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## Chapter 3 Class notes

by: Miranda Williams

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# Chapter 3 Class notes CH 1213

Marketplace > Mississippi State University > CH 1213 > Chapter 3 Class notes
Miranda Williams
MSU
GPA 3.125

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Gives examples of some important concepts including moles to grams and molarity.
COURSE
Chemistry 1
PROF.
Charles Nettles, II
TYPE
Class Notes
PAGES
2
WORDS
CONCEPTS
molarity, Moles, to, grams, conversions, dilution, formula, mass, solute, solvent
KARMA
25 ?

## Popular in Department

This 2 page Class Notes was uploaded by Miranda Williams on Monday September 12, 2016. The Class Notes belongs to CH 1213 at Mississippi State University taught by Charles Nettles, II in Fall 2016. Since its upload, it has received 3 views.

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Date Created: 09/12/16
Chapter 3: Composition of Substances and Solutions Molecular and Formula Mass  The molecular mass is the mass in atomic mass units (amu) of an individual molecule. o To calculate the molecular mass, multiply the atomic mass for each element in a molecule by the number of atoms of that element and then total the masses. Example: Molecular Mass of HOH= 2(atomic mass of H) +atomic mass of O =2(1.008)+16.00amu=18.02 amu  Molecular weight is an average molecular mass, determined by the periodic table atomic masses, which are average atomic masses. Formula Mass  Formula Mass- a sum of the atomic weights of the atoms in the empirical formula of the compound.  To calculate the formula mass, it is the same process of calculating the molecular mass. The Mole and Molar Mass  The mole is defined as the amount of substance that contains as many elementary entities as there are atoms in exactly 12g of carbon-12.  The mole determined Avogadro’s number. o Avogadro’s number is: 1mole=6.022∗10 23  Molar Mass  The molar mass of a substance is the mass in grams of one mole of the substance. o The mass of a mole of cabon-12 by definition is exactly 12g.  Mass of 1 carbon-12 atom= 12 amu  Mass of 1 mole of carbon-12= 12g Grams to moles Molecular mass Molecular mass

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