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# 052908 - STOICHIOMETRY Zumdahl Chapter 3 Stoichiometry y...

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Unformatted text preview: STOICHIOMETRY Zumdahl Chapter 3 Stoichiometry y The study of quantities of matter consumed and produced in a chemical reaction y Why do we care? Relative and Atomic Masses y Only relative masses can be determined from what we have already learned: { Law of Definite Proportions { Law of Multiple Proportions { Avogadros Law y Example the Law of definite proportions gives: { For NO: 14 g N to 16 g O Relative and Atomic Masses y Need to define an mass unit for atoms y Set m( 12 C) = 12.0000000 atomic mass units (amu) y Base all other masses on this y 13 C 13.0034 amu: 1.11 % y 12 C 12.0000 amu: 98.89 % How to Measure Atomic Masses Determining Average Atomic Mass Isotope Atomic Mass Relative Abundance 70 Ge 69.924 amu 20.5 % 72 Ge 71.922 amu 27.4 % 73 Ge 72.923 amu 7.8 % 74 Ge 73.921 amu 36.5 % 76 Ge 75.921 amu 7.8 % Relation to kg Microscopic Microscopic Macroscopic Macroscopic y Atomic Mass Units { 1 carbon atom = 12.011 amu { 1 sulfur atom = 32.07 amu { 1 oxygen atom = 16.00 amu { 1 gold atom = 197.00 amu y Define a Mole and use it to get grams { 1 mole carbon = 12.011 g { 1 mole sulfur = 32.07 g { 1 mole oxygen = 16.00 g { 1 mole gold = 197.00 g Relative Mass Scales (amu vs g) The Mole Avogadros number: 6.02214 x 10 23 things in a mole The Mole...
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## This note was uploaded on 07/27/2008 for the course CHEM 105A taught by Professor Bau during the Summer '04 term at USC.

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052908 - STOICHIOMETRY Zumdahl Chapter 3 Stoichiometry y...

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