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Understanding Stoichiometry in Chemistry: Key Concepts and Mole Ratios

This note provides an introduction to stoichiometry, the study of quantitative relationships between reactants and products in chemical reactions, grounded in the law of conservation of mass. It emphasizes the importance of understanding chemical equations, including interpreting particles, moles, and mass. Key examples illustrate how to apply mole ratios as conversion factors to relate reactants and products, enabling further success in chemistry calculations. Students are encouraged to practice interpreting equations and work on assigned homework for mastery.

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Understanding Stoichiometry in Chemistry: Key Concepts and Mole Ratios

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  1. Chemistry Ch 12 Stoichiometry Notes #1

  2. What is stoichiometry? • Study of quantitative relationships btwn amounts of reactants used and products formed by a chemical reaction • Based on the law of conservation of mass • Chapter 11 math is the basis of the chapter 12 math – if you don’t get it – ask!

  3. Interpreting equations • 4Fe (s) + 3O2 (g) -> 2Fe2O3 (s) • Particles • Moles • Mass

  4. Example - interpreting • N2 (g) + 3H2 (g) -> 2NH3 (g) • Particles • Moles • Mass

  5. Homework • Interpreting • 6-14 on side 1 of sg • Number 1 on the supplemental • That much should be DONE for tomorrow!

  6. Mole Ratios • Ratio between the numbers of moles of any 2 substances in a balanced chemical equation • We will be using mole ratios as conversions factors in future math problems • Mole ratios show relationships between reactants and products in equations

  7. Example – Mole Ratio • 2Al (s) + 3Br2 (l) -> 2AlBr3 (s) • How many will there be? • Number of species x 1 less • Species = reactants and products

  8. Example – Mole Ratio • What is the mole ratio with the biggest value? • What is the mole ratio relating Al to Br? • What is the mole ratio relating the product to Al? • HW – back of SG and #2 on supp

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