Don’t Make the Mistake Of Not Knowing Boyle’s Law For the CSET

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Gas Laws and Basic Atmospheric Forces

The density (the mass of a unit of volume) of air is about 1.225 kg/m³ at mean sea level [msl] and decreases with altitude. The molecular activity exerts a force in all directions measured in terms of pressure. This activity, the internal kinetic energy, is proportional to the absolute temperature. (Absolute temperature is expressed in Kelvin units [K]. One K equals one °C and zero degrees in the Celsius scale is equivalent to 273 K). There are several gas laws and equations which relate temperature, pressure, density and volume of a gas.

Air is a gas. Gases have various properties which we can observe with our senses, including the gas pressure (p), temperature, mass, and the volume (V) which contains the gas. Careful, scientific observation has determined that these variables are related to one another, and the values of these properties determine the state of the gas.

In the mid 1600’s, Robert Boyle studied the relationship between the pressure p and the volume V of a confined gas held at a constant temperature. Boyle observed that the product of the pressure and volume are observed to be nearly constant. The product of pressure and volume is exactly a constant for an ideal gas.

In the video above, you will see an animation of the relationship between p (gas pressure), mass, and the volume (v).

Boyle’s Law Defined

Temperature is constant
Volume occupied by a gas varies inversely with the applied pressure
Equation: P1V1 = P2V2
Boyle’s Law has constant temperature
Inverse Relationship
If p goes up, then V goes down
If p goes down, then V goes up
Pressure = 1/volume
Pressure is inversely proportional to volume.

Example

If the original pressure of a gas is 1 atm with a volume of 40 mL, what is the new volume when the pressure is increased to 2 atm?

P1 = 1 atm
V1 = 40 mL
P2 = 2 atm
V2 = ?????

P1V1 / P2 = V2

(1 atm)(40 mL) / (2 atm) = 20 mL

V2 = 20 mL

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