CHE132_FinalExam_Fa22_Form2B

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1 CHE 132 Final Exam Fall 2022 Form 2B Directions 1. Place all other items besides your exam out of sight and or beneath your seat. 2. Place your ID (face up), pencils, erasers, and a scientific calculator at your desk now. You may be asked to show proof of ID and sign an attendance sheet. 3. On your scantron, starting from the left, write and bubble-in your (leave extra spaces blank): SBID NUMBER under IDENTIFICATION NUMBER 4. Print your name clearly and sign. 5. DO NOT OPEN YOUR EXAM until told to do so. 6. All scantron forms must be submitted by10:45 am . No extra time will be given. 7. All answers must be entered on the Scantron answer sheet, which you must turn in. 8. Answer sheets will not be returned, so record your answers next to each question on the exam for comparison with the answers when they are posted on Blackboard. Use the space between questions, the backs of pages, or the extra sheets for analysis and calculations. 9. There are 28 questions on this quiz and 20 total pages. 10. For multiple choice questions, bubble in the letter of the one choice that best completes the statement or answers the question on the scantron form. No credit will be given for multiple answers. 11. For numerical response/short answer questions, e nter your answers on the right-hand side of the scantron in the appropriately numbered line . A small amount of partial credit will be given when possible. 12. Once you open the exam, be sure you have all the pages including a Periodic Table and a sheet of equations/conversion factors. 13. General Chemistry Policies: Possession of cell phones, smart watches, other communication devices, or any unauthorized materials during the exam will result in a grade of 0 on this exam, a report to Academic Judiciary, and a possible grade of F for the course. If you do not have an ID, note that on the sign-in sheet, and you must see Dr. Nagan the day after the exam and show her a valid ID.

2 CHE 132 Final Exam Equations D H soln = -LatticeE + D H hydration K = ° C + 273.15 ° F = 9/5 ( ° C) + 32 d=m/V M 1 •V 1 =M 2 •V 2 ∆࠵? = ࠵? + ࠵? ∆࠵? = ࠵? ! ࠵? = ࠵?࠵? "! ∆࠵? ∆࠵? #$% ° = ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) − ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) ࠵? = ࠵? ( ࠵?࠵?࠵? ∆࠵? = ) !"# * ∆࠵? "+## = − ∆- * ∆࠵? .#/%" = ∆- $!%&’ * $!%&’ ∆࠵? +%01 = ∆࠵? "2" + ∆࠵? "+## ∆࠵? #$% ° = ∑ ࠵? ࠵? ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) − ∑ ࠵? ࠵? ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) D G = D H-T D S ∆࠵? #$% ° = ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) − ∑ ࠵? ∆࠵? ’ ° (࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?) Rate=k[A] m [B] n ࠵? 3/5 = 3 6[8] ( ࠵? 3/5 = [8] ( 56 ࠵? 3/5 = :.<=> 6 ln[࠵?] . = −࠵?࠵? + ln[࠵?] : 3 [8] $ = ࠵?࠵? + 3 [8] ( [ ࠵?] . = −࠵?࠵? + [࠵?] : [࠵?] . = [࠵?] : ࠵? ?6. ࠵? = ࠵?࠵? ? ) % *+ ࠵?࠵? 6 , 6 - = − @ % A E 3 * , − 3 * - F ln ࠵? = − @ % A 3 * + ln ࠵? ࠵?࠵? ! = − log ࠵? ! ࠵?࠵? = − log[࠵? " ࠵? # ] ࠵?࠵? = ࠵?࠵? $ + ࠵?࠵?࠵? [& — ] [(&] ࠵?࠵?࠵? = ࠵?࠵? ! + ࠵?࠵?࠵? [)( " ] [)] %࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵?࠵? = [( # * " ] $% [(&] &’&(&)* ࠵? 100% ∆࠵?° = −࠵?࠵?࠵?࠵?࠵? ࠵? +,-- ° = ࠵? +$/012, ° − ࠵? $312, ° or ࠵? +,-- ° = ࠵? 4,25+/613 ° + ࠵? 1762$/613 ° Units Conversions 1 m = 1.0936 yds 1 cm = 0.39370 inch 760 torr = 1 atm 1 inch = 2.54 cm 1 km = 0.621371 mile 760 mm Hg = 1 atm 1 Å = 10 -10 m 1 mL = 1 cm 3 101,325 Pa = 1 atm 1 kg = 2.2046 lbs 1 L = 10 -3 m 3 1.013 bar = 1 atm 1 lb = 453.59 g 1 gallon = 3.7854 L 1 Pa = 1 N/m 2 1 lb = 16 oz 1 quart = 0.94633 L 4.184 J = 1 cal 1 ton = 2000 lbs 1 mol = 6.022 X 10 23 4 qts = 1 gallon Constants R 0.08206 L•atm•K -1 •mol -1 8.314 J•K -1 •mol -1 h 6.626 x 10 -34 J•s k B 1.38 x 10 -23 J/K F 96,485 C/mol c 2.998 x 10 8 m/s C = k H P P solution = χ solvent P solvent o Δ T = K b m solute Δ T = K f m solute Π = MRT Δ T = iK f m solute Π = iMRT Δ T = iK b m solute K c = [ C ] c [ D ] d [ A ] a [ B ] b K p = p C c p D d p A a p B b K p = K c ( RT ) Δ n a x = x ⎡ ⎣ ⎤ ⎦ ° c a i = p i p ref x = − b ± b 2 − 4 ac 2 a K w = [H 3 O + ][OH — ] =[H + ][OH — ]= 1.0 x 10 -14 at 25 °C K a xK b = K w pK a = − log K a pOH = − log[ OH − ] pH + pOH = 14.00 = pK w

