1 / 8

Chemistry 122 Fall Quarter 2013 - Review

Chemistry 122 Fall Quarter 2013 - Review. 1) Sapling HW 14 11:50 pm Wednesday, 12/4/2013 2) Final Exam : (~ 2/3 Quantitative & ~ 1/3 Qualitative ) Wednesday, 12/11/2013, 8:00-10:00 am SL 120 . Chapter 5- The Gaseous State. Pressure: Lb/in 2 , Atm, mm Hg, Torr, Pa

issac
Download Presentation

Chemistry 122 Fall Quarter 2013 - Review

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Chemistry 122Fall Quarter 2013 - Review 1) Sapling HW 1411:50 pm Wednesday, 12/4/2013 2) Final Exam:(~ 2/3 Quantitative & ~ 1/3 Qualitative) Wednesday, 12/11/2013, 8:00-10:00 am SL 120

  2. Chapter 5- The Gaseous State Pressure: Lb/in2, Atm, mm Hg, Torr, Pa Pressure conversions for atmospheric pressure Barometers, Manometers Gas Laws: Boyle’s, Charles’s, Avogadro’s, Dalton’s, Combined, Ideal, Graham’s, Van der Waal’s Using Gas Laws for calculations STP (0oC & 1 atm) (1 mole gas = 22.4 L @ STP) Limitation to Ideal gas law - Van der Waal’s work Kinetic-Molecular Theory – Basics behind gas laws Significant Figures ~ 13 % (Point %)

  3. Chapter 6 - Thermochemistry Uses of thermochemistry Units for Energy: joules & calories Types of Energy – PE, KE (formula: KE = 1/2mV2) Heat Energy – SIGNS, units, names, symbols State Function Simple & Bomb Calorimeters Heat Capacity (C), Specific Heat Capacity (s) Heat Equations: q=CxΔT q=sxgxΔT ΔHr = ∑HBBroke-∑HBformΔHr = ∑ Hof prod – ∑Hof react Hess’s Law (add & subtract reactions to get new ΔHr) ∆Hof : Definition and use Above 5 ways to calculate heats of reaction- From: 1) C, 2) s, 3) Hess’s Law, 4) Bond energies, 5) Heats of formation Standard State (o) = 1 atm & 25oC Drawing Lewis Structures ~ 15 %

  4. Chapter 11 – Liquid & Solid States Phase Changes & Names Vapor Pressure Heating Curves & Calculations: q= g x s x ΔT; q= ΔHv,fx n MP, BP, TP, CT – Definitions & Uses Phase Changes & Energies Involved: ΔHvap & ΔHfusion Phase Diagrams - Draw and Interpret Polarity of both Bonds & Molecules Intermolecular Forces – Names, types, ~ strength Solids – ionic, molec, metal, cov; amorp, cryst Unit Cells – cubic types & simple calculations X-Ray Diffraction Lewis Structures ~ 11 %

  5. Chapter 12 - Solutions Solubility Rules Definitions Solution Types Lattice & Solvation Energies Le Chatelier’s Principle Henry’s Law for gas solubility: (s2/s1 = p2/p1) Concentration Terms: Xa, W/W%, pp_, M, m Colligative Properties: BP, FP, VP, Osmosis Van Hoft’s Factor, i Equations: Henry’s, BP, MP, Osmosis Use equations for calculations of: ΔT, i, MW, K’s, x, n, m Colloids; Tyndal effect Dilution Problems: C1V1 = C2V2 ~ 15 %

  6. Chapter 13 – Rates of Reactions Rate definition Factors that influence rates of reactions How measure rates Rate Law / Rate Expressions Rates, Orders, Rate Constant - what they are & calculations How to get complete Rate Law (orders) - Two ways Integrated Rate Laws & Plots (integrated rate eqns; given) Uses of Integrated Rate Equations Half-Life (t1/2) for 1st Order Rxn Mechanisms – Definition, terms & Uses Catalysts & Intermediates Arrhenius Equation & Energy of Activation (Ea) Progress of Reaction Plot - ∆H & Ea Enzymes as Catalysts ~ 22 %

  7. Chapter 14 – Chemical Equilibrium Definition of Chemical Equilibrium Equilibrium Reaction & Expression Equilibrium Constant, K or Ka, Kb, Ksp, Kf Equilibrium Expression: Write from reaction Calculations: “IE Table”; K; initial & equilibrium concentrations (amount of H+ for a weak acid & solubility of a slightly soluble compound); simplification of math with ([ ]/K > 100); use of Q Le Chatelier’s Principle Kw = 1.00x10-14 (for water) Beer’s Law: A = εbc Water & Solids Dropping from Equil. Expression ~ 22 %

  8. Study for the Final – Even if you are content with your present grade. Without study you will end up like these miserable felines. “Lion Cut” Cat in Minnesota

More Related