Chapter 3 PPt - Chem I

# Chapter 3 PPt - Chem I - Chapter#3 Stoichiometry Mole Mass...

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Chapter #3 : Stoichiometry - Mole - Mass Relationships in Chemical Systems 3.1: The Mole 3.2: Determining the Formula of an Unknown Compound 3.3: Writing and Balancing Chemical Equations 3.4: Calculating the amounts of Reactant and Product 3.5: Fundamentals of Solution Stoichiometry

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Mole The Mole is based upon the definition: The amount of substance that contains as many elementary parts (atoms, molecules, or other?) as there are atoms in exactly 12 grams of carbon -12. 1 Mole = 6.022045 x 10 23 particles
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 Fig 3.1

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Mole - Mass Relationships of Elements Element Atom/Molecule Mass Mole Mass Number of Atoms 1 atom of H = 1.008 amu 1 mole of H = 1.008 g = 6.022 x 10 23 atoms 1 atom of Fe = 55.85 amu 1 mole of Fe = 55.85 g = 6.022 x 10 23 atoms 1 atom of S = 32.07 amu 1 mole of S = 32.07 g = 6.022 x 10 23 atoms 1 atom of O = 16.00 amu 1 mole of O = 16.00 g = 6.022 x 10 23 atoms 1 molecule of O 2 = 32.00 amu 1 mole of O 2 = 32.00 g = 6.022 x 10 23 molecule 1 molecule of S 8 = 2059.52 amu 1 mole of S 8 = 2059.52 g = 6.022 x 10 23 molecules
Molecular Mass - Molar Mass ( M ) The Molecular mass of a compound expressed in amu is numerically the same as the mass of one mole of the compound expressed in grams. For water: H 2 O Molecular mass = (2 x atomic mass of H ) + atomic mass of O = 2 ( 1.008 amu) + 16.00 amu = 18.02 amu Mass of one molecules of water = 18.02 amu Molar mass = ( 2 x atomic mass of H ) + atomic mass of O = 2 ( 1.008 g ) + 16.00 g = 18.02 g 18.02 g H 2 O = 6.022 x 10 23 molecules of water = 1 mole H 2 O

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CaCO 3 100.09 g Oxygen 32.00 g Copper 63.55 g Water 18.02 g Fig. 3.2 One Mole of Common Substances
Information Contained in the Chemical Formula of Glucose C 6 H 12 O 6 ( M = 180.16 g/mol) Carbon (C) Hydrogen (H) Oxygen (O) Atoms/molecule of compound Moles of atoms/ mole of compound Atoms/mole of compound Mass/molecule of compound Mass/mole of compound 6 atoms 12 atoms 6 atoms 6 moles of 12 moles of 6 moles of atoms atoms atoms 6(6.022 x 10 23 ) 12(6.022 x 10 23 ) 6(6.022 x 10 23 ) atoms atoms atoms 6(12.01 amu) 12(1.008 amu) 6(16.00 amu) =72.06 amu =12.10 amu =96.00 amu 72.06 g 12.10 g 96.00 g Table 3.2

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Mass - Mole Relationships of a Compound Mass (g) of Element Moles of Element Atoms of Element Mass (g) of compound Amount (mol) of compound Molecules (or formula units of compound) Amount (mol) of compound For an Element For a Compound
Calculating the Number of Moles and Atoms in a Given Mass of Element Problem: Tungsten (W) is the element used as the filament in light bulbs, and has the highest melting point of any element 3680 o C. How many moles of tungsten, and atoms of the element are contained in a 35.0 mg sample of the metal? Plan:

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Chapter 3 PPt - Chem I - Chapter#3 Stoichiometry Mole Mass...

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