At constant pressure, the volume of a given mass of an ideal gas is directly proportional to its absolute temperature.
This means that if you increase the temperature of a gas while keeping the pressure constant, the volume will also increase proportionally.
Here's a simple explanation:
* Temperature is a measure of the average kinetic energy of the gas molecules.
* Volume is the space occupied by the gas molecules.
* As the temperature increases, the molecules move faster and collide more frequently with the container walls.
* This increased collision pressure pushes the container walls outwards, resulting in an increase in volume.
Mathematically, Charles's Law can be expressed as:
V₁/T₁ = V₂/T₂
Where:
* V₁ = Initial volume
* T₁ = Initial absolute temperature (in Kelvin)
* V₂ = Final volume
* T₂ = Final absolute temperature (in Kelvin)
Important Note:
* Charles's Law applies to ideal gases, which are theoretical gases that behave perfectly according to the gas laws.
* Real gases deviate from ideal behavior at high pressures and low temperatures.
* To use Charles's Law, you need to express the temperature in Kelvin, not Celsius.
Example:
If a balloon with a volume of 1 liter at 20°C (293 K) is heated to 40°C (313 K), its volume will increase to:
V₂ = V₁ * T₂ / T₁
V₂ = 1 L * 313 K / 293 K
V₂ ≈ 1.07 L
The volume increases by approximately 7% as the temperature increases by 20°C.
