Principles of Chemistry II
Principles of Chemistry II CHEM 1212
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Date Created: 10/05/15
N V39 FINAL EXAM REVIEW The types of solids that are characterized by low melting point softness and low electrical conduction isare a 0905 solids Ionic Molecular Metallic Covalentnetwork Both ionic and molecular Hydration is a speci c example of the phenomenon known generally as rap96x Dissolution Disordering Sothion Condensation Dilution The principle reason for the extremely low solubility of NaCl in benzene C5H5 is the rap96x The concentration of nitrogen in water is Great strength of solventsolvent interactions Great strength of solutesolvent interactions Great strength of solutesolute interactions Great weakness of solutesolvent interaction Nonspontaneity of the increased disorder due to mixing of solute and solvent M when the partial pressure of N2 above the solution is 0826 atm Henry s Law constant for this system is 68XlO394 molLatm a nun00 56X10394 12x103 82X10393 043 56 Calculate the molarity molality and mole fraction of methanol CH30H is a solution composed of 265 g CH30H and 244 g water Assume that the density of the solution is 0975 gmL a 0305 298X10393 306 0611 298 339 0575 298 339 0611 298 306 00575 298 306 00611 6 The vapor pressure of pure water at 25 C above a solution containing 18 g of glucose a nonelectrolyte MW 180 gmole in 95 ofwater a 243 b 234 c 0451 d 0443 e 238 7 A solution prepared by dissolving 060 g of nicotine a nonelectrolyte in water to make 12 mL of solution has an osmotic pressure of 755 atm at 250C The molecular weight of nicotine is gmole a b 43 c 40 d 160 e 060 8 Emulsifying agents typically a are nonpolar b are hydrophobic at both ends c are hydrophilic at both ends d have a hydrophobic end and a hydrophilic end e are used to separate a colloid into its constituent phases 9 At equilibrium all chemical process have ceased the rate of the forward reaction equals that of the reverse the rate constant for the forward reaction equals that of the reverse both the rate of the forward reaction equals that of the reverse and the rate constant of the forward reaction equals that of the reverse none of the above moo 9 D 10 Consider the following equilibrium a 2S0 g 02g lt gt 2 803 g From which of the following starting conditions would it be impossible for this equilibrium to be achieved a 10 mol 803 g in a 10 L container b 025 mol SO g 050 mol 0 g and 010 mol 803 g in a 10L container c 025 mol SO g and 025 mol 0 g in a 10 L container d 050 mol 0 g and 050 mol 803 g in a 10 L container e equilibrium can be achieved from any of these starting conditions 11 The equilibrium constant for reaction 1 below is 422X10393 equilibrium constant for reaction 2 is 3A2Blt gt2D The value of the E 1 2DElt gt3A2B2 a b c d e 578x10392 422x10393 178x10395 237 The value cannot be determined from the data given 12 The expression for Kc for the reaction below is 4CuOs CH4g lt gt 4Cus 2HzOg 002g a CuO Cu b CuO4Cu4 c Cu4Cu04 d COleHZOlzCHU e CH4C02H202 13 The following reaction was carried out at 250C with the initial concentration of N02 g being 070 molL and no NO g or 02 g initially present At equilibrium the N02 concentration was found to be 028 molL Calculate Kc for the reaction 2N02 999 t 02 H 2NOg 19 094 047 014 14 KC for the reaction below at 250C below is 48X10396 Calculate the equilibrium concentration molL ofClz g if the initial concentration of ICl g is 133 molL There is no I or C12 initially present 21Clg rug96x Clzg lt gt 12g 29x10393 58x10393 32x10396 64x10396 343 15 Consider the following reaction at equilibrium 2002g H 200g 02g AH 5141d The yield of COg in reaction can be maximized by carrying out the reaction a at high temperature and high pressure b at high temperature and low pressure c at low temperature and low pressure d at low temperature and high pressure e in the presence of solid carbon 16 Which ofthe following is a weak acid a HNO3 b HI c HBr d H2803 e HCIO4 17 At 60 C KW 96X103914 What are the concentration of the H and OH ions 1n pure water that is neutral at 60 C a H0H39 4 8x1014 b H0H39 4 8x107 c Ht0H39 31x10397 d HlOH39 10x10397 e Hl 10 x10397 OH39 