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CHEM 112

by: Olivia Lee

CHEM 112 CHEM 112000

Olivia Lee
GPA 3.65
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week 2 notes
Class Notes




Popular in Chemistry

Popular in Chemistry

This 2 page Class Notes was uploaded by Olivia Lee on Sunday January 24, 2016. The Class Notes belongs to CHEM 112000 at Purdue University taught by Abu-Omar in Winter 2016. Since its upload, it has received 7 views. For similar materials see Chemistry in Chemistry at Purdue University.


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Date Created: 01/24/16
CHEM 112 1 nd Edition Lecture 3 Outline of Last Lecture I. Volume and its relation to pressure II. Boyle’s Law III. Charles’ Law Outline of Current Lecture I. Ideal Gas Law II. Dalton’s Law III. Kinetic-Molecular Theory of Gasses Current Lecture  Ideal Gas Law PV=nRT  We can solve for density in the Ideal Gas Law using substitution d= m = Px MN v RT  Two balloons filled with CO2 & O2 held at equal temperature and pressure. They have… -same number of molecules -same number of moles -CO2 has the greatest mass -CO2 has the greatest density  Dalton’s Law of Partial Pressures -gases in a mixture behave independently and exert the same pressure they would exert if they were in the container alone. -when a gas is collected about a liquid, such as water, the liquid’s vapor adds to the gas and total pressure. P(total) = P(gas) + P (H20 vapor) Example problem: Suppose 2.25 L of H2 gas is collected over water at 18.0 degrees Celsius and 722.8 torr. How many moles of H2 are produced in this reaction? 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. 1. Convert to K: 18°C +273=291 Kelvin 2. Convert to atm & subtract water pressure value 722.8torr−15.5torr=.931atm 760 3. Plug into PV=nRT (.931atm)(225L)=n(0.08206)(291K) Solve for n.  Kinetic-Molecular Theory of Gasses -a model that explains experimental observations about gases under normal temperature and pressure conditions that we encounter in our environment. -the pressure of a gas arises from the sum of the collisions of the particles with the walls of the container. -the average kinetic energy of gas particles depends only on the absolute temperature. Compare the gasses Ar, CO2, and H2 all at the same temperature. Which has average greatest kinetic energy? Same because ‘T’ is the same. Which has the greatest average velocity? Hydrogen because it’s the lightest gas.


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