1. Calculate the volume of gas released at 227 o C under 83.1 kPa pressure when 16 kg of NH 4 NO 3 is exploded forming N 2, O 2, & H 2 O:

2. Thermo- chemistry

3. Thermochemistry The study of heat transfer in chemical reactions

4. Thermochemistry Heat change Calorimetry TCE

5. Thermo- chemical Terms

6. System That part of nature upon which attention is focused

7. Surroundings That part of nature around the part upon which we are focused

8. Reaction Coordinate A graph of energy change versus time in a chemical reaction

9. Time Energy R P

10. Exothermic Rxn Chemical reactions that release, give off heat, or lose heat

11. Endothermic Rxn Chemical reactions that absorb, take in heat, or gain heat

12. Heat Change

13. Specific Heat The heat required to raise one gram of a substance 1 o C C: (J/g o C, J/kg o K)

14. Sp. Heat  H = mC  T

15. Heat of Fusion The heat required to melt one gram of a substance at its normal MP H f : (J/g or J/kg)

16. Heat of Fusion  H = mH f

17. Heat of Vaporization The heat required to boil one gram of a substance at its normal BP H v : (J/g or J/kg)

18. Heat of Vap.  H = mH v

19. Calculate the heat change when 10.0 g H 2 O goes from –100.0 o C to 200 o C. MP = 0 o CBP = 100 o C H f = 334 J/g H V = 2260 J/g C ice = 2.06 J/gK C water = 4.18 J/gK C steam = 2.02 J/gK

20. Drill: Calculate the heat required to change 25 g of water from 140.0 o C to 60.0 o C MP = 0 o CBP = 100 o C H f = 334 J/g H V = 2260 J/g C ice = 2.06 J/gK C water = 4.18 J/gK C steam = 2.02 J/gK

21. Calorimetry Experimental measure of heat transfer

22. Calorimeter Device used to measure heat transfer A calorimeter is an adiabatic system Experimental yield

23. Adiabatic System A system that exchanges zero heat with its surroundings  H system = 0

24.  H (J)  H = q = the heat or enthalpy change in a system  H sys = mC  T sys parts

25. Calorimetry  H system = 0  H sys =  H cal +  H rxn  H rxn = -  H cal  H rxn = -mC  T cal

26. When Q reacts in a 1.5 kg calorimeter containing 2.5 kg water ch. from 22.5 o C to 26.5 o C. Calculate  H rxn. C water = 4.18 J/gK C cal = 2.00 J/gK

27. When X reacts in a 2.0 kg calorimeter containing 1.5 kg water went from 22.5 o C to 30.5 o C. Calculate  H rxn. C water = 4.18 J/gK C cal = 1.50 J/gK

28. Homework Problems 7 & 8 On page 234

29. Thermo- chemical Equation Terms

30. Typical Reaction HCl + NaOH  NaCl + HOH

31. Heat of Reaction The heat or enthalpy change of a chemical reaction  H rxn

32. Typical Ionization HCl  H + (aq) + Cl - (aq)

33. Heat of Solution The heat or enthalpy change when a substance is dissolved  H soln

34. Combustion Reaction C x H y + O 2  CO 2 + HOH

35. Heat of Combustion The heat or enthalpy change when a substance is burned  H combustion

36. Rxn Making Cpds from ele H 2 + ½ O 2  H 2 O

37. Heat of Formation The heat required to form one mole of a compound from pure elements  H f o (kJ/mole)

38. The Degree Symbol Indicates standard conditions & molar quantities by itself or from a balanced equation.

39. Enthalpy Heat flow in a system  H

40. Gibb’s Free Energy Energy of a system that can be converted to work Determines spontaneity  G

41. Energy of Formation The energy required to form one mole of a compound from pure elements  G f o (kJ/mole)

42. Exergonic Reaction A reaction in which free energy is given off  G < 0

43. Endergonic Reaction A reaction in which free energy is absorbed  G > 0

44. Exergonic Reaction A reaction which can be spontaneous  G < 0

45. Endergonic Reaction A reaction which cannot be spontaneous  G > 0

46. Reaction at Equilibrium  G = 0

47. Interrelation Term (  G)  G interrelates thermochemistry, chemical equilibria, & electrochemistry

48. Entropy A measure of disorder  S o

49. Entropy of Formation The entropy of one mole of a substance S f o (J/mole o K)

50. Drill: Define: Heat of reaction Heat of solution Heat of formation Energy of formation Entropy of formation

51. Thermochemical Equation An equation that shows changes in heat, energy, etc

52. Drill: Identify type of rxn when:  G > 0  G < 0  G = 0

53. Thermochemical Equation  H o rxn   H f o products   H f o reactants

54. Thermochemical Equation  G o rxn   G f o products   G f o reactants

55. Thermochemical Equation  S o rxn   S f o products  S f o reactants

56. Thermochemical Equation Stoichiometry of heat change Solves theoretical yield

57. Interrelating Equation  G  H  S

58. Calculate  H,  G, &  S when 19.7 kg of BaCO 3 is decomposed into BaO + CO 2 Cmpd BaCO 3 CO 2. BaO  H f o -1216.3 -393.5 -553.5  G f o -1137.6 -394.4 -525.1 S f o 112.1 213.6 70.4

