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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

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chemistry 122 fall quarter 2013 review

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

chapter 5 the gaseous state
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 %)

chapter 6 thermochemistry
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 %

chapter 11 liquid solid states
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 %

chapter 12 solutions
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 %

chapter 13 rates of reactions
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 %

chapter 14 chemical equilibrium
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 %

slide8
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