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by: Rebecca Justice

Moles CHM 111

Rebecca Justice
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About this Document

This covers everything we talked about with moles including converting and Avogadro's number.
Foundational general chemistry
Cynthia A Harwood
Class Notes
General Chemistry, Moles, Avogadros Number




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This 3 page Class Notes was uploaded by Rebecca Justice on Tuesday October 18, 2016. The Class Notes belongs to CHM 111 at Purdue University taught by Cynthia A Harwood in Fall 2016. Since its upload, it has received 17 views.


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Date Created: 10/18/16
Chapter 3 Stoichiometry (Week 8) Tuesday, October 18, 2016 10:04 AM Molecular compounds are made up of molecules Molecules are a small number of nonmental atoms held together by covalent bonds Using water as an example, because the masses of Hydrogen and Oxygen will vary based on the samples of water taken there is a more convenient way to express the composition of a compound that would work for ANY sample size PERCENT COMPOSITION! Makes it possible to convert the mass of each component into a percentage of the total mass which will be standard across all samples THE MOLE Mole- SI unit for describing the amount of a substance Amount of substance that contains the same number of particles as present in exactly 12 g of pure carbon-12 Mole (mol)- counting unit for objects (atoms, molecules, ions, etc.) 6.022*10^23 (Avogadro's number) used to determine number of objects Avogadro's number was chosen so that 1 mole of 12C atoms has a mass of exactly 12g 1 mol = 6.022*10^23 formula units To be clear one formula unit of water is one H2O molecule or one formula unit of elemental nitrogen is one N2 molecule Moles* Avogadro's number= number of formula units Number of formula units/ Avogadro's number= moles Some quick definitions Molecular mass- mass of one molecule (in amu) Formula mass- mass of one formula unit (in amu) Molar mass- mass of one mole of molecules or formula units (in g/mol) Molar mass (M) of a substance= mass of 1 mole in grams…numerically equal to the formula weight in amu EX: Avg. mass of 1 C atom= 12.011 amu Mass of 1 mole of C= 12.011 g Molar mass= mass of 1 mole in grams


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