what is the relationship between the pressure of a gas and the absolute temperature when the volume is kept constant ?
The pressure of a gas is directly proportional to the absolute temperature of the gas.
THANK YOU ! ( :
The relationship between the pressure of a gas and the absolute temperature when the volume is kept constant is described by Gay-Lussac's Law, also known as the pressure-temperature law. According to this law, the pressure of a gas is directly proportional to its absolute temperature when the volume remains constant.
Mathematically, Gay-Lussac's Law can be expressed as:
P1/T1 = P2/T2
Where:
P1 and P2 are the initial and final pressures respectively,
T1 and T2 are the initial and final temperatures respectively.
To understand this relationship, let's consider an example. Imagine you have a gas confined in a container with a fixed volume. If the temperature of the gas increases while the volume remains constant, according to Gay-Lussac's Law, the pressure of the gas will also increase proportionally. Similarly, if the temperature decreases, the pressure will decrease.
This relationship can be explained by the behavior of gas molecules. As temperature increases, the kinetic energy of the gas molecules increases. With higher kinetic energy, the gas molecules collide more frequently and with greater force against the walls of the container, resulting in an increase in pressure.
Conversely, if the temperature decreases, the gas molecules have lower kinetic energy, resulting in fewer and weaker collisions with the container walls, leading to a decrease in pressure.
In summary, when the volume of a gas is kept constant, the pressure of the gas and its absolute temperature have a direct, proportional relationship, as described by Gay-Lussac's Law.