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Practice Test 3 Key - CE“ 3Y3“(Prairwacst'r 3"K7...

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Unformatted text preview: CE“ 3Y3“ (Prairwacst'r 3 "K7 JWUUU l /"\ l. (30 points) Answer the following questions concerning the Deacon process (once used for making chlorine), using the thermochemical data given in the table below (all values relate to stande ambient temperature, 298 K, and 1 bar pressure) 2Hc1(g) + ‘1/2 02<g) :2 H20(g> + c12<g) gas AH; (kJ/mole) AG; (kJ/mole) S398 (J/mole K) / HCl —92 —95 187 H20 —242 —229 189 C12 0 0 223 02 0 0 205 A a) Determine AHggg and AS398 for the production of one mole of C12(g) by the above reaction. Attack; 162452 km) + o — (266:2 temp—go) ._ {my/met W A“? 1’52? k7 430.. width» A5024? ‘ Wc‘ 3.4+ 223 ‘ 20373 ” licmg : -4Lflb’fima 1?? we; Oh if «’7 K AsonY : “4%.; 32k} 1Q” makim; W kw‘QQCdx b) Assuming AH° and AS° for the reaction to be independent of temperature, determine Kf at 900 K. — -3 0:- —_ eL/rzr)/o/J) ACQoo 537/212 @00 k7( I/érw‘i ( /~T Student Name V21: Student PID No. Section No. c) Ifone mole each of HCl, 02, C12, and H20 are placed in a 5.0 L container at 900 K, in which direction will the reaction proceed to reach equilibrium? (Assume all Kyl’ gases behave ideally.) Cow K erL “C?“ 09‘ \lea 0-9— lfiP exocrcSSKM w/in/‘fmf 4mm}: ‘ ‘«+ In I . ComWV’ Kw ; cei- movie) :5 : .m 1 (515% M \/ @3310an l“r Q0: i' 50L — V L033 LEE-300K - 0'2; I MK (904 K 5 reao‘ilam. Pmceeols waci {-1) 9.73%)?” (1) Given the initial conditions of part (c), determine the mole fiactions of all four components at equilibrium. (Assume that the change in moles of 02 in reaching equilibrium can be neglected in the calculation.) o 4 v" (“0.4; 90‘an RT ,1 mew a“. __, (”@291“ng \’ 335: (HEY w Q—zg)‘ n“; l+§= 1.2% [Age [+2 “GEMS: /.7. H“ mm; His (9" [Ar-3m: 21+; “Linkage Me = 991$ M 0.10 r g Student Name ‘5 g i Student PID No. Section No. 4 e) Calculate AG for the mixing process at equilibrium. \r 52m = m [2: xii" xi] 1 33' y (Roma [£0.3ifik(03|$ll Jr Oxide/0'5) + 0.23 £10353] (£an “8(400143 2 -zo)o>27 VJ; 2. (25 points) a) An ideal solution is prepared by mixing three moles of acetone with 2 moles of diethyl ether at 303K. The vapor pressure of pure acetone at 303K is 0.39 bar and the vapor pressure of pure diethyl ether at this temperature is 0.78 bar. What is the vapor pressure of the solution? 5 a. 3‘ “' l ‘ Xamrpaua «L Xbfiaan “3 (.3451. (0.3% 23 + QM” yon? 0 3NW 57%? (P : O,S‘§l§m. P: 0.5/5— Aw b) If the solution is sealed in a can that is initially evacuated and allowed to come to equilibrium. What are the mole fractions of acetone and diethyl ether in the vapor at 303K. = f— 0H3 affé (10(quth raw (0.1aoX. 39993 - Yacetone = @ 17’; Ydiethyl ether = 0 .57 Student Name lg a: 1: Student PID No. Section No. (20 Points) Answer the following questions, given the data for NH3 listed below: AHvap = 23.4 kJ/mole AHfus = 5.7 kJ/mole density of 1i uid = 1.33 cm3 density of so 'd = 0.89 cm3 normal fi'eezing temperature = 195 K a) The vapor pressure of pure liquid NH3 at 205 K is 100 mm Hg. Estimate the boiling temperature of the liquid in a pressure cooker where the pressure above the liquid is maintained at 5 atm. (1 atm = 760 mm Hg, MNH3 = 17 g/mole) F‘: '00 Niall“? PL: §R+M~7éofiyififit 3YOOAA’4} @m T? Q0514 A<£>L'AHMP(_L_ L> R 12 7‘1 T, La<3300> 1 'SZBJL/MWMQ (J, , J, > “T f" T 20‘" N gar/KM L ~ .L- 1 —§ -/i£l2)(lo k-l ‘ TL ZOS‘L _ l ‘3 mouth $53M; a" — I ‘1 Lyhli’S Student Name k c, Student PID No. K“ SectionNo. b) What is the temperature of an equilibrium mixture of NH3 solid and liquid at 100 atm external pressure? (Assume that the densities and AH data given above are independent of temperature.) ‘7 1).," [DO (L'i'w. ‘ 1; 0 file. AM» ’ 2 l‘: lq+u~ 5T‘3 [45" 0LT TAV T 71 I ’ - - I - / I A - V ~ v — W _,_- .- dw New 41 £3 “0/: AV T T» —. l7; 4.. - ,l_ 3 1“. rue» ”3%; 373/3 1 ._ 3 m. — ms am 4 an a: r» m 7' ”‘ A' = —(,31><:o‘3_L__ F wwoc I’Ooatwlmn {700% $1 ‘é Sine-3m +3 ‘4 T -—/.o‘iwo Law 1 A (/ 3’ (15’ “(toixm’VMau , 8-“ $47 a j" J/ ,0?2 Mm “,Oiitxgm(/7:L ”SMl'L‘ [‘l 3'! ‘ l omits . ', O! l 7; = (Mr/A e "v {/62}? /< ( A Student Name Ii ( ‘ Student PID No. r\ Section No. 4. (25 Points) a) A vapor pressure curve for C02(g) dissolved in water at 274 K is shown below. If a bottle containing such a solution is sealed and placed under a C02 pressure of 10.0 bars, at what temperature will it freeze? (Assume that the solution is semi— ideal and that AHfus = 6.0 kJ/mole, M1420 = 18 g/mole.) ><COL K00; (PCDL ’r \O x _ [(10 lanes ' . 1 0. a C07” L/fl. 6M5 S, A *— [0 *1 AT? — 671,204?” ‘m 1000? H441 fili— X01 » x/mfl 973/57 (035») 1 “259K #5 I _ 7,, 7‘? : 273/?(‘ 258M 2 [‘70 ”Jelly? aflmr‘ msea’ " '- 2352M ...
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