Energy & Chemical Change

1. Energy & Chemical Change -_______ is the ability to do ______ or produce _____ I. Potential Energy -__________ energy is the energy of ________, like the water stored behind the dam, or the energy of ____________ of a __________, which depends on the _____ of ______, the _______ and _____ of ______ joining the ______ together, and the way the ______ are _________

2. Energy & Chemical Change I. Potential Energy The ____ of all the _____ _____________ _________ for all ______ in a ________ determines the chemical _________ _______ for that __________

3. Energy & Chemical Change II. Kinetic Energy -__________ energy is the energy of ________. When the gates of the dam open, the _________ energy of the stored water is converted to _________ energy and used to do the ______ of generating ___________ -the ________ energy of a __________ is directly related to the _______ ________ of its _________ and is ______________ to its ____________

4. Energy & Chemical Change III. Specific Heat -the _________ ______ of a substance is the amount of ______ required to raise the ____________ of ____ _____ of that substance ____ _________ _______ -the _________ ______ of ______ is ____ ________, or _____ J/g·°C A. Calculating Specific Heat

5. Energy & Chemical Change III. Specific Heat A. Calculating Specific Heat If the temperature of 34.4 grams of ethanol increases from 25.0°C to 78.8°C, how much heat has been absorbed by the ethanol?

6. Energy & Chemical Change III. Specific Heat A. Calculating Specific Heat A 4.50-gram nugget of pure gold absorbed 276 joules of heat. What was the final temperature of the gold if the initial temperature was 25.0°C?

7. Energy & Chemical Change q c = x m x ΔT III. Specific Heat A. Calculating Specific Heat A 155-gram sample of an unknown substance was heated from 25.0°C to 40.0°C. In the process, the substance absorbed 5676 joules of energy. What is the specific heat of the substance, and what is the substance? q = the heat absorbed or released c = the specific heat of the substance m = the mass of the sample in grams ΔT = the change in temperature in °C

8. Energy & Chemical Change III. Specific Heat A. Calculating Specific Heat How much heat, in calories, is absorbed by a 2000 kilogram granite boulder as it is warmed from 25.0°C to 44.0°C? A 100.0-gram ingot of silver absorbed 1182 joules of heat. What was the final temperature of the silver if the initial temperature was 25.0°C?

9. Energy & Chemical Change III. Measuring Heat -a _____________ is an insulated device used for measuring the amount of _____ _________ or _________ during a ________ or ________ reaction, usually by measuring the __________ change of a known _____ of ______ What is the specific heat of an unknown metal, and what is the unknown metal, if a 49.4 gram sample of the metal is heated to an initial temperature of 115°C and placed in 125 grams of water, raising the temperature of the water from 25.6°C to 29.3°C and lowering the temperature of the metal from 115°C to 29.3°C?

10. Energy & Chemical Change III. Measuring Heat -calorimetry lab 1. Hypothesis: 2. Prediction: 3. Gather Data: A. Safety: B. Procedure:

11. Energy & Chemical Change III. Measuring Heat -calorimetry lab 3. Gather Data: B. Procedure:

12. Energy & Chemical Change III. Measuring Heat -calorimetry lab 3. Gather Data: B. Procedure:

13. Energy & Chemical Change III. Measuring Heat -calorimetry lab 3. Gather Data: B. Procedure: 4. Analyze Data: 5. Draw Conclusions:

14. Energy & Chemical Change IV. Enthalpy (Heat) of Reaction -_________ is the _____ of a system at a constant _________, while the _________ of ________, or _____ is the ___________ between the _________ of the substances at the __________ of the reaction and the substances at the ____ of the reaction -a ______________ __________ is a balanced chemical equation that includes the _______ _____ of all reactants and products and the energy change, expressed as the _______ in ________, or ____

15. Energy & Chemical Change IV. Enthalpy (Heat) of Reaction Referring to Table 16-5 on p. 501 of your text write a complete balanced thermochemical equation for the combustion of sucrose, hydrogen, and ethanol.

16. Energy & Chemical Change V. Changes of State -physical processes, such as ________ in ______, also absorb or release _____ -the amount of _____ required to _________ one _____ of ______ into ____ is called that substance’s ______ ______________ of ___________, or _____ -the amount of _____ required to ____ one _____ of ______ into _______ is called that substance’s ______ ______________ of ______, or _____

17. Energy & Chemical Change V. Changes of State -the amount of _____ that must be _________ in the ___________ process of ____________ is the same amount of _____ that is ________ in the ___________ process of ___________, or _____ = ______ -the amount of _____ that must be _________ in the ___________ process of ________ is the same amount of _____ that is ________ in the ___________ process of ___________, or _____ = ______

18. Energy & Chemical Change V. Changes in State Referring to Table 16-6 on p. 502 of your text write a thermochemical equation for the condensation of ethanol, the solidification of methanol, and the vaporization of ammonia.

19. Energy & Chemical Change VI. Calculating Energy Releases in a Reaction What amount of heat, in kilojoules, is required to melt 25.7 grams of solid methanol at the melting point of methanol? What amount of heat, in kilojoules, is evolved when 275 grams of ammonia gas condenses to a liquid at the boiling point of ammonia? What mass, in grams, of methane must be burned in order to produce 12,880 kilojoules of heat?

