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Chapter12 Section01 Edit

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  • 1. Chemistry 12.1
  • 2. 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.
    12.1
  • 3. Using Everyday Equations
    • Using Everyday Equations
      • How is a balanced equation like a recipe?
    12.1
  • 4. Using Everyday Equations
        • A balanced chemical equation provides the same kind of quantitative information that a recipe does.
    12.1
  • 5. Using Everyday Equations
        • An equation can represent the manufacturing of a single tricycle.
    12.1
  • 6. Using Balanced Chemical Equations
    • Using Balanced Chemical Equations
      • How do chemists use balanced chemical equations?
    12.1
  • 7. 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 .
    12.1
  • 8. 12.1
  • 9. 12.1
  • 10. 12.1
  • 11. 12.1
  • 12. for Sample Problem 12.1 Problem Solving 12.1 Solve Problem 1 with the help of an interactive guided tutorial.
  • 13. Interpreting Chemical Equations
    • Interpreting Chemical Equations
      • In terms of what quantities can you interpret a balanced chemical equation?
    12.1
  • 14. 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.
    12.1
  • 15. Interpreting Chemical Equations
      • Number of Atoms
    12.1
  • 16. Interpreting Chemical Equations
    • Number of Molecules
    12.1
  • 17. Interpreting Chemical Equations
    • Moles
    12.1
  • 18. Interpreting Chemical Equations
    • Mass
    12.1
  • 19. Interpreting Chemical Equations
    • Volume
    12.1
  • 20. Interpreting Chemical Equations 12.1
  • 21. Mass Conservation in Chemical Reactions
    • Mass Conservation in Chemical Reactions
      • What quantities are conserved in every chemical reaction?
    12.1
  • 22. Mass Conservation in Chemical Reactions
      • Mass and atoms are conserved in every chemical reaction.
    12.1
  • 23. Conceptual Problem 12.1
  • 24. Conceptual Problem 12.1
  • 25. Conceptual Problem 12.1
  • 26. for Conceptual Problem 12.1 Problem Solving 12.4 Solve Problem 4 with the help of an interactive guided tutorial.
  • 27. 12.1 Section Quiz.
    • 12.1.
  • 28. 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
  • 29.
      • 2. A reaction that produces iron metal from iron ore is shown below.
      • Fe 2 O 3 •H 2 O( s ) + 3CO( g )  2Fe( s ) + 3CO 2 ( g ) + H 2 O( 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
    12.1 Section Quiz.
  • 30.
      • 3. What is conserved in the reaction shown below?
          • H 2 ( g ) + Cl 2 ( 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
    12.1 Section Quiz.
  • 31. END OF SHOW