1. by Jossie Kosasih
2. Properties of Gases
2.1. Kinetic Molecular Theory
2.1.1. gases are compressible
2.1.1.1. The volume of a gas decreases when pressure is exerted on the gas. The molecules are pushed closer together, leaving the volume of the gas to consist of empty space.
2.1.2. gas pressure
2.1.2.1. Pressure is the result of gas molecules colliding with objects, particularly the walls of a container. Pressure from a gas is the total force of collisions distributed over the area it collides with (force per unit area)
2.1.3. Boyle's law
2.1.3.1. If the volume is reduced, gas molecules will move a shorter distance before colliding with the walls of the container.
2.1.4. Charles' Law
2.1.4.1. As the temperature of a gas increases, the molecules move about faster (meaning an increase in average kinetic energy). They will spread out to occupy more space
2.2. Explanation
2.2.1. The kinetic molecular theory provides a good explanation of gas pressure, temperature and the gas laws for an ideal gas
3. Ideal gas law
3.1. a combination of Boyle's law, Charles' law, and Avogadro's theory
3.2. describes the interrelation of pressure, temperature, volume, and chemical amount of matter of gases
3.2.1. According to Boyle's law, the volume of a gas is inversely proportional to the pressure: V ∝ 1/P
3.2.2. According to Charles' law, the volume of a gas is directly proportional to the absolute temperature: V ∝ T
3.2.3. According to Avogadro's theory, the volume of a gas is proportional to the chemical amount of matter: V ∝ n
3.3. Combining these three statements produces: V ∝ 1/P x T x n
3.4. PV = nRT - ideal gas law formula
3.4.1. V = (a constant, R) x 1/P x T x n V = nRT/P
3.4.2. R = PV/nT
4. Ideal Gases
4.1. a hypothetical gas that obeys all gas laws perfectly under all conditions of temperature, pressure and volume.
4.2. does not condense into a liquid when cooled and graphs of its volume and temperature and of pressure and temperature are in perfect straight lines.
4.3. molecules
4.3.1. very far apart compared to their size and are in constant, random, straight line motion because no forces exist between them
4.3.2. Molecules also undergo elastic collisions, meaning no energy would be lost (hard molecules).