96x10397 18 A solution haVing a pH of 14 would be described as a distinctly basic b slightly basic c neutral d slightly acidic e distinctly acidic 19 Calculate the pH of a solution that has the H30 concentration of 050M a 030 b 1370 c 030 d 730 e 050 20 What is the pH of 500mL of solution 00123 grams of CaOH2 a 296 b 317 c 968 d 1083 e 1104 21 Calculate the H in 0010 M HOCl solution Ka 3510398 a 19X10395M b 36X105M c 58X10395M d 40X10396M e 72X10396M 22 Which of the following statements is false a Solvolysis is the reaction of a substance which the solvent in which it is dissolved b Hydrolysis is the reaction of a substance and water c The anion of a weak acid reacts with water to form nonionized acid and OH39 ions d According to Bronsted Lowery the anions of strong acids are very strong bases e The conjugate acid ofa strong base is a very weak base 23 The reaction that occurs when NH4Br dissolves in water is a NH4 OH39 NH4OH b Br39 H30 cgt HBr H20 c NH3 HzO39 NH4 0H d NH4 HzO39 NH3 H30 e Br39 HzO39 HBr OH39 24 What is thepH ofa solution which is 00400 M in formic acid HCOzH and 00600 M in sodium formate NaHCOO a 392 b 396 c 400 d 952 e 408 rump Which one of the following in not a buffer NH3 amp NH4ZSO4 HBr amp KBr HCN amp NaCN NH3 amp NH4Br CH3 COOH amp NaCH3 C00 26 Consider a solution which is 015 M in HF and 010 M in KF Which response contains all the true statements and no others I If NaOH is added potassium ions react with hydroxide ions II If a small amount of NaOH is added the pH increases very slightly III If HN03 is added hydrogen ion reacts with uoride ion IV If more KF is added the pH decreases a I III and IV b II and III c II and IV d III e Another combination 27 A buffer solution is prepared by mixing 250 mL of 100 M HNOz wtith 500 mL of 0500 M calcium nitrite CaNOzz Calculate the pH a 999 443 335 305 365 488 28 Calculate the pH ofa solution prepared by adding 800 mL of0 100 M NaOH solution to 100 mL of 0100 M HN03 solution a b c d e 195 202 208 216 224 29 What a weak acid is titrated with a strong base the pH at the equilivance point is always a b c d e 7 Less than 7 Greater than 7 Less that 1 Greater than 4 30 Consider the titration of a solution of a weak acid by adding a solution of a strong base Which response includes all of the following statemtns that are true and no others a b c d e II III IV V II and IV III IV and V I and III IV and V the endpoint cannot be detected using an indicator The pH at the end of the equilivance point is 700 The solution is buffered before the equilivance points The solution is buffered both before and after the equilivabce point Methyl orange pH color range 3144 would be a better indicator for this titration than would thymol blue pH range 8096 3 l The molar solubility of BaC03 is 90X10395M at 25 C What is the solubility product constant for BaC03 a b c d e 12x10398 81x10399 53x103912 40x103915 67x103911 32 Calculate the solubility product constant for lead uoridePbFz Its molar solubility is 21x10393 M at 2500 a b c d e 44x10396 42x10397 93x10397 93x10399 37x10398 33 Chemical treatment of municipal water supplies commonly entails use of CaCO AlzSO43 and CLz The purpose of adding CaO is to Remove all HC0339 as solid CaC03 Remove most 804392 as solid CaSO4 Remove all Cl39 as CaClz Selectively kill anaerobic but not aerobic bacteria Make the water slightly basic so that addition of A12SO43 will afford a gelatinous precipitate of AlOH3 a 0306 34 In any electrochemical cell the cathode is always The positive electrode The negative electrode The electrode at which some species gains electrons The electrode at which some species loses electrons The electrode at which oxidation occurs rap96x 35 Oxidation occurs at the in a voltanic cell and oxidation occurs at the in an electrolytic cell a Anode anode Cathode cathode c Anode cathode d Cathode anode e Anode salt bridge L O A cell is constructed by immersing a strip of lead in a 10 M PbNO3z solution and a strip of silve in a 10 M NgNOg solution The circuit is completed by a wire and a slat bridge As the cell operates the strip of silver gains mass silver only and the concentration of silver ions in the solution around the silver