Boyle's law is about the relationship between pressure and volume if
temperature and the amount of molecules are held constant.
The volume of a fixed mass of gas is inversely proportional to the
pressure at a constant temperature.
The relation can also be written as pressure times volume equals
An increasing container volume decreases the pressure.
A decreasing container volume increases the pressure.
At constant temperature
P1V1 = P2V2
When the volume of a container decreases, the distance between
the gas molecules shrink. As a result of this
they bump into each other more often than if they where farther
apart. The increased molecular movements push at the walls
inside the container and increases the pressure.
Example: A balloon with a volume of 1000.0 L (V2) is filled
with a gas at 1 atmospheres (P2).
If the pressure is reduced to 0.319
(altitude 8000m) without a change in temperature ( T1 , T2 = 300
Kelvin ), what
would be the new volume of the balloon?
Answer ( image below ): 3134 L
Chemistry Software - Home