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The Arithmetic of Equations

12.1. The Arithmetic of Equations.

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The Arithmetic of Equations

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  1. 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 they need to make a certain amount of product. Determining the quantities of reactants and products in a reaction requires a balanced chemical equation.

  2. 12.1 Using Everyday Equations • Using Everyday Equations • How is a balanced equation like a recipe?

  3. 12.1 Using Everyday Equations • A balanced chemical equation provides the same kind of quantitative information that a recipe does.

  4. 12.1 Using Everyday Equations • An equation can represent the manufacturing of a single tricycle.

  5. 12.1 Using Balanced Chemical Equations • Using Balanced Chemical Equations • How do chemists use balanced chemical equations?

  6. 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.

  7. 12.1 Interpreting Chemical Equations • Interpreting Chemical Equations • In terms of what quantities can you interpret a balanced chemical equation?

  8. 12.1 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.

  9. 12.1 Interpreting Chemical Equations • Number of Atoms

  10. 12.1 Interpreting Chemical Equations • Number of Molecules

  11. 12.1 Interpreting Chemical Equations • Moles

  12. 12.1 Interpreting Chemical Equations • Mass

  13. 12.1 Interpreting Chemical Equations • Volume

  14. 12.1 Interpreting Chemical Equations

  15. 12.1 Mass Conservation in Chemical Reactions • Mass Conservation in Chemical Reactions • What quantities are conserved in every chemical reaction?

  16. 12.1 Mass Conservation in Chemical Reactions • Mass and atoms are conserved in every chemical reaction.

  17. Conceptual Problem 12.1

  18. Conceptual Problem 12.1

  19. Conceptual Problem 12.1

  20. 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

  21. 12.1 Section Quiz. • 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

  22. END OF SHOW

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