1 18 hydrogen 1 H 1.0079 2 Periodic Table of the Elements 13 14 15 16 17 helium 2 He 4.0026 lithium 3 Li 6.941 beryllium 4 Be 9.0122 boron 5 B 10.811 carbon 6 C 12.011 nitrogen 7 N 14.007 oxygen 8 O 15.999 fluorine 9 F 18.998 neon 10 Ne 20.180 sodium 11 Na 22.990 magnesium 12 Mg 24.305 3 4 5 6 7 8 9 10 11 12 aluminum 13 Al 26.982 silicon 14 Si 28.086 phosphorus 15 P 30.974 sulfur 16 S 32.065 chlorine 17 Cl 35.453 argon 18 Ar 39.948 potassium 19 K 39.098 calcium 20 Ca 40.078 scandium 21 Sc 44.956 titanium 22 Ti 47.867 vanadium 23 V 50.942 chromium 24 Cr 51.996 manganese 25 Mn 54.938 iron 26 Fe 55.845 cobalt 27 Co 58.933 nickel 28 Ni 58.693 copper 29 Cu 63.546 zinc 30 Zn 65.409 gallium 31 Ga 69.723 germanium 32 Ge 72.64 arsenic 33 As 74.922 selenium 34 Se 78.96 bromine 35 Br 79.904 krypton 36 Kr 83.80 Rubidium 37 Rb 85.468 strontium 38 Sr 87.62 yttrium 39 Y 88.906 zirconium 40 Zr 91.224 niobium 41 Nb 92.906 molybdenum 42 Mo 95.94 technetium 43 Tc [98] ruthenium 44 Ru 101.07 rhodium 45 Rh 102.91 palladium 46 Pd 106.42 silver 47 Ag 107.87 cadmium 48 Cd 112.41 indium 49 In 114.82 tin 50 Sn 118.71 antimony 51 Sb 121.76 tellurium 52 Te 127.60 iodine 53 I 126.90 xenon 54 Xe 131.29 Cesium 55 Cs 132.91 barium 56 Ba 137.33 lanthanum 57 La 138.91 hafnium 72 Hf 178.49 tantalum 73 Ta 180.95 tungsten 74 W 183.84 rhenium 75 Re 186.21 osmium 76 Os 190.23 iridium 77 Ir 192.22 platinum 78 Pt 195.08 gold 79 Au 196.97 mercury 80 Hg 200.59 thallium 81 Tl 204.38 lead 82 Pb 207.2 bismuth 83 Bi 208.98 polonium 84 Po [209] astatine 85 At [210] radon 86 Rn [222] Francium 87 Fr [223] radium 88 Ra [226] actinium 89 Ac [227] rutherfordium 104 Rf [261] dubnium 105 Db [262] seaborgium 106 Sg [266] bohrium 107 Bh [264] hassium 108 Hs [269] meitnerium 109 Mt [268] darmstadtium 110 Ds [271] roentgenium 111 Rg [272] ununbium 112 Uub [285] ununquadium 114 Uuq [289] cerium 58 Ce 140.12 praseodymium 59 Pr 140.91 neodymium 60 Nd 144.24 promethium 61 Pm [145] samarium 62 Sm 150.36 europium 63 Eu 151.96 gadolinium 64 Gd 157.25 terbium 65 Tb 158.93 dysprosium 66 Dy 162.50 holmium 67 Ho 164.93 erbium 68 Er 167.26 thulium 69 Tm 168.93 ytterbium 70 Yb 173.04 lutetium 71 Lu 174.97 thorium 90 Th 232.04 protactinium 91 Pa 231.04 uranium 92 U 238.03 neptunium 93 Np [237] plutonium 94 Pu [244] americium 95 Am [243] curium 96 Cm [247] berkelium 97 Bk [247] californium 98 Cf [251] einsteinium 99 Es [252] fermium 100 Fm [257] mendelevium 101 Md [258] nobelium 102 No [259] lawrencium 103 Lr [262] l

