1. Keeping Track of Energy During Chemical Change

2. – Use energy bar diagrams to represent energy accounts at various stages of reaction – Provide mechanism for change – Connect thermal and chemical potential energy – Focus on what is happening during the course of the reaction

3. Endothermic reaction – How do you know on which side to write the energy term? If you had to supply energy to the reactants, the products store more energy energy + Na 2 HCO 3  NaOH + CO 2 (g) Think of an algebraic equation If 3 + y = x, which is greater, y or x? Consistent with generalization that separated particles have more energy

4. Endothermic reaction This is the standard energy diagram found in most texts. But it doesn’t tell the whole story.

5. Energy Bar Charts Show energy transfers between surroundings and system Allow you to consider other energy accounts

6. Consider role of E th How does heating the reactants result in an increase in E ch ? Energy to rearrange atoms in molecules must come from collisions of molecules Low energy collisions are unlikely to produce molecular rearrangement

7. Heating system increases E th Hotter, faster molecules (surroundings) transfer energy to colder, slower molecules (system) Now reactant molecules are sufficiently energetic to produce reaction

8. Heating system increases E th Hotter, faster molecules (surroundings) transfer energy to colder, slower molecules (system) Now reactant molecules are sufficiently energetic to produce reaction

9. Now reaction proceeds During collisions, particles trade E th for E ch as products are formed After rearrangement, resulting particles move more slowly (lower E th ).

10. Consider all steps in process 1.Heating system increases E th of reactant molecules 2.Energy is transferred from E th to E ch now stored in new arrangement of atoms

11. Exothermic reaction How do you know on which side to write the energy term? – If energy flows from system to surroundings, then the products must store less E ch than the reactants CaO + H 2 O  Ca(OH) 2 + energy

12. Exothermic reaction CaO + H 2 O  Ca(OH) 2 + energy – Place energy bars for E ch

13. Exothermic reaction – Now take into account changes in E th When reactant molecules collide to produce products that store less energy, new molecules move away more rapidly

14. Exothermic reaction – System is now hotter than surroundings; energy flows out of system until thermal equilibrium is re- established

15. Consider all steps in process 1. Decrease in E ch results in increased E th 2. System is now hotter than surroundings 3. Energy eventually moves from system to surroundings via heating

16. Contrast Conventional Diagram This is the standard energy diagram found in most texts. But, again,it doesn’t tell much of the story

17. What about a spontaneous endothermic process? When Baking Soda (NaHCO 3 ) is added to vinegar (HC 2 H 3 O 2 ), the resulting reaction gets colder What caused the E th to decrease? – Some E th of vinegar was needed to separate the bonds in the reactants – Resulting products have greater E ch than before

18. Reaction useful for cold-packs The system trades E th for E ch Eventually energy enters cooler system from warmer surroundings (you!)