Chemistry 2 Exam Study Guide Chapters 4 6 Formula Sheet PV nRT P1V1 T1 P2V2 T2 Pressure P f a force area Pi XiPT Pi Partial Pressure Xi Mole Fraction PT Total Pressure Xi ni nT ni Partial Moles nT Total Moles Force F mass x acceleration Avogadros Number 6 022 x 10 23 1 pascal Pa 1 N m 2 1 atm 101 325 Pa 1 atm 760 mmHg torr Kelvin C 273 15 Vrms 3RT M Urms 3RT M r1 r2 t2 t1 M2 M1 Prefixes Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca 1 2 3 4 5 6 7 8 9 10 D P MM RT D m v MM m n MM dRT P U Ufinal Uinitial U H P V P Pfinal Pinitial T Tfinal Tinitial V A x H V Vf Vi V 0 P V 0 Wsys 0 W P V or P V W F x H PT Pi Pi Total Pressure Partial Pressure Partial Pressure Yield Actual Yield Theoretical Yield 100 R 0821 liters atm moles kelvin R 8 31 jewels kelvin moles J Kilograms m 2 s 2 Daltons Law of Partial Pressures PT nT RT V nT Total number of moles nA nB nC Van der Waals Equation for non ideal gas P an 2 v 2 V nb nRT P an 2 v 2 corrected pressure V nb corrected volume a b are empirical constants Ideal Gas Boyle s law P at 1 V at constant n and T Charles s law V T at constant n and P Avogadro s law V n at constant P and T V nT P PV nRT Vacuum O Pressure KEavg mVavg 2 KEavg aT Average kinetic energy KEavg of molecules increase as temperature increases Oxidation Reduction or Redox reactions and Net Ionic Equations Example Lead II A Nitrate X is added to Strontium B Iodide Y Pb II 2 NO3 Sr 2 I AX BY AY BX Since Nitrates NEVER precipitate you can cross out X Nitrate and therefore B Strontium as well Leaving you with Pb 2I PbI2 as your Net Ionic Compounds That Never Precipitate Some Compounds That Always Precipitate Nitrate NO3 Acetate C2H3O2 Ammonium NH4 All the Alkali Metals Column 1 of the Periodic Table Carbonate CO3 2 Phosphate PO4 3 Balancing Molecular Equations and Net Ionic AgNO3 aq KI aq Products Balanced Molecular Equation AgNO3 aq KI AgI s KNO3 aq Total Ionic Equation Ag aq NO3 aq K aq I aq AgI s K aq NO3 aq Ag and I form a precipitate because of the solubility rules of molecular compounds and therefore cannot be broken down to the ion level Therefore they combine to form a solid and leave potassium K and nitrate NO3 to be crossed out as spectator ions Net Ionic Ag I AgI Half Reactions 2RbCl aq F2 g 2RbF aq Cl2 g 2Rb 2Cl F2 0 2Rb 2F Cl2 0 We have 2Cl Cl2 Cl is losing 2 electrons to get to Cl2 We have F2 2F F2 is gaining 2 electrons to get to 2F Oxidation loss of electrons 2Cl Cl2 2e is the reducing agent F2 2e Cl 2F Reduction gain of electrons F2 is the oxidizing agent LEO the lion goes GER LEO GER Loses Electrons Oxidation Gains Electrons Reduction Solubility Chart Soluble Compounds Insoluble Exceptions Compounds containing alkali metal ions Li Na K Rb Cs Halides of Ag Hg2 2 and Pb 2 Ammonium ion NH4 Sulfates of Ag Ca 2 Sr 2 Ba 2 Hg2 2 and Pb 2 Nitrates NO3 Acetates CH3COO Bicarbonates HCO3 Chlorates ClO3 Perchlorates ClO4 Halides Cl Br I Sulfates SO4 2 Insoluble Compounds Soluble Exceptions Carbonates CO3 2 Compounds containing alkali metal ions Phosphates PO4 3 Compounds containing alkali metal ions and the ammonium ion NH4 and the Ba 2 ion Chromates CrO4 2 Sulfides S 2 Hydroxides OH Oxidation States Give the oxidation state of the underlined elements a KMnO4 1 7 2 b HNO2 1 3 2 Energy is the capacity to do work Types of Energy Kinetic Molecular motion Potential Energy available by virtue of an objects position Radiant Energy from the sun and earths primary energy source Thermal Energy associated with the random motion of atoms and molecules Heat Chemical Energy stored within the bonds of chemical substances Kinetic Molecular Theory of Gases Gases are composed of molecules whose size is negligible compared to the Attractive repulsive forces between two gas molecules are negligible distance between molecules EXCEPT when they collide Gas molecules move randomly in all directions and at various speeds When gas molecules collide the collisions are elastic the energy is conserved remains the same for the entire system The average kinetic energy KEavg of the molecules increases as the temperature increases KEavg mvavg and KEavg T 2 Therefore KEavg mvavg cT c some proportionality constant m mass 2 of molecule vavg average speed m s Increase Temperature increase the kinetic energy increase the of molecular collisions increase the Pressure Heat Transfer of thermal energy between 2 bodies that are at different temperatures Temperature is a measure of thermal energy Electrolyte Substance that when dissolved in water results in a solution that can conduct electricity Strong Electrolyte 100 dissociation NaCl s Na aq Cl aq Weak Electrolyte not completely dissociated CH COOH 3 CH COO aq H aq 3 A reversible reaction The reaction can occur in both directions Nonelectrolyte A substance that when dissolved results in a solution that does not conduct electricity Strong Electrolyte Weak Electrolyte Nonelectrolyte HCl HNO3 HClO4 H2SO4 NaOH CH3COOH NH2 2CO urea HF HNO2 NH3 H2O CH3OH methanol C2H5OH ethanol C6H12O6 glucose C12H22O11 sucrose Ba OH 2 Pure water is an extremely Ionic Compounds weak electrolyte Br nsted acid Proton donor Must contain at least one ionizable proton Br nsted base Proton acceptor Neutralization Reaction acid base salt water HCl aq NaOH aq NaCl aq H2O Cl H Na OH Na Cl H2O Cross out your spectator ions of Na and Cl since you know that HCl acid and OH base must combine to make water H OH H2O Neutralization Reaction Involving a Weak Electrolyte weak acid base salt water HCN aq NaOH aq NaCN aq H2O HCN Na OH Na CN H2O HCN OH CN H2O Neutralization Reaction Producing a Gas acid base salt water CO2 2HCl aq Na2CO3 aq 2NaCl aq H2O CO2 2Cl 2H 2Na CO3 2 2Na 2Cl H2O CO2 2H CO3 2 H2O CO2 Titration When a solution of accurately known concentration is added gradually to another solution of unknown concentration until the chemical reaction between the two solutions is complete Titrations are used in the analysis of Acid Base Reactions H2SO4 2NaOH 2H2O Na2SO4 Redox Reactions 5Fe 2 MnO4 8H Mn 2 5Fe 3 4H2O Equivalence Point Point at which the reaction is complete Indicator Substance that changes color at or near the equivalence point Thermochemistry Study of heat exchange in chemical reactions Thermodynamics The scientific study of the interconversion of heat and other 1st Law of Thermodynamics Energy can be converted from one form to another kinds of energy but cannot be created or destroyed Diffusion When a …
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