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4 Table 1. Acid Dissociation and Base Dissociation Equilibrium Constants at 25 °C. Name K a Name K b H 2 C 2 O 4 (Ka 1 ) 5.9 x 10 -2 Ethylamine (CH 3 CH 2 NH 2 ) 4.3 x 10 -4 HSO 4 – 1.2 x 10 -2 Methylamine (CH 3 NH 2 ) 4.4 x 10 -4 H 2 SO 3 (Ka 1 ) 1.2 x 10 -2 Dimethylamine [(CH 3 ) 2 NH] 5.9 x 10 -4 Chlorous acid (HClO 2 ) 1.1 x 10 -2 Diethylamine [(CH 3 CH 2 ) 2 NH] 8.6 x 10 -4 Citric acid (H 3 C 6 H 5 O 7 , Ka 1 ) 7.4 x 10 -3 Trimethylamine [(CH 3 ) 3 N] 7.4 x 10 -5 H 3 PO 4 (Ka 1 ) 7.2 x 10 -3 Ammonia (NH 3 ) 1.76 x 10 -5 Hydrofluoric acid (HF) 6.8 x 10 -4 Pyridine (C 5 H 5 N) 1.7 x 10 -9 Nitrous acid (HNO 2 ) 4.6 x 10 -4 Hydroxylamine (NH 2 OH) 6.6 x 10 -9 Cyanic acid (HCNO) 3.5 x 10 -4 Aniline (C 6 H 5 NH 2 ) 4.0 x 10 -10 Formic acid (HCOO H ) 1.8 x 10 -4 Lactic acid 1.4 x 10 -4 HC 2 O 4 – 6.4 x 10 -5 Benzoic acid (C 6 H 5 COO H ) 6.3 x 10 -5 Hydrazoic acid (HN 3 ) 1.9 x 10 -5 Acetic acid (CH 3 COO H ) 1.8 x 10 -5 Propanoic acid (CH 3 CH 2 COO H ) 1.3 x 10 -5 H 2 CO 3 (Ka 1 ) 4.2 x 10 -7 H 2 PO 4 – (Ka 2 ) 6.3 x 10 -8 HSO 3 – 6.2 x 10 -8 HClO 2.9 x 10 -8 HBrO 2.3 x 10 -9 HCO 3 — (Ka 2 ) 4.8 x 10 -11 HPO 4 2— (Ka 3 ) 4.2 x 10 -13 Table 2. Constants and Properties of Water. Solvent Boiling Point (°C) K b (°C/m) Freezing Point (•C) K f (°C/m) Water 100.0 0.512 0.0 1.86

5 Table 3. Solubility Product Constants at 25 °C. Compound Formula K sp Barium fluoride BaF 2 2.45 x 10 -5 Barium sulfate BaSO 4 1.07 x 10 -10 Calcium carbonate CaCO 3 4.96 x 10 -9 Calcium fluoride CaF 2 1.46 x 10 -10 Calcium hydroxide Ca(OH) 2 4.68 x 10 -6 Calcium sulfate CaSO 4 7.10 x 10 -5 Copper(II) sulfide CuS 1.27 x 10 -36 Iron(II) carbonate FeCO 3 3.07 x 10 -11 Iron(II) hydroxide Fe(OH) 2 4.87 x 10 -17 Iron(II) sulfide FeS 3.72 x 10 -19 Lead(II) chloride PbCl 2 1.17 x 10 -5 Lead(II) bromide PbBr 2 4.67 x 10 -6 Lead(II) sulfide PbS 9.04 x 10 -29 Magnesium carbonate MgCO 3 6.82 x 10 -6 Magnesium hydroxide Mg(OH) 2 2.0 x 10 -13 Silver chloride AgCl 1.77 x 10 -10 Silver chromate Ag 2 CrO 4 1.12 x 10 -12 Silver bromide AgBr 5.35 x 10 -13 Silver iodide AgI 8.51 x 10 -17 Barium chromate BaCrO 4 2.10 x 10 -10

