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The Arithmetic of Equations

Learn the essential concepts of balanced chemical equations, stoichiometry, and conservation laws in chemical reactions. Explore how chemists use equations and interpret quantities like mass and volume in reactions. Master the art of chemical equation calculations.

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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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