CHEM 1212: Principles of Chemistry II

1. Convert between different temperature units including Kelvins.
2. Explain the first law of thermodynamics.
3. Define a state function, exothermic and endothermic process, enthalpy and enthalpy changes.
4. Calculate heat in joules using heat capacities, change in temperature, and heating curves.
5. Calculate Enthalpies of reactions.
6. Apply Hess’s Law to determine enthalpies.
7. Use bond energies to calculate enthalpies.
8. Calculate lattice energies using the Born-Haber cycle.
9. Identify Spontaneous Processes.
10. Utilize and Apply the Second Law of Thermodynamics.
11. Utilize the Third Law of Thermodynamics with absolute entropy.
12. Calculate Entropy Changes.
13. Calculate Gibbs Free Energy.
14. Determine the effect of Temperature on Spontaneity.
15. Convert between different pressure units including atmospheres.
16. Explain the Kinetic Molecular Theory.
17. Apply the Ideal Gas Law to changes in gaseous systems.
18. Calculate density, molar mass and molar volume of gases.
19. Relate intermolecular forces to vaporization and vapor pressure.
20. Utilize the Clausius-Clapeyron equation as Pressure and temperature changes.
21. Relate intermolecular forces to phase diagrams.
22. Relate intermolecular forces to trends in solubility.
23. Apply Henry’s Law and the Solubility of Gases.
24. Apply Raoult’s Law to solutions of volatile substances.
25. Convert between Units for Colligative Properties of solutions.
26. Define reaction rate and describe how it changes over time.
27. Write the rate law expressions, and integrated rate law expressions.
28. Calculate half-lives and rate constants.
29. Apply rate laws to radioactive decay and radiometric dating.
30. Use the Arrhenius equation to examine the effect of temperature on reaction rate.
31. Describe the effect of orientation factor and collision frequency on rates of reactions.
32. Describe the use of elementary steps to explain rate laws.
33. Explain how catalysts lower the transition states of reactions.
34. Describe dynamic equilibrium.
35. Describe the relationship between the equilibrium constant, K, and the chemical equation.
36. Manipulate equilibrium constants.
37. Predict the direction of change based on the reaction quotient.
38. Calculate K for heterogeneous equilibria.
39. Apply Le Chatelier’s Principle when a disturbance occurs at equilibrium.
40. Calculate using the equilibrium constant.
41. Apply Thermodynamics to equilibrium.
42. Explain how temperature affects K.
43. Define the Arrhenius Acid and Base.
44. Describe acid strength based on molecular structure.
45. Describe base strength.
46. Describe conjugate pairs.
47. Utilize the autoionization of water and define pH, pOH, pKa and pKb.
48. Determine Percent Ionized in strong or weak acid or basic solutions.
49. Find the pH in acidic or basic solutions.
50. Describe the acid-base properties of ions and salts excluding any weak-weak interaction.
51. Use the Henderson-Hasselbalch equation to calculate pH of buffers and changes.
52. Utilize pH buffers and describe Buffer Effectiveness, buffer range and capacity.
53. Calculate the pH of a monoprotic acid solution in a titration.
54. Define Lewis Acids and Bases.
55. Draw and label the components of a voltaic cells.
56. Calculate the potential of a standard voltaic cell.
57. Relate cell potential, free energy and the equilibrium constant.