Review_for_Exam_2

Review_for_Exam_2 - 3. Oxidation – Reduction Reactions...

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Review for Exam 2
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From before Stoichiometry - Conversions Mole mole Use the mole ratio from the balanced Chem. Equation Mole Mass Use the Molecular weight as a conversion factor This is specific to the atom or molecule you are working with Mole Number of Particles Use Avogadro’s number as a conversion factor This is specific to the type of particle you are working with
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For Exam 2 Solution (Solute, Solvent, Solubility, Saturation point ) Electrolyte (Strong, weak, non–electrolytes) Molarity Making a solution of known concentration Calculate concentration of ions Dilution formula M 1 V 1 = M 2 V 2 moles of solute = Molarity = liters of solution M
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Nomenclature Types of Chemical Reactions 1 . Precipitation Reactions ( Formula equation,Complete ionic equation,Net ionic equation, Rules for Solubility ) 2. Acid Base Reactions ( Neutralization reaction, Titration)
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Unformatted text preview: 3. Oxidation – Reduction Reactions (Oxidation State and rules, Balancing Oxidation – Reduction Equations) Gases State of a Gas Units for pressure ( Common units: Torr, Hg; SI units: pascal, atm) Gas laws Boyle’s, Charles’s, Avogadro’s, Ideal gas law, Daltons law of partial pressures, Mole fraction -Kinetic molecular theory Gas properties Root mean square (rms) velocity, diffusion, effusion Thermochemistry 1. Energy ( Potential, Kinetic, Internal energy, The First Law of Thermodinamics) Δ E = q + w 2. Work, Heat (w= - P Δ V, exothermic, endothermic energy) 3. Enthalpy (Hess’s law, Standard enthalpies of formation) Questions to practice for Chapter 6 Page 278. Exercises: 69, 70, 71 Page 279. Exercises: 72, 73, 74 Page 279. Exercises: 82, 83....
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This note was uploaded on 04/21/2011 for the course CHEM 102 taught by Professor Peterpastos during the Spring '08 term at CUNY Hunter.

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Review_for_Exam_2 - 3. Oxidation – Reduction Reactions...

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