Two students use hot plates to boil water in open bottles. The bottles are ident

Question

 Two students use hot plates to boil water in open bottles.  The bottles are identical but Bottle 1 is one-third full of liquid while Bottle 2 is two-thirds full.  Bottle 1 is in a lab room on campus (T = 20oC) and Bottle 2 is in a walk-in refrigerated room at the dining commons (T = 1oC).  The pressure in each room is 1 atm.

Each bottle is boiled vigorously for several minutes.  Assume that in this process, water vapor pushes all air out of the bottles (i.e., only water vapor particles remain in the space above the liquid). The bottles are then removed from the hot plates and immediately sealed with tight-fitting lids.

A long time after the bottles are sealed, when the contents have reached equilibrium, is the pressure inside Bottle 1 greater than, less than, or equal to the pressure inside Bottle 2?  Explain.

At equilibrium, what is the pressure in each bottle?

Explanation / Answer

Bottle 1 will likely have greater pressure than bottle 2, after equilibrium is reached the rate of cooling of water
will be faster in bottle 2 which means that the vapor condenses into liquid quickly creating less pressure inside
Where as in bottle 1 it is opposite, since it is at 20oC. Therefore pressure inside bottle 1 will be greater

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