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CH3 notes

CH3 notes - Chapter 3 Stoichiometry A B C D E F G H Mole...

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Chapter 3 Stoichiometry A. Mole Concept B. Empirical Formulas C. Molecular Formula D. Balanced Chemical Equations E. Calculations from Balanced Chemical Equations F. Limiting Reagents G. Yield H. Summary HW #P2 P2 will be covered by Quiz 1 and Exam 1.

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Chapter 3 Stoichiometry h Amounts How do we measure amounts? A. Mole Concept Atoms are small and difficult to count; the mole is a convenient laboratory-scale number of particles. Definition B A mole is the amount of substance that contains as many elementary entities (atoms, molecules, ions, etc.) as there are atoms in exactly 12g of 12 C. 12g of 12 C has 6.022 h 10 23 atoms of 12 C 6.022 h 10 23 is called Avogadro's number 1 mole of O 2 has 6.022 h 10 23 molecules of oxygen 1 mole of H 2 O has 6.022 h 10 23 molecules of water
Note that the mole is also defined by relation to mass 1 mole of 12 C = 12g of 12 C 1 atom of 12 C = 12 amu 1 mole of a compound equals the mass of the compound in grams equal to the molecular mass 12.00g 12 C = 1 mole 12 C = 6.022 h 10 23 atoms of 12 C 32.06g S = 1 mole S = 6.022 h 10 23 atoms of S 12.01g C = 1 mole C = 6.022 h 10 23 atoms of C 18.0g of H 2 O = 1 mole H 2 O = 6.0h10 23 molecules of H 2 O 32.0g of O 2 = 1 mole O 2 = 6.0h10 23 molecules of O 2 Examples: 1) What is the molar mass of glucose, 6 12 6 C H O ?

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2) How many carbon atoms are in 1.00 mole of C 6 H 12 O 6 ?
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CH3 notes - Chapter 3 Stoichiometry A B C D E F G H Mole...

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