#Chem 162-2008 2nd week recitation

#Chem 162-2008 2nd week recitation - CHEMISTRY 162-2008 2ND...

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CHEMISTRY 162-2008 2 ND WEEK RECITATION ANNOUNCEMENTS E-MAIL Students should have received my e-mail HOMEWORK Comparison of  my  homework and the Solutions Manual ATTENDANCE Sign in EXAMS QUIZZES Chem 162-2008 2 nd week recitation 1
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Dr. Ed Tavss Chem 162 edtavss@aol.com TAVSS’ SCHEDULE** Pd. Mon Tue Wed Thu Fri 0 Office hours Hickman 206 8:15 - 9:15 1 Chem 162 Recitation Section 23 Hickman 201 9:30 - 10:25 (freq. 9:30 – 11:00) 2 Chem 162 Lecture Hck-138 11:10- 12:05 Chem 162 Lecture Hickman 138 11:10 -12:05 Chem 162 Lecture Hickman 138 11:10 - 12:05 3 Chem 162 Recitation Section 25 Hickman 201 Sched: 12:50 – 1:45 12:20 – 1:15 (freq. 12:20-1:50) Chem 162 Recitation Section 31 Hickman 211 Sched: 12:50 – 1:45 12:20 – 1:15 (freq. 12:20-1:50) ** Recitations frequently run  ~ 30 minutes late. Wednesday, 2/6 to Monday, 2/11, Rec. quiz I, Wednesday, 2/20, Exam I, 9:40 – 11:00 PM, Chapters 12.1 – 13.11 Wednesday, 2/27 to Monday, 3/3, Rec. quiz II Wednesday, 3/26, Exam II, 9:40 – 11:00 PM, Chapters 14-16.5 Monday, 4/7 to Thursday, 4/10, Recitation quiz III Wednesday, 4/23, Exam III, 9:40 – 11:00 PM, Chapters 16.6-18.6,22 Monday, 5/12, Final Exam, noon - 3 PM, Chapters 12-19, 22.7-22.9 ?, Last day to drop course with “W” Chem 162-2008 2 nd week recitation 2
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PLAN FOR TODAY : CONCENTRATIONS OF SOLUTIONS - %, M, m, X, i X COLLIGATIVE PROPERTIES - van’t Hoff factor - Vapor pressure of solutions (Raoult’s Law) - Boiling point elevation - Freezing point depression - Osmotic pressure HENRY’S LAW ENERGETICS OF SOLUTIONS AND SOLUBILITIES Chem 162-2008 2 nd week recitation 3
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FORMULAS g solute + g solvent = g solution ; mol solute + mol solvent = mol solution Mass percent = grams of solute/100 g solution Mole percent = moles of solute/100 moles solution Molarity = moles of solute/L of solution Difficult but important interconversion Molality = moles of solute/kilogram of solvent PPM = grams of solute/1,000,000 grams solution Volume percent = volume of solute/100 mL of solution Proof = 2 x Vol. %; e.g., 2 x 40 mL/100 mL solution = 80 proof Mole fraction: X A = n A /(n A + n B ) X A + X B = 1 Particle fraction: i X A = in A /(in A + in B ) i X A + i X B = 1 Raoult’s law: Don’t use: P soln = X solvent P o solvent Use: P soln = i X solvent P o solvent For two volatile components: P soln = i X solventA P o solventA + i X solventB P o solventB i X solvent = in solvent /(in solvent + in solute ) i X A + i X B = 1 van’t Hoff factor, “i”; i = moles of particles in solution/moles of solute dissolved Boiling-point elevation: ΔT = T f - T i = K b im solute Freezing-point depression: ΔT = T f - T i = -K f im solute (+K f gives absolute change in temp; -K f gives actual T f or T i ) Osmotic pressure: πV = inRT π = (n/V)iRT = iM solute RT ΔH soln = ΔH solute-solutebondbreaking + ΔH solvent-solventbondbreaking + ΔH solute-solventbondforming Henry’s Law: S A =kP A ; M A = Solubility of dissolved gas in solution
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This note was uploaded on 09/23/2009 for the course CHEM 162 taught by Professor Siegal during the Spring '08 term at Rutgers.

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#Chem 162-2008 2nd week recitation - CHEMISTRY 162-2008 2ND...

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