Chemistry - The Central Science Chapter 3

Chemistry - The Central Science Chapter 3 - Chapter 3...

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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 HW #P2 3.4, 3.12, 3.20, 3.24, 3.34, 3.46, 3.58, 3.63, 3.73, 3.91 P2 will be covered by Quiz 2 and Exam 1.
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Chapter 3 Stoichiometry Y 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 – 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 C. 12 12 g of C has 6.022 × 10 atoms of C 23 6.022 × 10 is called Avogadro's number 2 1 mole of O has 6.022 × 10 molecules of oxygen 2 1 mole of H O has 6.022 × 10 molecules of water
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Note that the mole is also defined by relation to mass 1 mole of C = 12g of C 12 1 atom of C = 12 amu 1 mole of a compound equals the mass of the compound in grams equal to the molecular mass 12.00g C = 1 mole C = 6.022 × 10 atoms of C 23 32.06g S = 1 mole S = 6.022 × 10 atoms of S 12.01g C = 22 2 18.0g of H O = 1 mole H O = 6.0×10 molecules of H O 2 32.0 g of O = 1 mole O 6.0×10 molecules of O
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Chemistry - The Central Science Chapter 3 - Chapter 3...

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