Final answer:
Boyle's Law states that at a constant temperature, the pressure of an ideal gas is inversely proportional to its volume. Charles' Law states that at a constant pressure, the volume of an ideal gas is directly proportional to its absolute temperature. Both laws provide an approximation of the behavior of real-world gases.
Step-by-step explanation:
(a) Boyle's Law states that at constant temperature, the pressure of an ideal gas is inversely proportional to its volume. This means that if the volume of the gas is halved, the pressure is doubled. This relationship is represented by the formula P1V1=P2V2.
(b) Charles' Law states that at constant pressure, the volume of an ideal gas is directly proportional to its absolute temperature. In other words, if the temperature increases, the volume of the gas also increases. This relationship is represented by the formula V1/T1=V1/T2.
In both laws, one variable can be altered while the other remains constant, demonstrating the relationship between pressure, volume, and temperature in an ideal gas. In reality, gases are not 'ideal', but these laws provide a close approximation of their real-world behavior.
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