. This will cause more vapor from cup 1 to move in.
Using this principle, we simply have to calculate how much energy a 150 degree C flame will give off in 1 hour, assuming there is no loss of energy during conduction (again, ideal). Using calorimetry , we can then calculate how much water will evaporate in 1 hour. Ideally, about half of this volume will be in cup 2 and half in cup 3. Some will remain in the gas phase, so it will be a little less.
DESU if you really care about the specifics it would probably be easier to just run the experiment 10 times and compile the data.
