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Chapter 12 Stoichiometry

Chapter 12 Stoichiometry. Like a Recipe. A balanced chemical equation provides the same kind of quantitative information that a recipe does. What is it??. Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction.

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Chapter 12 Stoichiometry

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  1. Chapter 12Stoichiometry

  2. Like a Recipe • A balanced chemical equation provides the same kind of quantitative information that a recipe does.

  3. What is it?? • Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. • The calculation of quantities in chemical reactions is a subject of chemistry called stoichiometry

  4. Let’s Look at an everyday example! • In a five day work week, tiny tike is scheduled to make 640 tricycles. How many wheels should be in the plant on Monday morning to make those tricycles?

  5. Interpreting Chemical Equations • A balanced chemical equation can be interpreted in terms of different quantities, including numbers of atoms, molecules, or moles; mass; and volume.

  6. Interpreting (Cont.)

  7. Interpreting (cont.) • Always remember : Mass and atoms are always conserved in a chemical reaction.

  8. Example of Interpreting a Chemical reaction

  9. Section 2 Chemical Calculations

  10. Writing and Using Mole Ratios • Mole Ratios are used to convert between: • moles of reactant and moles of product • moles of reactants • moles of products • A mole ratio is a conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of moles.

  11. Example #1 • List the mole ratios present in the equation

  12. Example #2

  13. Practice on your own • Page 360 #11

  14. Mass to Mass claculations

  15. Example #4

  16. Practice on your Own • Page 361 # 13

  17. Other Stoichiometric Calculations • In a typical stoichiometric problem, • given quantity is first converted to moles • mole ratio from the balanced equation is used to calculate the number of moles of the wanted substance • moles are converted to any other unit of measurement related to the unit mole, as the problem requires

  18. Problem Solving Approach

  19. Practice on your own • Page 364 # 15

  20. Volume- Volume

  21. 12.3 Limiting reagent and Percent yield

  22. Limiting Reagent and Excess Reagent • limiting reagent is the reagent that determines the amount of product that can be formed by a reaction • Excess Reagent- is the reagent not used up (what is left over in a chemical reaction)

  23. ExampleChemical Equation for the preparation of Ammonia

  24. Example #1

  25. Practice on your own • Page 370 # 25

  26. Example # 2

  27. Percent Yield • The percent yield is a measure of the efficiency of a reaction carried out in the laboratory. • Theoretical yield -maximum amount of product that could be formed from given amounts of reactants • Actual yield the amount of product that actually forms when the reaction is carried out in the laboratory

  28. Example #1 (Percent Yield )

  29. Example #2 percent yield

  30. Practice on your own • Page 374-375 # 29 and 31

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