1. States of Matter I: Gases
S.L.O 4.1: Kinetic Molecular Theory of Gases S.L.O 4.2 Absolute Temperature Scale on the Basis of Charles’s Law

2. 4.1.1 list down the postulate of kinetic molecular theory (KMT) of gases; *
The particles are so small compared to the distances between them that their volume may be ignored
The particles are in constant motion
The particles exert no forces on each other (i.e., no attractive or repulsive, bu they still bang into each other)
The kinetic energy of the collection of particles is assumed to be directly proportional to the K temperature for the gas
A gas is composed of a large number of particles called molecules 
Gas molecules collide with one another and with the walls of the container, but these collisions are perfectly elastic; that is, they do not change the average kinetic energy of the molecules.

3. 4.1.2 state and explain the gas laws (Boyle’s, Charles’s, Avogadro’s, Dalton’s law of partial pressure and Graham’s law of diffusion/effusion);
BOYLE’S LAW:For a fixed amount of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional. Or Boyle's law is a gas law, stating that the pressure and volume of a gas have an inverse relationship, when temperature is held constant.
CHARLE’S LAW: It states that, for a given mass of an ideal gas at constant pressure, the volume is directly proportional to its absolute temperature, assuming in a closed system.
AVAGADRO’S LAW: states that, "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules".
DALTON’S LAW OF PARTIAL PRESSURE: states that in a mixture of non-reacting gases, the total pressureexerted is equal to the sum of the partial pressuresof the individual gases.
GRAHAM’S LAW OF DIFFUSION/EFFUSION:Graham's law states that the rate of diffusion or of effusion of a gas is inversely proportional to the square root of its molecular weight.

4. 4.2.1 explain absolute zero on the basis of Charles’s law;U
Charles law states that at constant pressure, a given quantity of gas will have a volume proportional to the absolute temperature.
Charles law explain the relation betwee absolute zero and volume of a gas.
According to charles law volume of a gas increases or decreases with every k increase or decrease in temperature.

5. 4.2.2 convert temperature into different scales; A
From
To Fahrenheit
To Celsius
To Kelvin
Fahrenheit (F) F
(F - 32) * 5/9
(F - 32) * 5/
Celsius (C or o)
(C * 9/5) + 32 C C
Kelvin (K)
(K ) * 9/5 + 32 K K