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Chemistry 12.1

Chemistry 12.1. Section 12.1. The Arithmetic of Equations. 12.1. The Arithmetic of Equations.

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Chemistry 12.1

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  1. Chemistry 12.1 Section 12.1 The Arithmetic of Equations

  2. 12.1 The Arithmetic of Equations • More than 3000 cocoons are needed to produce enough silk to make just one elegant Japanese kimono. Like silk manufacturers, chemists must know how much reactant (stuff) they need to make a certain amount of product. Determining the quantities of reactants and products in a reaction requires a balanced chemical equation.

  3. 12.1 Using Everyday Equations • Using Everyday Equations • How is a balanced equation like a recipe?

  4. 12.1 Using Everyday Equations • A balanced chemical equation provides the same kind of quantitative information that a recipe does.

  5. 12.1 Using Everyday Equations • An equation can represent the manufacturing of a single tricycle.

  6. 12.1 Using Balanced Chemical Equations • Using Balanced Chemical Equations • How do chemists use balanced chemical equations?

  7. 12.1 Using Balanced Chemical Equations • 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.

  8. 12.1

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  12. 12.1 Interpreting Chemical Equations • Interpreting Chemical Equations • In terms of what quantities can you interpret a balanced chemical equation?

  13. 12.1 Interpreting Chemical Equations • A balanced chemical equation can be interpreted in terms of different quantities, including the following: • numbers of atoms • molecules or moles • mass • volume

  14. 12.1 Interpreting Chemical Equations • Number of Atoms

  15. 12.1 Interpreting Chemical Equations • Number of Molecules

  16. 12.1 Interpreting Chemical Equations • Moles

  17. 12.1 Interpreting Chemical Equations • Mass

  18. 12.1 Interpreting Chemical Equations • Volume

  19. 12.1 Interpreting Chemical Equations

  20. 12.1 Mass Conservation in Chemical Reactions • Mass Conservation in Chemical Reactions • What quantities are conserved in every chemical reaction?

  21. 12.1 Mass Conservation in Chemical Reactions • Mass and atoms (quantity) are conserved in every chemical reaction.

  22. Conceptual Problem 12.1

  23. Conceptual Problem 12.1

  24. Conceptual Problem 12.1

  25. 12.1 Section Quiz. • 1. A manufacturer of bicycles has 5350 wheels, 3023 frames, and 2655 handlebars. How many bicycles can be manufactured using these parts? • 2675 bicycles • 2655 bicycles • 3023 bicycles • 5350 bicycles

  26. 12.1 Section Quiz. • 2. A reaction that produces iron metal from iron ore is shown below. • Fe2O3•H2O(s) + 3CO(g)  2Fe(s) + 3CO2(g) + H2O(g) • In this equation, the volume of gas at STP that reacts and the volume of gas at STP produced will be • 3 L and 4 L. • 67.2 L and 89.6 L. • 67.2 L and 67.2 L • 3 L and 3 L

  27. 12.1 Section Quiz. • 3. What is conserved in the reaction shown below? • H2(g) + Cl2(g)  2HCl(g) • only mass • only mass and number of moles • only mass, number of moles, and number of molecules • mass, number of moles, number of molecules, and volume

  28. The End

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