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FSU CHM 1045 - Exam 2 Study Guide
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CHM1045 Exam 2 Study Guideo Writing and balancing chemical equations. ex. Write and balance equation Al2O3Al+O2  Al2O34 Al+3O22Al2O3o Calculating amount of reactants and products Ex. C6H12O6 + 6O2  6CO2 + 6H2O856 grams of C6H12O6 is consumed, mass of CO2 produced?856 C6H12O6 g * 1 mol C6H12O6 = 4.725 mol C6H12O6 180.2g C6H12O64.725 mol C6H12O6 * 6 mol CO2 * 44.01g CO2 = 1.25*103 g CO2 1 mol C6H12O6 1 mol CO2o Limiting reagent calculations. Ex. 637.2g of NH3 are treated with 1142g CO2 A.) Find the limiting reagent B.) Mass of (NH2)2CO C.) How much excess reagent is left in grams. 2NH3 + CO2  (NH2)2 CO + H2Oa.) 637.2g NH3 * 1 mol NH3 * 1 mol(NH2)2CO = 18.7 mol (NH2)2 CO 17.031g NH3 2 mol NH31142g CO2* 1 mol CO2 * 1 mol(NH2)2CO = 25.9 mol (NH2)2 CO 44.01g CO2 1 mol CO2Limiting Reagent is NH3b.) 18.7 mol (NH2)2 CO * 60.06 g(NH2)2 CO = 1.12*103g (NH2)2 CO 1 mol (NH2)2 COc.) 18.7 mol (NH2)2 CO* 1 mol CO2 * 44.01gCO2 = 823.4 1 mol(NH2)2CO 1 mol CO2 1142g-823.6g=319gChapter 4o SolutionsElectrolyte vs. nonelectrolyte Electrolyte: can completely ionized and create electricityNonelectrolyte: doesn’t produce any electricity o Precipitation reactionsWhat is a precipitate?An insoluble solid that separates from solutiono Acid-base reactionsBrønsted acid vs. Brønsted baseAcid: a proton donorBase: A proton accepter What is a monoprotic acid? Diprotic? Triprotic? Monoprotic: each unit yields one hydrogen upon ionization Diprotic: each unit yields two hydrogen upon ionizationTriprotic: each unit yields three hydrogen upon ionizationHydronium ion A hydrated proton ex. H3O+Bronsted Acid donates a proton to a Bronsted BaseNeutralization reactionA reaction between an acid and a base. Generally produce salt & waterAcid+ Base  Salt + WaterWhat is a salt?A product of an acid-base reactionGas forming reactionsSalt likes carbonates, bicarbonates, sulfites, and sulfideso Oxidation-reduction reactions Oxidation numbersOxidizing agent vs. reducing agentTypes of redox reactions displacement, disproportionation, combination, and decomposition Half reactions o TitrationsAcid-base titrationsRedox titrations Chapter 5o Pressure Pressure= Force/Areao Boyle’s LawP1V1=P2V2o Charles’s LawV1/T1= V2/T2o Gay-Lussac’s LawP1/T1=P2/V2 o Avogadro’s LawV= K4no Ideal gas lawPV=nRTo STPR=.021 L*atm/K*molo Density and molar mass calculations(Molar mass) M=dRT/P(Density) D=M/Vo Partial pressure and mole fraction PA= nART/Vo Kinetic molecular theory KE = .5mu---2 = CT o Gas diffusionR1/R2=


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FSU CHM 1045 - Exam 2 Study Guide

Type: Study Guide
Pages: 3
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