2. Energy in Reaction Some reactions give off energy –Called _________ –Examples: –They feel _______

3. Energy continued Some reactions take in energy –Called ___________ –Examples: –They feel _________

4. From your lab…. What type of reaction was it? Where did the energy come from? What do we need to know to figure out how much energy was transferred?

5. Energy Calculations q = mC  T

6. Specific Heat Tells you how easily something heats up

7. Specific heats

8. Calculate your Q

9. Heat of Combustion How much energy is given off when a substance is burned. Measured in kilojoules or kilocalories

10. Heat of combustion Thermal energy/mass of substance burned Q/mass of candle burned

11. Molar heat of combustion Amount of energy to burn 1 mole of a substance kJ/mol Q/moles burned

12. What is efficiency???

13. What are some ways your car is inefficient?

14. Where are some places your lab set up could have lost heat??

15. Step 1 Bonds need to be broken so that they can be rearranged –Endothermic - energy is needed Energy + CH 4 + 2O 2  C + 4H + 4O Energy must be added to “pull apart” the compounds

16. Step 2 The separate atoms need to form new bonds to make our products. –Exothermic change - energy is given off C + 4H + 4O  CO 2 + 2H 2 O + energy

17. Energy Reaction coordinate Reactants Products 2 Hydrogens1 Oxygen 2 Waters

18. Overall Reaction The energy released when bonds are formed in CO 2 and H 2 O is more than the energy needed to break the bonds of CH 4 and O 2 –Therefore, the total reaction is exothermic (gives off energy)

19. Exo Vs Endo If the total reaction GIVES OFF heat it is exothermic If the total reaction REQUIRES HEAT it is endothermic If one reaction is exothermic, the complete opposite would be endothermic

20. Energy Reaction coordinate Reactants Products Activation Energy  Energy required to make the reaction happen

21. Energy Reaction coordinate Reactants Products Heat released Exothermic Reaction

22. Energy Reaction coordinate Reactants Products Heat absorbed Endothermic Reaction

23. Practice Problems How many calories of heat are taken in when 10.0 g of water cool from 50.0 o C to 25.0 o C? Iron has a specific heat of 0.11 cal/gºC. How much heat will it take to change the temperature of 48.3 g of iron by 32.4ºC?