strip decreases while the strip of lead loses mass and the concentration of the lead ions in the solution around the lead strip increases Which of the following represents the reaction that occurs at the cathode in this cell a Pb 2e39 9 Pb b Pb a Pb 2equot 0510 11gt UO 4 11gt 00 D None of these 37 Which one of the following statements about the oxidizing strength of the group IB metals Cu Ag Au is true a Cu is easier to oxidize than Au Au is easier to oxidize than Ag c Ag is easier to oxidize than Cu d Au is easier to oxidize than Cu e Nothing can be decided about this from a table of electrode potentials 38 Which of the following statements about the half cell process is true for the cell Cd l Cdzt 1M l l Cu2 1M l Cu Cu2 is reduced at the anode Cu2is reduced at the cathode Cd2 is reduced at the anode Cd2 is reduced at the cathode The spontaneous reaction that occurs in this cell is not a redox reaction rap96x 39 What is the numerical value for the standard cell potential for the following reaction 2Cr3 aq 3Cus a 2Crs 2Cu t aq a l08 V b 040 V c 040 V d 108 V e 252 V 40 Calculate the Gibbs Free Energy change fro the reaction below when initial concentration of Cr and Cu2 are 100 M 2Cr3 aq 3Cus a 2Crs 2Cu2 aq a 232 k b 623 k c 3 13 k d 232 k e 523 k 41 Calculate the equilibrium constant at 25C for the reaction below Answer is only approximate 2Cr3 aq 3Cus a 2Crs 2Cu2 aq a 1039126 b 1056 C 1088 d 1039109 e 103938 42 Four of the following factors can affect the forward rate of a chemical reaction Which one cannot affect this rate Note the question refers to reaction rate not equilibrium a Temperature b Presence of a catalyst c Concentration of reactants for the forward reaction d Removal of some of the products of the forward reaction e Physical sate nature of the reactants 43 Rage data have been determined at a particular temperature for the overall reaction 2N0 2H2 9 N2 2HzO in which all reactants and products are gases Trial Initial NO Initial Hz Initial Rate M s39l l 0 020 2 010 030 00225 3 020 020 00600 The rate law expression is rap96x rap96x rate kNO2Hz2 rate 1ltNOH22 rate kNO2Hz rate kNOHz none of the answers are correct snow 44 Evaluate the speci c rate constant k at the temperature at which the data were collected The rate law expression is rate kB2C A 2B 3C 9 Products Experiment Initial A Initial B Initial C Initial rate loss of A 1 010 M 020 M 010 M 40x102 M min391 2 040 M 020 M 010 M 40x10392 M min391 3 020 M 020 M 025 M 10x10391 M min391 4 020 M 040 M 010 M 16x10391 M min391 10 M392 min391 048 M392 min 61 M392 min 10 M392 min 14 M392 min 45 Consider a chemical reaction involving compounds A and B which is found to be rst order in A and second order in B at what rate will the reaction occur in experiment 2 Experiment Rate M s39l l 010 2 initial A 10 M 20 M Initial B 020 M 060 M 12 M s391 020 060 18 036 46 The rate constant for the rst order reaction A 9 B C is k 33 x10392 min391 at 57K What is the half life for this reaction at 57K a 21 min 30 min c 61 min d 91 min e 1200 min 47 Which statement is incorrect a The reaction rate for a zero order reaction is independent of concentration 090 0 The specific rate constant for a second order reaction is independent of temperature The half life for a first order reaction is independent of initial concentrations The rate law expression relates rate and concentration The integrated rate equation relates time and concentration 48 The disporportionation autooxidationreduction of the hypochlorite ion to chlorite and chloride ions occurs in aqueous solution The rate expression is found to be rate KClO392 Which one of the following possible mechanisms is consistent with this information Reaction 3ClO39 9 C10339 2Cl39 a C1039 ClO39 9 C10239 Cl39 slow c 3ClO39 9 C10339 2Cl39 d 01039 010239 a 010339 0139 fast ClO39 9 C1 039 slow 0 C1039 9 0239 Cl39 fast C1 0239 9 02 Clquot fast 02 ClO39 9 C10339 fast one step ClO39 9 O Cl39 slow 0 01039 a 02 0139 fast 01039 02 a 010339 fast 49 The reaction A 2B 9 B A proceeds by the following mechanism A is a catalyst AB9AB slow AB B 9B2 A fast What is the rate law expression for this reaction DP99 rate k A rate kB Rate k A B Rate 1ltAB2 Rate k A2B