6 Table 4. Standard Reduction Potentials in Aqueous Solution at 25 °C. Reduction Half-Reaction E°(V) F 2 ( g ) + 2 e − → 2 F - ( aq ) +2.87 Au + ( aq ) + e − → Au ( s ) +1.83 Co 3+ ( aq ) + e − → Co 2+ ( aq ) +1.82 H 2 O 2 (l) + 2 H + ( aq ) + 2 e − → 2 H 2 O ( l ) +1.78 Au 3+ ( aq ) + 3 e − → Au ( s ) +1.52 MnO 4 − ( aq ) → Mn 2+ ( aq ) unbalanced under acidic conditions +1.50 Cl 2 ( g ) + 2 e − → 2 Cl − ( aq ) +1.36 MnO 2 ( s ) → Mn 2+ ( aq ) unbalanced under acidic conditions +1.23 Pt 2+ ( aq ) + 2 e − → Pt ( s ) +1.20 Ag + ( aq ) + e − → Ag (s) +0.7994 Fe 3+ ( aq ) + e − → Fe 2+ ( aq ) +0.771 MnO 4 − ( aq ) → MnO 2 ( s ) unbalanced under basic conditions +0.59 I 2 (g) + 2 e − → 2 I − ( aq ) +0.535 Cu + ( aq ) + e − → Cu ( s ) +0.521 Cu 2+ ( aq ) + 2 e − → Cu ( s ) +0.337 2 H 3 O + (aq) + 2 e − → H 2 ( g ) + 2 H 2 O ( l ) 0.000 Fe 3+ ( aq ) + 3 e − → Fe ( s ) −0.036 Pb 2+ ( aq ) + 2 e − → Pb ( s ) −0.126 Sn 2+ ( aq ) + 2 e − → Sn ( s ) −0.1315 Ni 2+ ( aq ) + 2 e − → Ni ( s ) −0.25 Co 2+ ( aq ) + 2 e − → Co ( s ) −0.28 Cd 2+ ( aq ) + 2 e − → Cd ( s ) −0.40 Cr 3+ ( aq ) + e − → Cr 2+ ( aq ) −0.41 Fe 2+ ( aq ) + 2 e − → Fe ( s ) −0.44 Zn 2+ ( aq ) + 2 e − → Zn ( s ) −0.763 Cr 3+ ( aq ) + 3 e − → Cr ( s ) −0.74 Cr 2+ ( aq ) + 2 e − → Cr ( s ) −0.91 Mn 2+ ( aq ) + 2 e − → Mn ( s ) −1.18 V 2+ ( aq ) + 2 e − → V ( s ) −1.18 Zr 4+ ( aq ) + 4 e − → Zr ( s ) −1.53 Al 3+ ( aq ) + 3 e − → Al ( s ) −1.66 Mg 2+ ( aq ) + 2 e − → Mg ( s ) −2.356 Ba 2+ ( aq ) + 2 e − → Ba ( s ) −2.90

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10 CHE 132 Fall 2022 Final Exam Form 2B ____ 1. Choose the electron configuration for Fe 3+ ? A. [Ar]4s 2 3d 3 B. [Ar]3d 5 C. [Ar]4s 2 3d 5 D. [Ar]4s 2 3d 9 E. [Ar]4s 2 3d 6 ____ 2. Determine the chemical formula for the compound triammineaquaethylenediaminecobalt(III) chloride A. [Co(en) 3 ]Cl 3 B. [Co(NH 3 ) 3 (H 2 O)(en)]Cl 3 C. [Co(NH 3 ) 3 (H 2 O)(en)]Cl 2 D. [Co(H 2 O)(en) 3 ]Cl 3 E. [Co(H 2 O)(en) 3 ]Cl ____ 3. What is the oxidation state of Fe in K 3 [Fe(CN) 6 ]? A. 1 B. 2 C. 3 D. 6 E. 3-

