CHE 131 Lecture Notes - Lecture 17: Ideal Gas Law, Partial Pressure, Van Der Waals Equation

• School: Stony Brook University
• Department: Chemistry
• Course: CHE 131
• Professor: Benjamin Hsiao, Jiangyong Jia, Roy Lacey

Document Summary

Partial pressure depends on how many moles in the mixture -- how many molecules dont care how many type. Mole fraction = fraction of moles for each individual component. Mixture is uniform so diff components of gas have the same temperature - occupy the. Ideal gas law = mole fractions in terms of pressure same volume. Mole pressure is like pressure fraction and only works for ideal gases. Percentage contribution to pressure is the percentage contribution to the moles. Partial pressure must know mole fraction to multiply by total pressure. When talking about reaction in solutions it s a similar process. Density is very low, gas occupies tiny amount of volume. Higher temperature larger the energy, kinetic energy is proportional to temperature. Under room temperature, speed is 100 m/s pretty fast. Moving at high speed makes it warm otherwise it"ll be cool. Molecules don"t influence each other except when they collide,most of times they don"t.