Chemistry 1302A/B Lecture Notes - Lecture 2: Kinetic Theory Of Gases, Ideal Gas Law, Partial Pressure

• School: Western University
• Department: Chemistry
• Course: Chemistry 1302A/B
• Professor: Felix Lee

Document Summary

Due to avogadro"s law, we can devise that: "equal volumes, of different gases at the same temperature and pressure contain the same number of moles" This is contrary to what we know about molar mass where two substances with the same number of grams have different amounts of moles. A mixture of different gasses behaves like a single pressure. Ptotal = sum of partial pressure of each gas. The number of moles of the constituent gas expressed as a fraction of the whole thing. Gasses diffuse very very quickly i. e, if you mixed nitrogen and hydrogen in one room, the would completely mix in a matter of seconds. The amount of pressure that"s caused by molecules of a gas that come from a liquid. Thus, we add the pressure that the evaporated state of this water would have to the pressure. An average of the substances based upon a predetermined weighting system.