1. © Copyright Pearson Prentice Hall Slide 1 of 30 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

2. © Copyright Pearson Prentice Hall Slide 2 of 30 > The Arithmetic of Equations > Using Everyday Equations How is a balanced equation like a recipe? 12.1

3. Slide 3 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Using Everyday Equations A balanced chemical equation provides the same kind of quantitative information that a recipe does. 12.1

4. Slide 4 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Using Everyday Equations An equation can represent the manufacturing of a single tricycle. 12.1

5. © Copyright Pearson Prentice Hall Slide 5 of 30 > The Arithmetic of Equations > Using Balanced Chemical Equations How do chemists use balanced chemical equations? 12.1

6. Slide 6 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations 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

7. © Copyright Pearson Prentice Hall Slide 7 of 30 > The Arithmetic of Equations > Interpreting Chemical Equations In terms of what quantities can you interpret a balanced chemical equation? 12.1

8. Slide 8 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations 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

9. Slide 9 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Interpreting Chemical Equations Number of Atoms 12.1

10. Slide 10 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Interpreting Chemical Equations Number of Molecules 12.1

11. Slide 11 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Interpreting Chemical Equations Moles 12.1

12. Slide 12 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Interpreting Chemical Equations Mass 12.1

13. Slide 13 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Interpreting Chemical Equations Volume 12.1

14. Slide 14 of 30 © Copyright Pearson Prentice Hall > The Arithmetic of Equations Interpreting Chemical Equations 12.1

15. © Copyright Pearson Prentice Hall Slide 15 of 30 > The Arithmetic of Equations > Mass Conservation in Chemical Reactions What quantities are conserved in every chemical reaction? 12.1

16. © Copyright Pearson Prentice Hall Slide 16 of 30 > The Arithmetic of Equations > 12.1 Mass Conservation in Chemical Reactions Mass and atoms are conserved in every chemical reaction.

17. © Copyright Pearson Prentice Hall Slide 17 of 30 Conceptual Problem 12.1

18. © Copyright Pearson Prentice Hall Slide 18 of 30 Conceptual Problem 12.1

19. © Copyright Pearson Prentice Hall Slide 19 of 30 Conceptual Problem 12.1

20. © Copyright Pearson Prentice Hall Slide 20 of 30 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

21. © Copyright Pearson Prentice Hall Practice Problems Slide 21 of 30 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.

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