the temperature of gas is proportional to the
volume
title: Charles's law text: Charles's law Charles's law (also known as the law of volumes) is an experimental gas law that describes how gases tend to expand when heated. A modern statement of Charles's law is: When the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be in direct proportion. This directly proportional relationship can be written as: or where: This law describes how a gas expands as the temperature increases; conversely, a decrease in temperature will lead to a decrease in volume. For comparing the same substance under two different sets of conditions, title: Gas text: pressure and temperature, density is a state variable of a gas and the change in density during any process is governed by the laws of thermodynamics. For a static gas, the density is the same throughout the entire container. Density is therefore a scalar quantity. It can be shown by kinetic theory that the density is "inversely" proportional to the size of the container in which a fixed mass of gas is confined. In this case of a fixed mass, the density decreases as the volume increases. If one could observe a gas under a powerful microscope, one would see title: Boyle's law text: air moves from high to low pressure. Related phenomena: Other gas laws: Boyle's law Boyle's law, sometimes referred to as the Boyle–Mariotte law, or Mariotte's law (especially in France), is an experimental gas law that describes how the pressure of a gas tends to increase as the volume of the container decreases. A modern statement of Boyle's law is The absolute pressure exerted by a given mass of an ideal gas is inversely proportional to the volume it occupies if the temperature and amount of gas remain unchanged within a closed system. Mathematically, Boyle's law can be stated as or title: Gay-Lussac's law text: Stanislao Cannizzaro was able to convince the First International Chemical Congress in 1860. This law is often referred to as Gay-Lussac's law of pressure–temperature, between 1800 and 1802, discovered the relationship between the pressure and temperature of a fixed mass of gas kept at a constant volume. Gay Lussac discovered this while building an "air thermometer". The pressure of a gas of fixed mass and fixed volume is directly proportional to the gas's absolute temperature. If a gas's temperature increases, then so does its pressure if the mass and volume of the gas are held constant. The law has a title: Temperature text: other systems, vibrational and rotational motions also contribute degrees of freedom. Maxwell and Boltzmann developed a kinetic theory that yields a fundamental understanding of temperature in gases. This theory also explains the ideal gas law and the observed heat capacity of monatomic (or 'noble') gases. The ideal gas law is based on observed empirical relationships between pressure ("p"), volume ("V"), and temperature ("T"), and was recognized long before the kinetic theory of gases was developed (see Boyle's and Charles's laws). The ideal gas law states: where "n" is the number of moles of gas and is the gas constant. This