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Schedule to Exam 1

Date Day Topics
1/14 Mon Introduced class. Went over syllabus. CH302 is harder that CH301.
1/16 Wed Reviewed some subjects from CH301. Concentrations: molarity, percent concentration, mole fraction, and molality. Also discussed importance of equilibrium - dynamic equilibrium. Pointed out importance of the mass action expression which is equal to Q (reaction quotient) at ALL times. IF the reaction is AT equilibrium, then the mass action expression will equal K, the equilibrium constant (much more of this when we get to Chapter 6 in February). Analyzed the free energy equation: G = H - TS. Plotted the equation. Slope is negative and equal to -S. All systems will respond to their condition by lowering the free energy - this is typically done by finding the perfect "balance" in the mix of reactants and products. First homework (hw01) is available on Quest.
1/18 Fri Discussed vapor pressure and the equilibrium involved. Showed how vapor pressure vs temperature is DIFFERENT than for an ideal gas. Why? Because of the increase in evaporation rate and thus the increase in gas (vapor) molecules. Plotted vapor pressure vs temperature. Showed the Clausius-Clapeyron equation which rates a set of vapor pressures at two different temperatures and the enthalpy of vaporization.
1/21 Mon MLK - Holiday. No class.
1/23 Wed Official start of Chapter 17. Thermodynamics of solvation - making solutions. Pointed out the differences between non-electrolytes, strong-electrolytes, and weak-electrolytes. Picked NaCl as our example of a dissolving solute. Showed the 3 theoretical steps in going from separate solute and solvent to a solution (homogeneous mixture). The enthalpy of solution can be positive or negative. A positive ΔH can still be spontaneous (-ΔG) as long as the entropy change (ΔS) is great enough.
1/25 Fri Finished up with section 17.2 - entropy effects on solvation. Then moved into sections 17.3. Discussed "likes dissolve likes". Also discussed the solubility of gases (like air) in solutions and in particular water. Henry's Law (p. 835) Looked at how temperature affects solubility - it can increase or decrease it. It depends on whether the chemical equation for solvation is endothermic or exothermic.
1/28 Mon Started in on section 17.4 and discussed vapor pressure of solutions. Raoult's Law is very important here. Gave out the list of 4 colligative properties and each of their equations.
1/30 Wed Went over Raoult's Law when 2 volatile liquids are mixed. Worked out a problem illustrating this mixing liquids "A" and "B". Also worked a problem where the molecular weight of an unknown was calculated via freezing point depression. Introduced the van't Hoff Factor (i) and defined the terms stated molality and effective molality. Asked clicker questions about the theoretical value of i for some salts.
2/1 Fri Finish colligative properties more discussion of van't Hoff Factor. Using colligative properties to calculate the percent ionization of a weak electrolyte. Will introduce colloids.
2/4 Mon Finished Chapter 17. Talked about colloids.
2/6 Wed Brief Exam 1 review/overview. Explained exam dos and don'ts. Officially started in on Chapter 6 - Equilibrium. Discussed the 2 views of equilibrium - (1) thermodynamics, and (2) kinetics.
2/7 Thu EXAM 1, 7-9 PM
2/8 Fri True K's (thermodynamic K's) do not have units. K's should actually be expressed using activities. Importance of knowing the differences in K, Kp, and Kc. Also discussed the way that K appears and it's value will totally depend on the way in which you balance the equation.