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Warm-Up 3/19/14 Balance these equations!
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Heat and Chemical Reactions
3/19/14
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Energy in Reactions Energy is stored in chemical bonds This means…
Bonds can be hard to break!
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Breaking & Forming Bonds
Step 1: Energy must be SUPPLIED to break chemical bonds Step 2: Energy is RELEASED when new chemical bonds are made
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Two Main Categories Exothermic Endothermic
More energy is RELEASED than SUPPLIED Heat “exits” Example: combustion More energy is SUPPLIED than is RELEASED Heat “enters” Example: photosynthesis, ammonium nitrate + water
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Reaction Coordinate Diagram
Shows stored energy of reactants and products Hump=where reaction is happening ∆E=overall change in energy after reaction occurs
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Represented by Equations
Enthalpy is heat energy. The change in heat energy during a chemical reaction is represented with ∆H. ∆H = E of products – E of reactants
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Combustion! Example
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Negative ∆H = exothermic (energy lost when creating products)
Positive ∆H = endothermic (energy gained when creating products)
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Try It! Exothermic or Endothermic?
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Your Job Complete the practice problems on the back of your notes for tomorrow Tomorrow: Balancing Equations QUIZ Test on Tuesday next week
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