11 ____ 4. If the overall rate of reaction is 8.0 x 10 -2 M/s, what is d[NH 3 ]/dt for the following reaction 4 ࠵?࠵? > (࠵?) + 5 ࠵? 5 (࠵?) 4 ࠵?࠵?(࠵?) + ࠵?(࠵?) A. –32 x 10 -2 M/s B. 32 x 10 -2 M/s C. 8.0 x 10 -2 M/s D. –4.0 x 10 -2 M/s E. 4.0 x 10 -2 M/s ____ 5. For a given reaction, the rate law is given by the following equation. What is the reaction order in NH 3 , O 2 and overall, respectively? ࠵?࠵?࠵?࠵? = ࠵?[࠵?࠵? > ] 5 [࠵? 5 ] A. 2, 1, 1 B. 1, 1, 2 C. 0, 2, 2 D. 1, 2, 1.5 E. 2, 1, 3 ____ 6. For the following reaction, calculate the ∆࠵? "2" ° ( B C•EFG ) . 4 ࠵?࠵? > (࠵?) + 5 ࠵? 5 (࠵?) → 4 ࠵?࠵?(࠵?) + 6 ࠵? 5 ࠵? (࠵?) A. 825.48 B. –200 C. 132.48 D. –675 E. 1.37

12 ____ 7. Glucose (C 6 H 12 O 6 ; 10.00 g) was dissolved in 100.0 g of water to a final volume of 115 mL. The density of a 10% by mass glucose solution is 103.75 g/mL. Calculate the molality of glucose in the solution (mol/kg). Molar mass glucose = 180.1559 g/mol A. 0.4652 B. 0.004652 C. 0.2921 D. 0.4826 E. 0.5551 For Problem #8 and #9, consider the following electrochemical cell: Pt( s )| Pt 2+ ( aq ) || Cr 3+ (aq), Cr 2+ ( aq )| Pt( s ) ____ 8. What is the coefficient in front of the Cr 3+ in the balanced chemical equation under aqueous acidic conditions? A. 1 B. 2 C. 3 D. 4 E. 6 ____ 9. What is E ° cell (V)? Put the value with appropriate significant figures in the Answer 9 blank.

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13 ____ 10. Which intermolecular interaction is predominant between ethylacetate (CH 3 COOCH 2 CH 3 ) and ethanol (CH 3 CH 2 OH)? A. dipole-induced dipole B. dipole-dipole C. dispersion D. hydrogen bond E. ion-dipole ____ 11. Rust consists of a number of different iron oxides. The equations below show an example rusting process. For the second reaction, which of the following is the correct K expression? A. ࠵? I = [- . ] [JK ,. ][L , ] B. ࠵? I = [- . ] / [JK ,. ] 0 [L , ] C. ࠵? I = MJK ,. N 0 [L , ] [- . ] / D. ࠵? I = [JK , L 1 •- , L][- . ] / [JK ,. ] 0 [L , ][- , L] 2 E. ࠵? I = MJK ,. N 0 [L , ][- , L] 2 [JK , L 1 •- , L] , [- . ] / ____ 12. A student places 25.0 mL of HCl in an Erlenmeyer flask and adds indicator. She then adds 12.35 mL of standardized 1.002 M NaOH until her indicator turns slightly pink. What is pH of the solution? A. pH < 1.00 B. pH <7 C. 7 D. pH > 7 E. This can’t be determined without knowing the concentration of NaOH. (1) (2)

14 ____ 13. Which is most soluble ionic compound in aqueous solution at 25 °C? A. CaF 2 B. FeCO 3 C. Ag 2 CrO 4 D. CaSO 4 E. PbS ____ 14. Consider a 1.0 M HBr aqueous solution. At equilibrium, what is the concentration of HBr? A. 0.0 M B. 0.5 M C. 1.0 M D. 2.0 M E. not enough information. ____ 15. What is the pOH of a 0.015 M aqueous solution of Sr(OH) 2 ? A. 13.18 B. 12.18 C. 0.82 D. 1.52 E. 1.82

