1. Unit 7 Test Review

2. quantity of heat needed to raise the temperature of 1 g of water by 1 C calorie

3. SI unit of energy Joule

4. quantity of heat needed to change the temperature of 1 g of a substance by 1 o C Specific heat

5. heat content of a system at constant pressure enthalpy

6. device used to measure the heat absorbed or released during a chemical or physical process calorimeter

7. the enthalpy change for a chemical reaction exactly as it is written heat of reaction

8. the change in enthalpy that accompanies the formation of a compound from its elements heat of formation

9. Hess's law of heat summation states that if you add two or more thermochemical equations to give a final equation, you can also add the heats of reaction to give the final heat of reaction

10. the energy required to melt a solid at its melting point heat of fusion

11. the enthalpy change caused by dissolving a substance heat of solution

12. Describe the heat changes when piece of metal is heated, then submerged in cool water. The temperature of the water will increase and the temperature of the metal will decrease.

13. What would the flask in which an endothermic reaction were occurring feel like? Cool to the touch

14. How is the transfer of heat measured? temperature changes

15. Who has greater bond energy in an exothermic reaction, the reactants or products? reactants

16. A process that absorbs heat is endothermic

17. How many kilocalories are in 3000 calories? 3 kilocalories (or Calories)

18. What does  H stand for? the heat of reaction for a chemical reaction

19. How do we determine the enthalpy change for a reaction in an aqueous solution (what tool do we need?) Use a calorimeter

20. The amount of heat released by the complete burning of 1 mole of a substance is the ____. Heat of combustion

21. endothermic or exothermic? endothermic

22. When a solid changes to a liquid, why doesn’t the temperature change during the melting process? The heat energy is being used to change the phase

23. Why does water have such a high specific heat? Hydrogen bonds

24. Compare the energy released in the formation of a compound to the energy required to decompose that compound The energy changes are the same

25. products are at a higher energy level than are the reactants endothermic or exothermic? endothermic

26. What is exchanged between the system and the surroundings in a closed system Energy only

27. What is exchanged between the system and the surroundings in an open system Energy and mass

28. What is exchanged between the system and the surroundings in an isolated system nothing

29. Know how to do specific heat problems Know how do calculate enthalpy changes