Lesson 12: Gas Laws

BOYLE'S LAW

The inverse relationship between pressure and volume. It states that the volume of a sample of gas changes inversely with the pressure of the gas as long as the temperature and the amount of the gas remain constant. When the pressure of the gas decreases, the volume of the gas increases. When the pressure of a gas increases, the volume of the gas decreases.

Boyle’s Law Definition 2

In 1662 Robert Boyle studied the relationship between volume and pressure of a gas of

fixed amount at constant temperature. Boyle's law was published in the same year.

Charle’s Law

or the relationship between volume and temperature, was found in 1787 by Jacques Charles, a French physicist and balloonist. The statement of Charles's law is : the volume (V) of a given mass of a gas, at constant pressure (P), is directly proportional to its temperature (T).

Gay-Lussac's law, Amontons' law

or the pressure law was found by Joseph Louis Gay-Lussac in 1808. Temperature and pressure relationship. It states that the pressure of a gas is directly related to its Kelvin temperature.

Avogadro's law

(hypothesized in 1811) states that the volume occupied by an ideal gas is directly proportional to the number of molecules of the gas present in the container. This gives rise to the molar volume of a gas, which at STP (273.15 K, 1 atm) is about 22.4 L.

The Combined

gas law or General Gas Equation is obtained by combining Boyle's Law, Charles's law, and Gay-Lussac's Law. It shows the relationship between the pressure, volume, and temperature for a fixed mass (quantity) of gas.

IDEAL GAS LAW

The law that describes the pressure, volume, temperature, and number of moles of a gas. Avogadro's law and the combined gas law develops into the ideal gas law

The ideal gas equation was first stated by Benoît Paul Émile Clapeyron in?

1834 as a combination of Boyle's law, Charles's law. Avogadro's law, and Gay-Lussac's law. Clapeyron was a French engineer, and one of the founders of thermodynamics.

What are the Ideal Gas Number of paricles constantly coliding with each

other randomly. In order to model and predict the behavior of gases, the

concept of an ideal gas was thus created. If a gas is ideal, then a few

assumptions need to be made. These can also be viewed as the ideal gas

properties.

1.Firstly, we assume that the volume of the gas particles is negligible. This

means that the volume of the container is much larger than the volume of

the gas particles.

2. Secondly, we assume that the gas particles have equal size, and do not

have intermolecular forces with other gas particles.

3. Thirdly, we assume that the gas particles move randomly according to

Newton's Laws of Motion.

4.Lastly, we assume that all collisions are perfectly elastic and have no

energy loss. This means that the collisions between gas particles and the

walls don't lose energy, and exert constant pressure.

Although no gas is perfectly ideal most gases are close enough at room

temperature and are nearly ideal.