2. 100 400 300 200 500 100 Burn, baby Burn 400 300 200 500 100 Diagrams & Curves 400 300 200 500 100 400 300 200 500 100 400 300 200 500 Stoichiometry Redux Energizer Bunny Heat specifically

3. Column 1, 100 What is the symbol for specific heat?

4. Column 1, 200 In what units is specific heat typically expressed?

5. Column 1, 300 Breaking bonds results in this type of ΔH.

6. Column 1, 400 Potential energy Low High Reactants Products Step 1 Step 2 Which side of the reaction would the excess energy in the diagram above be represented?

7. Column1, 500 If the same amount of energy is absorbed by sand and water, which one will heat up faster and why?

8. Combustion (burning) is this kind of reaction. Column 2, 100

9. Column 2, 200 Combustion requires this to occur.

10. Column 2, 300 Combustion reactions always yield these two products.

11. Calculate the amount of thermal energy (q) that is absorbed by the water. q = mcΔT c = 4.2 J/gc Column 2, 400 Mass of water100.0 g Initial water temp18.0 °C Mass of ethanol burned0.65 g Final water temp48.0 °C

12. Column 2, 500 Write a balanced combustion reaction for methane (CH 4 )

13. Column 3, 100 Where on the graph does a solid and liquid exist simultaneously?

14. Column 3, 200 Boiling point?

15. Column 3, 300 List three phase changes that are endothermic.

16. Column 3, 400 What state is this substance in at STP?

17. Column 3, 500 At 4 atm, the temperature of this substance is decreased from -10 °C to -80 °C. What phase change occurred?

18. Column 4, 100 State the law of conservation of energy.

19. Column 4, 200 What are the five main forms of energy?

20. Column 4, 300 What 2 states can energy exist in?

21. Column 4, 400 Breaking bonds is what kind of reaction?

22. Column 4, 500 C 5 H 12 + 8O 2  5CO 2 + 6H 2 O + 3510kJ How much energy is released if 80 g of pentane are combusted?

23. Column 5, 100 C 5 H 12 + 8O 2  5CO 2 + 6H 2 O + 3510kJ How much energy is released if 4.5 moles of pentane are burned?

24. Column 5, 200 4Fe (s) + 3O 2(g)  2Fe 2 O 3(s) + 1625 kJ How many moles of oxygen are required to produce 12187.5 kJ of energy?

25. Column 5, 300 Mass of water100.0 g Initial water temperature18.0 °C Mass of ethanol burned0.65 g Final water temperature48.0 °C Calculate the number of moles of ethanol (C 2 H 5 OH) consumed from the data above.

26. Column 5, 400 C (s) + 2S (s) + 89.3 kJ  CS 2(l) How many grams of carbon disulfide are produced from 267.9 kJ of energy?

27. Calculate the molar heat of combustion (kJ/mol) based on the data above. C water = 4.2 J/gc ethanol (C 2 H 5 OH) Column 5, 500 Mass of water100.0 g Initial water temperature18.0 °C Mass of ethanol burned0.65 g Final water temperature48.0 °C