what is the relationship between the pressure of a gas and the absolute temperature when the volume is kept constant ?
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When the volume of a gas is kept constant, a relationship called Boyle's Law states that the pressure of the gas is inversely proportional to its absolute temperature. This means that as the temperature increases, the pressure of the gas will also increase, and vice versa.
To understand why this relationship exists, we can look at the kinetic theory of gases. According to this theory, gas molecules are in constant motion and collide with each other and the walls of the container they are in. The pressure exerted by a gas is a result of these molecular collisions.
As the temperature of the gas increases, the average kinetic energy of the gas molecules also increases. This leads to more frequent and energetic collisions between the gas molecules and the container walls, resulting in an increase in pressure. Conversely, when the temperature decreases, the average kinetic energy decreases, causing fewer and less energetic collisions and a decrease in pressure.
To mathematically express this relationship, we can use the equation:
P₁/T₁ = P₂/T₂
Where P₁ and P₂ are the initial and final pressures, and T₁ and T₂ are the initial and final absolute temperatures, respectively. This equation shows the inverse relationship between pressure and temperature when volume is held constant.
To experimentally determine this relationship, you can perform a laboratory experiment where you measure the pressure of a gas at different temperatures while keeping the volume constant. By plotting the data and analyzing the trend, you can observe the direct relationship between pressure and absolute temperature.