How does temperature affect vapor pressure?
Answer:
Directly related.
Its directly proportional, Greater the temp greater is the VP
Even though it is not as linear for all vapors, here is a formula;
pressureXvolume= mass *gas constant *temperature.
This has been verified by experimental confirmations for centuries.
As the temperature goes up, something must go up on the other side to keep it equal. If the volume is fixed the only way to compensate is the pressure.
directly proportional
when the temp increases, pressure increses too
Consider the space under the lid of a jar of canned tomatoes. There is no air and only water vapor pressure, which being far less than atmospheric pressure at room temperature preserves a partial vacuum. Water molecules are constantly gaining enough excess energy by collisions (like billiard balls) to leave the water surface but a similar number of molecules must re-enter the water to keep absolute pressure constant for the average temperature of the water and vapor. As the temperature of the jar is increased, all water and vapor molecules possess greater average energy and the vapor molecules press a little harder on the lid (slightly decreasing the partial vacuum). At 212F the water is about to boil and the vapor molecules collectively exert the same pressure on the lid as the atmospheric pressure does on the other side and you can easily remove the lid. The same temperature/pressure relationship holds true for the water vapor in an air-filled room but actual pressure will not increase if the room leaks air. Relative humidity will increase from zero (dry) to 100 % as the vapor pressure increases from nil to the maximum that the air can hold without condensation.
vapor pressure increases as temperature increase because they are directly proportional.
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