Ideal Gas Laws

Gases can be described in terms of its temperature (T), the pressure (P) it exerts, the volume (V) it occupies, and the amount of substance there is (n). Ideal gases are made of very small particles that are in constant, random motion that collides elastically with each other and with the walls of the container. 1. Temperature (in Kelvin) is related to the average kinetic energy of gas molecules. 2. Pressure (in atmosphere or mmHg or torr) is related to the frequency of collision between molecules and walls of the container. 3. Volume (in liters or mL or m^3) is the space occupied by gas molecules 4. Amount of substance (in moles) is the number of gas molecules there is in a sample. a. Temperature and Pressure are directly related (Gay-Lussac's Law) when other variables are constant. b. Volume and Temperature are directly related (Charles' Law) when other variables are constant. c. Volume and amount of substance are directly related (Avogadro's Law) when other variables are constant. d. Volume and Pressure are inversely related (Boyle's Law) when other variables are constant. These laws can be summarized in a single equation known as Ideal Gas Law: PV = nRT; where P is pressure, V is volume, n is the amount of substance, T is temperature, and R is the universal gas constant.