Chem 1061 1st Edition Lecture 11 Outline of Last Lecture I Gases and Kinetic Molecular Energy a Identity of Gas II Gas Pressure and measurement a Measuring Gas Pressure b Units of Pressure III Gas Laws and Their Experimental Foundations a Boyle s Law b Charles Law Outline of Current Lecture IV Temperature V Avogadro s Law VI Gas Behavior and Standard Conditions a Standard Temperature and Pressure b Standard Molar Volume VII Ideal Gas Law VIII Applications of Ideal Gas Law Current Lecture Note on Temperature MUST use Kelvin K scale for gas calculations These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute Table 1 6 and Figure 1 11 have more on the difference of temperatures Fahrenheit Degree F Celsius Degree C Kelvin K We primarily use Celsius and Kelvin for Chemistry Avogadro s Law Volume is proportional to amount In mol Pressure and Temperature are constants Figure 5 7 and 5 19 are diagrams and information about experimental aspect of figuring out this law An increase in n mol results in an increase in V When there is the same n there is the same volume At the same temperature gases have the same kinetic energy Gas Behavior and Standard Conditions Standard Temperature and Pressure STP 0 degree C 273 15 K and 1 atm 760 torr Standard Molar Volume volume of 1 mol of ideal gas 22 4 L Ideal Gas Law Combines the relationships Boyle s V proportional to 1 P Charles V proportional to T Avogadro s V proportional to n V is proportional to nT P PV nRT R is a universal constant R 0 0821 atm L mol K NOTE THE UNITS ON R When some variables are constant and there is a change in one variable the ideal gas law simplifies Applications of Ideal Gas Law 1 Density of a Gas 2 Molar Mass of a Gas 3 Partial Pressure of a Gas in a Mixture a Collecting Gases over H2O 4 Stoichiometry Density of a Gas Density Mass Volume g L Identity of the gas matters why Density is proportional to molar mass PV nRT PV mass molar mass RT Rearrange the variables and you get molar mass P RT Mass V Density So density is proportional to molar mass The density of a heavier gas is higher
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