Etiket Arşivleri: Charles’ Law

Charles’ Law

Charles’ Law

The Temperature-Volume Relationship

Charles’ Law

French chemist Jacques Charles discovered that the volume of a gas at constant pressure changes with temperature.

As the temperature of the gas increases, so does its volume, and as its temperature decreases, so does its volume.

C h a r l e s ’  L a w

The law says that at constant pressure, the volume of a fixed number of particles of gas is directly proportional to the absolute (Kelvin) temperature, mathematically expressed as:

V = kT

Charles’ Law

V = kT

  V = Volume

  k = Charles’ Law constant   of Proportionality

  T = Temperature in Kelvins


Raising the temperature of a gas causes the gas to fill a greater volume as long as pressure remains constant.

Gases expand at a constant rate as temperature increases, and the rate of expansion is similar for all gases.


If the temperature of a given amount of gas is doubled, for example, its volume will also double (as long as pressure remains unchanged).

2V = 2kT

Charles’ Law

Charles’ Law can be modified to a convenient form by solving for k.

k = V / T

Charles’ Law

In a sample with volume V1 & temperature T1, changing either volume or temperature converts these variables to V2 and T2.

V1 / T1 = k = V2 / T2


V1 T2 = V2 T1

Demonstration of Charles’ Law

Relationship of Boyle’s Law and Charles’ Law

Practical Applications

Charles’ Law ( Raymond GREENLAW )

Charles’ Law

—By Raymond Greenlaw

—Learning Objectives

—State Charles’ Law

—Understand Charles’ Law

—Apply Charles’ Law

—Explain relevance of Charles’ Law to scuba

—Jacques Charles/Joseph Louis Guy-Lussac

—Ballooner and scientist


—Did not publish, sometimes called Charles/Guy-Lussac’s  Law after Joseph Louis Guy-Lussac

—Temperature Scales

—State Charles’ Law

—For any gas at a constant pressure, the volume of the gas is directly proportional to its absolute temperature.

—State Charles’ Law


V1/T1 = V2/T2, where Vi is volume and Ti is temperature in Kelvin

—V/T = k, where k is a constant

—Recall 0K = -273C and oK = -460F

—Note, pressure remains the same

—Charles’ Law Illustrated

—Understand Charles’ Law

—Temperature goes up volume goes up

—Temperature goes down volume goes down

—Rubber glove thought experiment

—Gas molecules thought experiment

—Balloon in the morning thought experiment


—2 liters of gas at 273C

—1 liter of gas at oC

—Since V1/T1 = V2/T2, we have 2/546 = 1/273

—Note, we converted temperatures to Kelvin by adding 273 as required by Charles’ Law.

—If we cool by 273C, we reduce volume by 1 liter.

—If we heat by 273, we increase volume by 1 liter.

—Apply Charles’ Law

—Not fully (XL) BCD contains .3 liters of air on a cool morning at oC

—BCD is left in a car and the temperature sores to 40C

—What is the new volume of air in the BCD, assuming it is still not totally full?

—Apply Charles’ Law (We assume no change in pressure.)

—We know intuitively that the volume goes up.

—.3/273 = x/313, so x = .34 liters

—Explain Relevance of Charles’ Law to Scuba

—We learned that as temperature increases volume increases.

—Consider a full cylinder of air.

—When heated the volume wants to increase by Charles’ Law, but in a tank there is no room for expansion, so the pressure must increase.

—Extreme temperature increases could result in a tank bursting.

—Do not leave full scuba tanks stored in direct sunlight or heat them.

—Getting Bent

—We know nitrogen dissolves in a diver’s body tissues under pressure.

—Suppose a diver goes deep and a lot of nitrogen dissolves in body tissues.

—As the diver surfaces, the diver is not bent.

—However, exposure to intense sunlight could cause gas coming out of solution to increase in volume (temperature goes up volume increases), so the diver could get bent.


—What happens if we fill tanks on a hot afternoon and dive the next day on a very cold morning?


—Naui Master Scuba Diver Manual, 2010.




—Figures borrowed from around the web, please let me know if any of the figures are not in the public domain and I will replace them.


—Thanks for coming!