Notes from april 26 - chem
Notes from april 26 - chem Chemistry 1030
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This 3 page Class Notes was uploaded by Emma Shoupe on Thursday April 28, 2016. The Class Notes belongs to Chemistry 1030 at Auburn University taught by Dr. Livia Streit in Spring 2016. Since its upload, it has received 11 views. For similar materials see General Chemistry 1 in Chemistry at Auburn University.
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Date Created: 04/28/16
Chemistry 1030 April 26, 2016 Chapter 11 – Gases https://docs.google.com/presentation/d/16UDwxEWD4o8C5cItI6elkonEEoDB3 n_lK9E3B9x-XEY/edit#slide=id.p16 11.1- Properties of Gases A sample of a gas assumes both the shape and the volume of a container Gases are compressible Densities are much smaller than liquids and solids and are variable depending on the temperature and pressure Gases are always homogenous mixtures with other gases 11.3- Gas Pressure Pressure- force applied per unit o Pressure = Force/Area o 1 Pa = 1 N/m squared o common standard pressure units- 1 atm = 760 mmHg = 760 torr = 101.3 kPa 11.4 Gas Laws Boyle’s Law- constant temperature o Pressure decreases, volume increases o Inverse relationship o Ex- balloon in a vacuum will expand o V = 1/P o P1 x V1 = P2 x V2 Charles and Gay-Lussac’s Law- states that the volume of a gas maintained at constant pressure is directly proportional to the absolute temperature of the gas o Example- heat a balloon and it expands. Cool a balloon and it shrinks. Avagadro’s Law – states that the volume of a sample of gas is directly proportional to the number of moles in the sample at a constant temperature and pressure Combined gas law- used to solve problems where any or all of the variables changes o look for variables you have and don’t have 11.5 – Ideal Gas Equation gas laws can be combined into a general equation that describes the physical behavior of all gases o R is called the gas constant…R = 0.08206 L·atm/mol·K o n= number of moles of gas o Be careful of units! (P= atm, V= Liters, T=Kelvin) PV = nRT