Problem Set 5 - Chem 208, Spring 2008 Name: Problem Set 5...

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Unformatted text preview: Chem 208, Spring 2008 Name: Problem Set 5 Due Friday, March 7, 2:00 PM SOLU'TYOU F Lab TA Name: Lab Day: Supplementary Problems: Ch 15 # 7, ll, 13, 15, 17, 29, 31, 33, 37, 39, 51 1. The equilibrium constants in terms of pressure (in atmospheres) were determined at 1123 K: 2c0 (g) <2 C(s) + C02 (3) C0(g) + (:1; (g) <=> COClz (g) Kp=7.7x10"5 Kp’=6.0x10'3 a) What is the equilibrium constant for the following reaction at 1 123 K? C(s) + C02(g) + 2C12 (g) <3 2coc12 (g) K,” = . C6) “302 (7) :3 2606a) I’fo = 53:73:: ZCO@)+2C/&(g) :3 ZCOC/LQ; Kr, =(gflxr/0"i£ Co) + COJrJ+ZCQw fiZCOC/a (/0 = 471109 b) The equilibrium constant for the reaction in part a) (above) is 4.32 x 104 at 600 K. Is this reaction endothermic or exothermic? Explain. Crud/A (fist/€425}? 7—- fno’ofiermk “race (I) decree; c) Consider a mixture of C(s), C03(g), Clg(g), and COClg(g) at equilibrium at 600 K. If the following changes are made, will the equilibrium shift to the left, to the right, or remain unchanged? In each case, explain your answer in no more than one sentence: 1. The total volume,V is decreased. E7W%gflE/H Afi. Ilka: Q cl;'{:é;r:uq (hm/J95 3mo/Eijsqt‘2‘ 2010/42.) 1qu‘. y J‘Igyflé'rtaj r"! ( m/méef" 07D (34; mo/ecv/EJ c/ecneasar‘ ii. Some C(s) is added. U0 SKI/ICE no7L affearh ,Zqfi e tyres-5 for-t “gr <0 ‘ iii. Some Cl (g)i added. "‘~ , . . 2 s éfw/ our” :Axfififiv 7% 0‘747‘ 7% COM,“ (/49) iv. Some helium (He) is added, causing the total pressure to increase. 72H“; fias A/o eflQC'?! Jinfe ’4‘; 041691;»?! aflC-cy/gargj [aren‘t/res“ 01: green: flf/ecf.‘/\7 In KP €K/rflff£um Chem 208, Spring 2008 Problem Set 5 Due Friday, March T, 2:00 PM 2. For the reaction of hydrogen with iodine to produce hydrogen iodide, Kc = 56.0 at 435°C. a) What is the value of Kp? ,5 __ HA7) +1219) “— 2 41(7) (13:54.0 (>4 4 o 4 = 2g (167”) 7 ’2 42/67) = Kc. . ‘. A7,: 5‘6. 0 b) Suppose you mix 0.45 mol of H2 and 0.45 mol of I; in a 10.0 L flask at 425°C. What is the partial pressure of each component in the mixture before and after equilibrium is reached? #zeW-Taw #Z/ijf- £1137— Ini‘i’(q‘i‘M) 2,93 25-3» 0 :(p.«5m/)fi:.oa m, (0‘55) W m4 Equal.) 25H 2sM 2”“ = 2.58% = 21L 2... 2 "PH: H (ZRL :5; P P ’P _ 25‘3—"0L H"— Iz— C Q-Lifi’x11‘l-30 2" = (S: :"H? (y x=2.03 "A P _ P : 2_S_8-2,03).ri‘m 2": 7H8(ZISQ-Rj _/ H), IL:(O.§SQ+M =— 1‘150 '7‘E3‘K P 3. Boric acid and glycerin form a complex: - LLOQ crim. HIE ‘ B(OH)3(aq) + glycerin (aq) (I) B(OH)3 - glycerin (aq) with an equilibrium constant of 0.90. If the concentration of boric acid is initially 0.10M, how much glycerin should be added so that in a total volume of 1.0 L, 60% of the boric acid is in the form of a complex? B(OHi31“il‘1°' F‘— B{0H)5-5I«,c ini’r (m) 6.10 X 0 aka Cm.) - 0-0L ~0-Oe 0. 0L. — Eqim (m) O-Okf- X-OOL, 009 [Word "iii-“)3 o. 0 C. = = .—._._—-—-—3-'—-—'-' : Z KC {BM} :1 [4361 (9.0%)(2g—9.06) Lofiomoo‘t) \ Angcfldoadop A'i—efim) {W} LOM L3:— fifmles M“? man Chem 208, Spring 2008 Problem Set 5 Due Friday, March 3’, 2:00 PM 4. The steam reforming of methane is an important industrial process: onus) + H20(g) -~—-— C0(g) + 3H2(g) K,: = 0.260 at 1200K a) A student mixes 1.00 mole of CH4 with 1.00 mole of H20 in a 1.0L flask at 1200K, and allows the reaction to come to equilibrium. What are the equilibrium concentrations of each component, in molest? CHqLo11+HLOfil # COLQMBHLGI KC: O-ZLO INHM) 1.0 to O O Ckfiimi -)< ~2< ram +3X git-Aim) 1.0 ‘K '0‘): X 3K 1' Kc: ECOJEHapflP: CK)(3K)5 _ ijfi : O. ZLO A-Lei‘m'. [CHQEHLOJ Q—0 ‘9‘); (Lo-KY“ ,_ q x 1 0ch # Ii [COJ=0.ZI?M Uta-x)" 7'7 x: [113032—52 57/‘7 x’“ ,._ case 2 amt/o” ~1 m“ 1.0-yr m fl 1""1 XL: 9.37x/0_&*9.S>/fi/O x 2 21%. -r “ b) You evacuate a 1.0 L flask, and then add 1.00 mole of CO(g). How many moles of H2 would you need to add to the flask so that at equilibrium, 0.70 moles of the CO(g) has reacted? ini‘i‘ (Ni 1.0 2: O 0 ch] (M) “0'7 “1'1 +03 +07 Erin [Mi 0'3 Kfiz'l 3: £0312“ = OHZKi (X'Z '3 (0.9835) x—z.) = Wakes = 0-75 2C: 2 85 Chem 208, Spring 2008 Problem Set 5 Due Friday, March 7, 2:00 PM 5. You are a member of a team of chemists discussing plans to operate an ammonia processing plant: N2(g) + 3H2(g) <3 2NH3(E) The plant operates at close to 700 K, where KP = 1.00 x 10‘4 for the reaction. The synthesis employs the stoichiometric 1:3 ratio of N2:H2. At equilibrium, the partial pressure of NH; is 500 atm. Calculate the partial pressures of each reactant, and the initial and equilibrium Pm. Nag) ’f‘ 3442(3] : 2 U#3(cj] ini‘i’ Pacing >C 3’: o ij (at) ~25 ~45 +50 Eqim(r~'l1—) 325—75 L L KP -.~ 3% :. Ioomo"l PM; H: (KEEN (aw—7g) 7 SO 3 2.50 x/O (X " 27 x -23 = W 2 3/0 X: s; lat-.4943 : PM; = at, aer Mails“ PM: SC-ZS=BI«+w PH = IL'B‘a—lm- Pub 1 Manama 1 PT” 121%“qu PMg ; So ail—M H 3 .4: ,9 4. 3 PM ...
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This note was uploaded on 04/16/2008 for the course CHEM 2080 taught by Professor Davis,f during the Spring '07 term at Cornell University (Engineering School).

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Problem Set 5 - Chem 208, Spring 2008 Name: Problem Set 5...

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