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ΔH. ΔS. Quick Calculations. spontaneity. Misc. 100. 100. 100. 100. 100. 200. 200. 200. 200. 200. 300. 300. 300. 300. 400. 400. 400. 400. 400. 500. 500. 500. 500. 500. Law that states that energy cannot be created or destroyed. Law of conservation of Energy.

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  1. ΔH ΔS Quick Calculations spontaneity Misc 100 100 100 100 100 200 200 200 200 200 300 300 300 300 400 400 400 400 400 500 500 500 500 500

  2. Law that states that energy cannot be created or destroyed

  3. Law of conservation of Energy

  4. ΔH is the change in _________ during a process

  5. enthalpy

  6. Sign of ΔH for boiling water

  7. positive

  8. Determine the sign of ΔH and ΔS for:Mg3N2(s)  3 Mg(s) + N2(g) + 200kJ

  9. ΔH = negative ΔS = positive .

  10. In an endothermic reaction, the standard enthalpy of formation of the products is ____________ (greater than or less than) the standard enthalpy of formation of the reactants?

  11. greater than

  12. Entropy is:

  13. A measure of disorder of a system

  14. Arrange the following in order of increasing entropy: HCl(g), HCl(aq), HCl(s), HCl(l)

  15. HCl(s), HCl(l), HCl(aq), HCl(g)

  16. What is the sign of ΔS for the sublimation of carbon dioxide.

  17. positive

  18. Predict the sign of ΔS for the reaction below: CaCO3 CaO + CO2

  19. positive

  20. When ammonium chloride dissolves in water, the temperature of the water drops. What is the sign of ΔS?

  21. positive

  22. For a reaction, ΔS = 64.0 J/K ΔH = 320. kJ/mol Find ΔG at 298K Is the reaction spontaneous at this temperature?

  23. 301 kJ, no

  24. For a reaction, ΔS = 64.0 J/K ΔH = 320. kJ/mol Under what conditions will this reaction become spontaneous?

  25. Above 5.00 x 103 K

  26. For a reaction, ΔS = -120.0 J/K ΔH = -240. kJ/mol Under what conditions will this reaction become spontaneous?

  27. Below 2000. K

  28. Use the bond energy table to find the energy change for breaking the reactant bonds in the reaction: 2Cl2 + O2 2Cl2O

  29. 979kJ

  30. Use the bond energy table to find the energy change for creating the product bonds in the reaction: 2Cl2 + O2 2Cl2O

  31. -812kJ

  32. Find ΔG, ΔH and ΔS for the reaction: 2Fe + 3Cl2 2FeCl3

  33. ΔG = -668 kJ ΔH = -798kJ ΔS = 436 J/K 2Fe + 3Cl2 2FeCl3

  34. What are the signs of ΔG, ΔH and ΔS for a reaction that is spontaneous at any temperature?

  35. ΔG = negative ΔH = negative ΔS = positive

  36. What are the signs of ΔG, ΔH and ΔS for melting wax

  37. ΔG = negative ΔH = positive ΔS = positive

  38. For a certain reaction: ΔH = 375. kJ ΔS = -125 J/K At what temperature will this reaction become spontaneous?

  39. The reaction is never spontaneous

  40. A student forms a yellow precipitate by mixing aqueous solutions of lead(II) nitrate and potassium iodide. Pb2+ + 2I- PbI2 Determine the signs of ΔG, ΔH and ΔS for this process.

  41. ΔG = negative ΔH = negative ΔS = negative

  42. When baking soda and vinegar are mixed in a beaker, the beaker feels cold to the touch. Determine the signs of ΔG, ΔH and ΔS for this process.

  43. ΔG = negative ΔH = positive ΔS = positive

  44. Name the law that says that in a natural process the entropy increases

  45. The Second Law of Thermodynamics

  46. What are the signs of ΔH, ΔG and ΔS for the condensation of a vapor?

  47. ΔG = negative ΔH = negative ΔS = negative

  48. Write the thermochemical equation for the formation of methane gas (CH4). ΔHf°= -75kJ/mol

  49. C + 2 H2 CH4 + 75kJ

  50. At what temperature will the process below be spontaneous: H2O(l) H2O(v)

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