Final08 - Final Exam Chemistry 112 808 Name: Last four...

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Unformatted text preview: Final Exam Chemistry 112 808 Name: Last four digits of SSN: { Each probiem is worth 10 points. Show all your work 1 Circle the final answer! pH should be given with two decimal accuracy! Remember unitSE! 1 2 3. 4 5 6 7 8. 9 10 11. 12. 1.3. 14. 15. 16. 17. 18. 19. 20. Compute freezing temperature of 5% soéution of CaBrg, assuming ideal behavior of this mixture. Kfof water is 1.86 0C kg/rmfi, MW of CaBrg : 200.0 g/moi. Freezing temperature of pure water is O 0C. 2. Compuw solubility (maximum concentrazion) in water of nitrogen gas at partial pressure of 60 torr, if its solubility at' partial pressure of 360 torr is 2.64x10'4 1m. 3. The equilibrium constant KP for the gas phase reaction. C0 + 1’12 «a CHgO is Kp = 5.6 am."1 at 300 “C. a. Calculate Kc for the reaction C0 + H3 <w—> CHgO b. Calculate KC for the reaction ZCHQO H 2C0 + 2H2. (2. Calculate the equilibrium pressure of CO if P(H2):0.5 aim, P(CH20)=3 atm. 4. A 20 L container is filicd wiih 0.15 mol of NOBr, ihcn sealed. NOBr than dccomposcs according to ZNOBr(g) <—+ 2N0(g) + Brig). The equilibrium concentration of Br; is 2.0 MG3 M. Compute Kc. 5. Will Ihe precipitate form if 100 mi, of 0.1 M H2804 solution are added to EOO mL (3.2 M AgNO3 solution? The Ksp of silver sulfate AggSO4, is 1.2 X 10": M3. 6. A water soiution contains 0‘526g of hemoglobin in 20.0 mL of solution has an osmotic pressure of 7.51 torr at 25 0C. What is the moiar mass of hemoglobin? 7. Calcuiate the pH of a mixture of 100 mL of 0.1 M of HCl with 200 ml, of 0.02 M OfHOCl. Ka(HOCl):3.0x1 0‘8. 8. The pH of a 0.2 M soiution of cyanic acid HCNO is 2.09. Calculate Ka for HCNO. 9. Calculate the pH of a mixture of 20 mL of 0.1 M Ca(OH)2 and 30 mL-of 0.2 M 0fHC104. 10—12. Caicuiate the pH in the titration of 20 mL of 0.1 M HCN (Ka = 7.2x10““3) with 0.2 M LiOH after 5 mL ofLiOH have been added 10 mL of LiOH have been added 15 mL of LiOH have been added. 13. How many kJ of work is rcquired to compress 360 L of hydrogen gas, initially at 2 atm, Linden" an external} pressure of 90 aim. Assume the ideal gas behavior. 14. A cataiyst décomposes methane via first order rate law, with methane half—fife of 2><10'2 5. How long should-methane be in contact with the catalyst to reduce its concentration 150 times? 15. Use {he experimental initiai rate data to determine the rate law and the rate constant for the gas—phase reaction H1 ~§~ CZHSI ——> C2 H6 + 12. Whai.‘ are {he unizs of rate constant? Experiment } Initial concentration, M ' Iniiéal raée 3 {HI} [021351] «A[12]/(At), NUS 3 3 \ 0.053 0.23 1 1.85x10‘5 2 \ 0106 R23 1 7. 4Ox10T ' 3 06106 | 0.46 4 3.453le 4 0.212 | 0.46 2 5.9236104 16. Determine rate constant and order of reaction from the concentratiomtime dependence given below. What is the rate of this rsaction at 500 s ? L Time, S N | [R.eacta11t}, M 7 [ 0M \ 20000 | j 20 i_1.0976 J g 50 0.44626 \ E u 120 } 0054647 300 \ 2.4682 x10"4 17. A reacfion rate quadruples when the temperaiure increases from 10°C to 30°C. What is the activation energy? 18. For the following reaction determine the oxidation states of all species on both the reactant and the product side and state which Species is being oxidized and which species is being reduced 2— _ PHMg)+ €104 (aq) “’ C1‘02 foq) "t 134(3) 19. Use the ion—electron method to balance the oxidation and the reduction half—reaction, anal then balance the overall reaction in acid solution. 20. Compute equilibrium constant at siandard conditions for the reaction + 2+ 03(5) “Em Ag (HQ) "’ Cu (m) + Ago) ‘ Rxn E°(V) CUZqu) “H26- “‘-> (311(5) Ag+(aq) +5 "m’ Ago) +0.80 Extra credit: (15 points). A voltaie cell works in aqueous soéution according to the eel] reacticn ZU(OH)2(S) +14%) —-> Li+(aq) + 211(3) + OH'(aq). Balance the reaction and compute cell voltage at 298 K when {LHZOJ M, pH=1 1.00 using the data: ' Rxn BOW) Lam) +5 —+ Lim 6.045 Zn(OH)2(-S) + 26— —+ 211(5) +2 (DH-(m1). "1 .250 Henry’s Law: C m H” Raoult’s Law: Psolvcm= 13°30le - XSDMM Boiling Point Eie-vation: ATE * kBm M : moms m 3 “30165 L k g Freezing Point Depression: ATF E Rpm. Osmotic Pressure: H = MRT 760 Torr : 1 atm R =3 0.0821 L'atm/mol-K R m 8.314 J/mol°K m4 .L ~~CCDd _[CCDd aA+bB .m— 00 . 01D Kequ Q nfiagb KP == KC(RT)A” ay2+by+c=0 y: [HAT] [01‘1"] m i x 10"4 2 kW PH "4“ pOH fl 14 = pkw * ~10g[H3O+] [H304] m 10-pI-I pOIAI.==¥10g[OI-I”] [OH‘] = mm m [£1.3O+][AW] Ra _ k [31$]ij [HA1 ' b x [B] kakb 2 kw pica + pica x pkw - n‘b Cb pH : pKa + h)ng pKa +10g fla ' Ca W = —PAV J L' aim = 101.3 J qsm = CAT qsm = —q5y5m AB = q + w AM 2 AE + PAV ‘ AH = AE + AnRT AG = AH — TAS AG m AGO + RTan AGO = —RTinKeq Kaq w 5W“ _ ASO m AHO 3‘1 " R RT 111K . . _WA[A]__A[B]_ MCL MD] mew aAt m bAt _+ cAt “Jr CIA: rate w 1<[A]X[B]> $21513?) """""""" "mi—Iii]; """""""""""""" " £52151} """" "‘[Iéi’lfijflé """"""""""""""""" " 1n[A] m 1n[A]o m kt rm 3 0.693/k Late m l<[A]2 if] = if]; t k2 R T1 T2 1 V m 1 J/C AGO m ~nFE° 1F 4—: 96,485 C/mol 6— At 298 K: ED 2 0.025678 1n Keg 0.0:913 10g Keq ’ E 2 EO_ 0.02:67SIH Q 2 EO_ 0.0291310g Q. ...
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Final08 - Final Exam Chemistry 112 808 Name: Last four...

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