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Lecture 3 (chapter 4 to 4.4) student

# Lecture 3 (chapter 4 to 4.4) student - Chapter4:TheMoleand...

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Chapter 4: The Mole and  Stoichiometry Chemistry: The Molecular Nature  of Matter, 6E Jespersen/Brady/Hyslop

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Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E Stoichiometry Mass balance of all formulas involved in  chemical reactions  Stoichiometric Calculations Conversions from one set of units to another  using Dimensional Analysis Need to know: 1. Equalities to make conversion factors 2. Steps to go from starting units to desired units 2
Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E Molecular to Laboratory Scale reactions at a molecular scale. It is known from experiments that:  Atoms must also have characteristic masses Just extremely small reactions to carry out experiments in laboratory Mole  is our conversion factor 3

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Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E The Mole Number of atoms in exactly 12 grams of  12 atoms How many atoms in 1 mole of  12 C ?  Based on experimental evidence 1 mole of  12 C = 6.022 × 10 23  atoms = 12.011 g Avogadro’s number = N A   Number of atoms, molecules or particles in  one mole  1 mole of X = 6.022 × 10 23  units of X 23 4
Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E Moles of Compounds Atoms    Atomic Mass Mass of atom (from periodic table) 1 mole of atoms = gram atomic mass  = 6.022×10 23  atoms Molecules  Molecular Mass   Sum of atomic masses of all atoms in  compound’s formula 1 mole of molecule X = gram molecular mass of X 5

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Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E Moles of Compounds Ionic compounds   Formula Mass Sum of atomic masses of all atoms in ionic  compound’s formula 1 mole ionic compound X = gram formula mass of X  = 6.022 × 10 23  formula units General Molar mass (MM) Mass of 1 mole of substance (element, molecule, or  ionic compound) under consideration 1 mol of X = gram molar mass of X     = 6.022 × 10 23  formula units 6
Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E SI Unit for Amount = Mole 1 mole of substance X = gram molar mass of X 1 mole S = 32.06 g S 1 mole NO 2 = 46.01 g NO 2 Molar mass is our conversion  1 mole of X = 6.022 × 10 23  units of X N A  is our conversion factor  1 mole H 2 O = 6.022 × 10 23    molecules H 2 O 1 mole NaCl = 6.022 × 10 23   7

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Jespersen/Brady/Hyslop Chemistry: The Molecular Nature of Matter, 6E
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Lecture 3 (chapter 4 to 4.4) student - Chapter4:TheMoleand...

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