Final answer:
Boyle's Law states that the volume of a gas is inversely proportional to pressure at constant temperature. Charles's Law explains that the volume of a gas is directly proportional to its absolute temperature at constant pressure. Dalton's Law of Partial Pressure indicates that the total pressure of a gas mixture is the sum of the individual gases' partial pressures.
Step-by-step explanation:
(a) Boyle's Law states that at a constant temperature, the volume of a certain quantity of a gas is inversely proportional to its pressure. This is explained by kinetic theory as the gas molecules are in constant motion and if the volume decreases, the gas molecules have less space to move, resulting in more frequent collisions and thereby, increased pressure.
(b) Charles's Law says that at constant pressure, the volume of a given amount of gas is directly proportional to its absolute temperature. From the kinetic perspective, as the temperature rises, the kinetic energy of gas molecules increase, they move faster and hit the walls of the container more frequently and with more force, thus the volume increases.
(c) Dalton's Law of Partial Pressure states that the total pressure of a mixture of gases is the sum of the partial pressures of individual gases in the mix. According to kinetic theory, each gas in a mixture acts independently of the others and all the gases contribute to the total pressure by virtue of their own individual particle collisions with the container walls.
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