1. WARM UP Write a balanced chemical equation for the reaction of iron (3+) with atmospheric oxygen, producing rust (iron oxide).

2. Chemical Reactions

3. Symbols and Terms Reactants Yield Products Coefficients Subscripts Elements Energy Compounds State of matter 6 CO 2(g) + 6 H 2 O (l)  C 6 H 12 O 6(s) + 6 O 2(g)

4. Balancing Law of Conservation of Mass – All elements equal __ CO 2(g) + __ H 2 O (l)  __C 6 H 12 O 6(s) + __ O 2(g)

5. Calculations Coefficients identify particles or moles – 6 CO 2 = 1 C 6 H 12 O 6 – 6 moles CO 2 = 1 mole C 6 H 12 O 6 6 CO 2(g) + 6 H 2 O (l)  C 6 H 12 O 6(s) + 6 O 2(g)

6. Calculations Do coefficient conversions – Change molecules (R  P) – 97.2 moles CO 2 x 1 mole C 6 H 12 O 6 = 16.2 moles C 6 H 12 O 6 1 6 moles CO 2 6 CO 2(g) + 6 H 2 O (l)  C 6 H 12 O 6(s) + 6 O 2(g)

7. WRAP UP Calculate how many moles of water would be needed to react with exactly 743 moles of carbon dioxide to run the photosynthesis reaction at peak efficiency. 6 CO 2(g) + 6 H 2 O (l)  C 6 H 12 O 6(s) + 6 O 2(g)