15 ____16. The amino acid histidine (H 3 C 6 H 8 N 3 O 2 ) is a polyprotic acid with three protons and is titrated with NaOH. Given that the pKa’s of the protons in aqueous solution at 25 °C are as follows: pK a1 = 1.82 pK a2 = 6.04 pK a3 = 9.17 How many equivalents of NaOH will need to be added in the titration to find when the pH = pK a3 ? A. 1.0 B. 1.5 C. 2.0 D. 2.5 E. 3.0 ____ 17. If you want to find the pH of a 0.100 M aqueous solution of CH 3 NH 2 , which reaction would you write for the ICE table? A. base dissociation equation for CH 3 NH 2 B. acid dissociation equation for CH 3 NH 2 C. acid dissociation equation for CH 3 NH 3 + D. reaction of OH – and water E. water reacting with water For problems 18-21, consider the information below. Suppose a 500.0 mL flask is filled with 2.1 moles H 2 (g), 0.50 moles F 2 (g) and 1.0 mole HF(g) and they react via the following reaction. ____ 18. Which statement is TRUE? A. The reaction is at equilibrium. B. The Q<K and therefore the reaction will shift to the right. C. The Q<K and therefore the reaction will shift to the left. D. The Q>K and therefore the reaction will shift to the right. E. The Q>K and therefore the reaction will shift to the left. H 2 (g) + F 2 (g) 2 HF(g) K = 1.15 x 10 2 at 400 °C

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16 For problems 19-21, consider the information below. Suppose a 500.0 mL flask is filled with 2.1 moles H 2 (g), 0.50 moles F 2 (g) and 1.0 mole HF(g) and they react via the following reaction. ____ 19. In the ICE Table, what is the equilibrium algebraic expression for [HF]? A. 1.0 + 2x B. 1.0 – 2x C. 2.0 + 2x D. 1.0 + x E. 2.0 – 2x ____ 20. In the quadratic equation, what are a , b and c ? Put the values in the Answer 20 blanks with 2 sig figs. ____ 21. What is the equilibrium concentration of [HF]? Put the value with appropriate units in the Answer 21 blank with 2 sig figs. H 2 (g) + F 2 (g) 2 HF(g) K = 1.15 x 10 2 at 400 °C

17 ____ 22. Below is a proposed mechanism for ClO – (aq) reacting with I – (aq) in the presence of OH – (aq) . You are trying to show that the rate law for this proposed mechanism matches an experimentally determined one. What is the expression for k overall or k’ for the proposed mechanism? Note : When writing an expression, H 2 O is not involved (just don’t include it). A. ࠵? O = 6 - 6 3- B. ࠵? O = 6 - 6 , 6 3- C. ࠵? O = ࠵? 5 D. ࠵? O = 6 3- 6 - 6 , E. ࠵? O = 6 - P 6 , 6 3- ____ 23. Which reaction coordinate diagram best fits the proposed mechanism for I – oxidation by ClO – ? A. B. C. D. E.

18 ___ 24. The reaction in Question 22 was run at a higher temperatures. At 65.0 °C, the rate constant was measured to be 0.986 M -1 •s -1 and at 100.0 °C, it was 2.304 M -1 •s -1 . What is E a ( kJ/mol )? Give your answer in the Answer 24 blank with 3 significant figures. ____ 25. Microwave plasma can be employed to decontaminate vegetative bacteria, yeast and some endospores packed in Tyvek. When examining the gas identities and kinetics, the following reaction was examined, where NO• is an NO gas molecule with an unpaired electron (a radical, •). 2 NO• (g) + O 2 (g) ⇌ 2 NO 2 (g) A plot of 1/[NO•] vs. time results in a straight line where k= 5.00 M -1 •s -1 . If the initial concentration of NO• is 2.00 × 10 -3 M, how long (seconds) will it take for the concentration of NO• to reach 1.00 x 10 -3 M? Give your answer in the Answer 25 blank with 3 significant figures.

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19 Consider the titration of aqueous solution of 20.00 mL of 1.35 M Propanoic acid (CH 3 CH 2 COOH ) in a 100 mL Erlenmeyer flask with 1.002 M KOH for Problems 26 and 27. ____ 26. After 15.00 mL of KOH is added to the Erlenmeyer flask, what is the pH of the solution? Place your answer with the correct number of significant figures in the Answer 26 blank. ____ 27. After 30.00 mL of KOH is added to the Erlenmeyer flask, what is the pH of the solution? Place your answer with the correct number of significant figures in the Answer 27 blank.

20 ____28. Cellulose is found naturally in structures such as trees and can be made into paper. To determine the molecular weight of a cellulose sample the osmotic pressure was determined. Cellulose (300.0 g) was dissolved in the solvent N,N -Dimethylacetamine/lithium chloride (DMAc/LiCl) to a final volume of 800.0 mL. The osmotic pressure of the sample was determined to be 0.602 atm at 25.0 °C. What is the average molar mass (g/mol) of the student’s cellulose sample? Place your answer with the correct number of significant figures in the Answer 28 blank.