20. Energy & Chemical Change VII. Hess’s Law -some __________ ___________ occur slowly over millions of years, while others occur under conditions difficult to duplicate in the _________, and others occur accompanied by the production of many other _________ -_______ ____ states that ____ or _____ thermochemical equations can be added together to produce a ______ __________, and the ____ of the _________ __________ for the individual __________ is the _________ _______ for the ______ _________

21. Energy & Chemical Change VII. Hess’s Law What is the enthalpy change, in joules, for the decomposition of Hydrogen peroxide? Hydrogen peroxide is made by the synthesis reaction of hydrogen and oxygen: So… Water is made by the synthesis reaction of hydrogen and oxygen: So the final equation for the decomposition is like the sum of the equations for the individual decomposition and synthesis reactions…

22. Energy & Chemical Change VII. Hess’s Law Add the individual equations together and cancel the common terms: What is the enthalpy change, in joules, for the following single replacement reaction: If: and…

23. Energy & Chemical Change VII. Hess’s Law First, if: then… finally:

24. Energy & Chemical Change VII. Hess’s Law What is the enthalpy change, in joules, for the following reaction: What is the enthalpy change, in joules, for the following reaction:

25. called the standard enthalpy of formation, represented by dHof. Unless specified, the temperature is 298 K. Energy & Chemical Change VIII. Standard Enthalpy (Heat) of Formation -________ _________ of __________, or _____, is the ________ in _________ that accompanies the __________ of ___ ____ of a _________ in its __________ ______ from its constituent _________ in their __________ ________ -_________ and __________ are in their _________ _______ at _____________ of ________ and _____ or _____ -formation reactions with negative _____ values are __________, and formation reactions with positive _____ values are ___________

26. Energy & Chemical Change IX. Hess’s Law Calculation Using Standard Enthalpies of Formation What is the enthalpy change, in kilojoules, for the following reaction:

27. Energy & Chemical Change IX. Hess’s Law Calculation Using Standard Enthalpies of Formation What is the enthalpy change, in kilojoules, for the following reaction:

28. Energy & Chemical Change IX. Hess’s Law Calculation Using Standard Enthalpies of Formation What is the enthalpy change, in kilojoules, for the following reaction: (See Appendix C, Table C-13, on p. 921)

29. Energy & Chemical Change IX. Hess’s Law Calculation Using Standard Enthalpies of Formation What is the enthalpy change, in kilojoules, for the following reaction: (See Appendix C, Table C-13, on p. 921)

30. Energy & Chemical Change IX. Hess’s Law Calculation Using Standard Enthalpies of Formation Given the enthalpy change for the reaction, calculate the standard enthalpy of formation for Sodium carbonate, in kilojoules: (See Appendix C, Table C-13, on p. 921)

31. Energy & Chemical Change IX. Hess’s Law Calculation Using Standard Enthalpies of Formation Given the enthalpy change for the reaction, calculate the standard enthalpy of formation for Iron(III) oxide, in kilojoules: (See Appendix C, Table C-13, on p. 921)

32. Energy & Chemical Change X. Spontaneous Processes -a ____________ ________ is a _________ or __________ change that occurs with ___ _________ ___________, like ______ ________ -_____ ________ is a ____________ ________, and an __________ _______, and if we ________ the reaction, the _____________ of ______ is ______________, and ____________ -however, not all _________ reactions are __________, not all ___________ reactions are _____________

33. Energy & Chemical Change XI. Entropy -besides __________, another factor that determines whether or not a reaction is _____________ or ________________ is ________ -________ is a measure of the ________, or ____________, of the __________ in a system -if the _______ of the system __________ during a reaction, the ________ is ________; if the _______ of the system ________ during a reaction, the _______ is ________

34. Energy & Chemical Change XI. Entropy -________ in _______ can be predicted A. Changes in State -as matter undergoes ________ in ______, from ______ to ________ to _____, the _________ become increasingly _________, and the _______ _________ -___________ gases in a _______ solvent ________ the ___________ and ________ of movement of the _______, which __________ the ______ B. Solvation of Gases C. Production of Gases

35. Energy & Chemical Change XI. Entropy D. Solvation of Solid or Liquid -__________ a ______ or a _______ _______ in a _______ _________ the ___________ or _________ of a system, which _________ the _______

36. Energy & Chemical Change XI. Entropy E. Increase in Temperature -an _________ in ___________ causes an ________ in the _______ ________ of the __________ of matter, regardless of which ______ it is in XI. Entropy -a ____________ ________ is one that _________ the ________ of the _________, or ________ -if _______ = ________ + _________, then __________ reactions, which ________ __________ by increasing ___________, ________ _________, and so are ___________ -also, if a reaction _________ _______, whether it is __________ or ___________, it _________ ________, and is ___________

37. Energy & Chemical Change XII. Free Energy -_____ _______ is the energy available to do _____, and is calculated by the equation: -if the change in the _____ ______, or _______, is ________, the process is ___________, and if the _______ is ________, the process is ______________ -when a reaction occurs under _________ conditions the _________ _____ _______ change, ________ is calculated by the equation:

38. Energy & Chemical Change XIII. Calculating Free Energy Change Calculate the free energy change, and determine the spontaneity of the reaction in which nitrogen and hydrogen form ammonia:

39. Energy & Chemical Change XIII. Calculating Free Energy Change Calculate the free energy change, and determine the spontaneity of the following reaction under standard conditions: