Quiz 2 Key - _ . . _-1__ —— Chem 111B Quiz 2 ' Feb; 22,...

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Unformatted text preview: _ . . _-1__ —— Chem 111B Quiz 2 ' Feb; 22, 2010 Sh 0w all work. 1. The equilibrium constant KBq for a certain reaction will change if changes. ' a. pressure b. time 0. volume temperature reactant concentrations 2. What is the relationship of the equilibrium constants for the following two reactions? (1) 2 Nona H N204(g); _ (2) N2041g) H 2 Noun 3... Keq of reaction (1) is the reciprocal of Keg of reaction (2). b. Keg of reaction (2) is the reciprocal of Kml of reaction (1) c. Keq of reaction (1) '== KW of reaction (2) Answers A and B are both correot There is no relationship between the Keqs of these reactions 3. What is the correct equilibrium constant expression for the following reaction? 2 curs) + 02(g) “r 2 (3110(5) ' " a. Iocq = 1/[02]2 b. K‘2;.:1'=[Cu0]2/[Cu]2 0. KW = [CuO]2/[Cu]2[02] 4. general rule helps predict the shift in direction of an equilibrium reaction? Le Chatelier's principle Haber process 0.. Equilibrium constant d. Bosch theory Chem 111B Quiz2 5. Consider the reaction: C02(g) + H2(g) H C0(g) + HgO-(g), for which K.: = 0.64 at 900 K. Ifthe initial C02 and of H2 are each 0.100 M, what will be the-equilibrium concentrations of each species after the reaction reaches equilibrium? a. [00;] = 0.044 M; [Hg] = 0.044M; [CO] = 0.056 M; [H20] = 0.056 M [C02] = 0.056 M; [Hg] = 0.056 M; [CO] = 0.044 M; [HgO] = 0.044 M c. [00;] = 0.020 M; [Hg] = 0.020 M; [CO] = 0.080 M; [HZO] = 0.030 M d. [00;] = 0.030 M; [Hg] = 0.030 M; [CO] = 0.020 M; [1-120] = 0.020 M e. None of the above '4' I i' 1 fffiifi" _ 'i I I! fr“ 5:! w I {:i a I; .a' “'f‘“ I if: r I {I}: a: -- '- "' “" I f, ,~, .- { 2.- a i‘" F; r Fm. I. 3 a “2%- ” ., 2?. r WM 4 {y}; I * -— :- Ifl- :fi;a It i {E 1.. g"? E ._ E .- . fr i. I I It. I {1 if" g... i if“! t. ~ 1.; mi T E if. _ Zim- __._.Il iii-1‘ i -- If“; gr 6. At somelemramrenthe reaction: 3 C10" H C103' + 2 C1" has an equilibrium i 3 i - i + - . yr" “#1:- r la # constan K.3 = 3 .2 X 10 .lf the components of this reaction are nnxed such that the1r ; 5:3 initial cesaéfiifatiSiis [C1] = 0.05 M; [C103] = 0.32; and [ClO'] = 0.74, is the mixture at equilibrium, yes or no? If the mixture is not at equilibrium in which direction, left to right or right to left, will reaction occur so that the mixture can reach equilibrium? 3. There is not enough information given to answer this question b. Yes, the mixture is at equilibrium nOW Feb. 22, 2010 uh: I. m" “'13:?” .1! F” 3 fly . r; I . . _- mam “rm : . fl} ,3”... q N0. Left to fight a; C if Wang... (HP! “fig. I U In I ’5‘ . .-- I M}, k“d. No. Rrght to left . - (if {13 ,2 are"; i J ‘3’, ‘ “‘21 i .. * {30 a M J ' i” g a ,gwwflwmmmmhmq.,_._nl_m=__fimvww hum .,—..-a f if. _- f f / -. F *1 ' ‘” L” in! b f - j firiwmmmhmwmfimmb hmfiflre' %=....,. " 7. Consider the following endothermic reaction: H2(g) + 12(g) H 2 HI(g). If the temperature is increased, more HI will be produced b. ' some HI will decompose, forming H2 and I; c. the magnitude of the equilibrium constant will decrease d. the pressure in the container will increase e. the pressure in the container will decrease ChemlllB ' Quizz Feb. 22, 2010 ' I 3. Consider the following reaction at equilibrium: N02(g) .+ C0(g) <——> N0(g) + C02(g). Suppose the volume of the system is decreased at constant temperature, What change will this cause in the system? a. A shift to produce more N0 b. A shift to produce more CO C. A shift to produce more N02 No shift will occur 9. Consider the reaction that describes the Haber process for the production of ammonia (NHg): N2(g) + 3 H2(g) <-> 2 3%) for which K; at 300 0C is 9.5. Calculate KP for this ' 0 . '— , reactlon at 300 C. a; .1 ~— r t W I. 3—?- a: 3 _'.'£ __.-r I - itl' H ..r-' .u-H'I a. hill ii. “in. f‘u .- -- EEK. .r'“ :""in I, .1 '- ‘ Hf i “ii Ii 1 :-"-"".‘I__'_,...-=fl""’rf ' .h. ' iv "" ' "‘-" "' ' . in” -' 'i “i i r? h? 1-: Cf ii: - x '3 ' i" t“ J ‘ R a“: K _"' 4 3 3 ’5 ‘“ p l -.-:-n- l. c KP == 2 1 X 10' r-r .. H J“ :- . "‘2 .7: ix. r“ J 1H F r 1“ F~_ fr d KP —— 1.6 x 10 "“ H- t 10. The following equilibrium constants have been determined for oxalic acid at 250 C: H2C204 4% H+ + H0204' K; = 6.5 x 10'2 HC204— ""1""— H+ + C204} Kc” : X 10-5 What is the equilibrium constant for the following reaction at the same temperature (textbook problem 14.30): H2C204 -——=--—......__2H+ + C2042“ - - .-r' E1 . \ 2 'i E ... . E a " #11 h; 5' 11‘ E are" «:4!!! Hg 1 f: -. New... '5 1; 1-- id” K “*1... a“ I F a in; :l, i L... 4“." ‘1...“- I E 6...; um m. I; u. 1... . j" a f .._ r .. u i r n J {i‘ i? In}: " "W " .a' w #- 2 i L . if? :5 Z. a!“ 1., ...
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This note was uploaded on 10/05/2011 for the course CHEM 1B taught by Professor Hagopian during the Summer '06 term at Irvine Valley College.

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Quiz 2 Key - _ . . _-1__ —— Chem 111B Quiz 2 ' Feb; 22,...

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