Final answer:
The relationship between temperature and pressure in a gas, described by Gay-Lussac's Law, shows that pressure and temperature are directly proportional when volume and moles of gas remain constant. Temperature measurements must be in Kelvin to apply this law, as it correctly reflects the linear relationship. This is fundamental in understanding gas behavior as per the kinetic molecular theory.
Step-by-step explanation:
Understanding the Relationship between Temperature and Pressure in Gases
The relationship between temperature and pressure in gases is a fundamental concept in thermodynamics and physical science. When a gas is confined to a constant volume, experimental data typically show that temperature and pressure have a linear relationship. This relationship is described by Gay-Lussac's Law, which states that the pressure of a given mass of gas varies directly with the absolute temperature when the volume is kept constant.
When describing the behavior of gases, it is essential to use the Kelvin scale for temperature measurements because it is an absolute scale where 0 Kelvin represents the absence of thermal energy. According to Gay-Lussac's Law, if the temperature measured in Kelvin is doubled, the pressure of the gas will also double, provided the volume and the amount of gas in moles remain unchanged. This proportional relationship is crucial for understanding how gases respond to changes in temperature within a closed system.
The intertwined nature of pressure, volume, and temperature with regards to gas behavior can be visualized and summarized through experimental illustrations such as figure 11.3.5, which shows the relative changes in these properties. These relationships are central to kinetic molecular theory, which provides a theoretical model to explain and predict the experimental behavior of gases.