chapter 3

# chapter 3 - CHAPTER 3 Stoichiometry The Mole Molar Mass...

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CHAPTER 3 Stoichiometry The Mole Molar Mass % Composition Molecular Formulae Chemical Equations Balancing Chemical Equations Stoichiometric Calculations Limiting Reactant Calculations

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Stoichiometry of Chemical Reactions For any chemical conversion of reactants, Reactants Products stoichiometry expresses the mathematical connections between all reactants and products involved in the reaction
Chemical Equations Example: consider the formation of water H 2 (g) + O 2 (g) H 2 O(g) Law of Conservation of Mass must be obeyed … therefore, equations must be balanced.

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One mole of common substances: CaCO 3 =100.09 g Oxygen, O 2 =32.00 g Copper = 63.55 g Water = 18.02 g
Counting objects of fixed relative mass 12 red marbles @ 7g each = 84g 12 yellow marbles @4e each=48g 55.85g Fe = 6.022 x 10 23 atoms Fe 32.07g S = 6.022 x 10 23 atoms S

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Figure 3.1: Mass spectrometer
Figure 3.2 (a): Peaks of neon injected

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• 6.02 x 10 23 • 1 mole of 12 C has a mass of 12 g Mole
• Definition: The amount of substance that contains as many elementary particles (atoms, molecules, ions, or other ?) as there are atoms in exactly 12 grams of carbon 12. • 1 Mole = 6.022145 x 10

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## This note was uploaded on 04/29/2009 for the course CH 52365 taught by Professor Mcdevitt during the Spring '09 term at University of Texas.

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chapter 3 - CHAPTER 3 Stoichiometry The Mole Molar Mass...

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