An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly eleastic and in which there are no intermolecular attractive forces. One can visualize it as a collection of perfectly hard spheres which collide but which otherwise do not interact with each other. In such a gas, all the internal energy is in the form of kinetic energy and any change in internal energy is accompanied by a change in temperature. An ideal gas can be characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them may be deduced from kinetic theory and is called the -Ideal Gas Law. (n.d.). Retrieved April 24, 2017, from http://hyperphysics.phy-astr.gsu.edu/hbase/Kinetic/idegas.html
This law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature. P is proportional to T ..., a constant can be put in: P / T = C As the pressure goes up, the temperature also goes up, and vice-versa. Also ..., initial and final volumes and temperatures under constant pressure can be calculated. -Jircitano, A. J. (n.d.). Gas Laws. Retrieved April 24, 2017, from http://chemistry.bd.psu.edu/jircitano/gases.html
In the mid 1600's, Robert Boyle studied the relationship between the pressure p and the volume V of a confined gas held at a constant temperature. Boyle observed that the product of the pressure and volume are observed to be nearly constant. The product of pressure and volume is exactly a constant for an ideal gas. p * V = constant -Boyle's Law. (n.d.). Retrieved April 24, 2017, from https://www.grc.nasa.gov/www/k-12/airplane/boyle.html
"At a fixed pressure, the volume of a gas is proportional to the temperature of the gas." - Elementary Gas Laws: Charles Law. (n.d.). Retrieved April 24, 2017, from http://www.iun.edu/~cpanhd/C101webnotes/gases/charleslaw.html