59. Calculate  H,  G, &  S when 13.6 g of CaSO 4 is changed into CaO + SO 2 + O 2 at 27 o C Cmpd CaSO 4 SO 2 CaO  H f o -1434.1 -296.8 -635.1  G f o -1321.8 -300.2 -604.0

60. Calculate the potential  H,  G, &  S for the reaction & S f o for O 2 when burning 8.8 kg of C 3 H 8 Cpd C 3 H 8 CO 2 H 2 O  H f o -103.8 -393.5-241.8  G f o - 23.5 -394.4-228.6 S f o 269.9 213.6 188.7

61. Calculate  H o,  G o, &  S when P + QR PR 2 + Q at -23 o C & T eq Compd QR PR 2  H f o (kJ/mole) -250-450  G f o (kJ/mole)-225-425

62. Heat Change Calculate the heat change when the temperature of 1.0 kg H 2 O is changed from –100.0 o C to 200.0 o C.

63. Lab Results: Cup H 2 O NaOH Thermo 5.0 g 50.0 g 4.0 g 15.0 g T i = 22.0 o CT f = 27.0 o C Cmpd NaOH Na + OH -  H f o -425.6 -240.1 -230.0 Determine: theoretical and experimental heat changes

64. When 2.00 g NaOH dissolves in a 1.0 L water in a 2.5 kg calorimeter, the temp. went from 22.5 o C to 26.5 o C. Calculate:  H o soln C water = 4.18 J/gK C cal = 2.00 J/gK

65. Bond Energy The energy change when one mole of bonds are broken  H o bond

66. Bond Equation  H bond o rxn   H bond o products  H bond o reactants

67. Bond Energies (kJ/mole) C-C347 C-H414 O-H464 C=O715

68. Drill:Calculate  H,  G, &  S in the production of 831mL ammonia at 227 o C under 250.0 kPa pressure Compd NH 3  H f o -46.1  G f o -16.5

69. HOLY MACKERAL

70. 1st Law Thermodynamics Total energy change = heat + work  E = q + W

71. Work W = Fd P = F/A V = Ad W = P  V =  nRT

72. 2nd Law Thermodynamics Total entropy in a system always increases assuming no energy is added to the system

73. Thermodynamic Rxns are State Rxns

74. State Reaction Reactions that are independent of the path; thus not dependent on intermediates

75. Calculate  H o,  G o, &  S when A + BC AC 2 + B at -23 o C & solve T eq Compd BC AC 2  H f o (kJ/mole) -150-250  G f o (kJ/mole)-125-225

76. Hess’s Law  H rxn is the same whether it occurs in a single step or a series of steps.

77. Calculate  H o,  G o, &  S when A + BC AC + B at -23 o C & T eq Compd BC AC  H f o (kJ/mole) -150-250  G f o (kJ/mole)-175-225

78. Write TE for the process 2 A + BC + D C + AH D + B 2 K H + KM + B K + MProduct

79. Write TE for the process 2 A + BC + D C + AH D + B 2 K H + KM + B K + MProduct

80. Write TE for the process 2 A + 2 BC + D C + A2 H D + B 2 K H + KP + B

81. Write TE for the process 2 A + 2 BC + D C + A2 H D + B 2 K 2 H + 2 K 2 P + 2 B

82. Drill: When 5.00 g NsCO 3 is decomposed to NsO & CO 2 in a 500.0 g calorimeter (C = 1.50 J/gK) containing 250 g of water (C = 4.18 J/gK), the water changes from 25.00 o C to 45.00 o C. Calculate the heat of rxn/mole of NsCO 3

83. Substance  H o f (kJ.mole) S  HS  H A-100H-150 B-150K-200 C -50P-250 D-125Q-300

84. Write TE for the process A + B2 C + 2 D C + A2 H + P D + B 2 K + P H + KP + Q

85. Review

86. Calculate  H total, when 40.0 g of H 2 O is changed from - 25 o C to 125 o C. FP w = 0.0 o C BP w = 100.0 o C H v = 2260 J/g C ice = 2.06 (J/g K) H f = 334 J/g C water = 4.18 (J/g K) C steam = 2.02 (J/g K)

87. Calculate  H o,  G o, &  S for AD 2 + BCAC 2 + BD at (-23 o C) Cpd BC AD 2 AC 2 BD  H f o -150 -250 -300 -175  G f o -125 -225 -250 -150 S f o 75 50 80 ? Determine S f o BD

88. Calculate  H o,  G o, &  S o for PbO 2 + COCO 2 + Pb Cpd PbO 2 CO CO 2  H f o -277.4 -110.5 -393.5  G f o -217.4 -137.2 -394.4 Calculate: T eq &  H of 48 g PbO 2

89. Calculate  H o,  G o, &  S o for N 2 O 5 + H 2 OHNO 3 Cpd N 2 O 5 H 2 O HNO 3  H f o -11.3 -285.8 -174.1  G f o -10.4 -237.2 -151.5

90. What does each symbol represent? Define what is represents:  H:  G:  S: