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L_622478_2009-05-28 - CHE 1113 TEST II DR POWELL WRRCH ‘...

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Unformatted text preview: CHE 1113 TEST II DR. POWELL WRRCH ‘ 7, 2008 Please print your name on both the test paper and the Scan Tron form. SECTION1. MULTIPLE CHOICE (7 points each). The decomposition of calcium carbonate has a AH = 556 kJ: “(1110\3 SWSXDW We CaC03(s) H 2002(9) + Ca0(s) Consider this system at equilibrium. What would happen to the value of Ko if the temperature was decreased? a) Kc would not change. b KC would increase. would decrease lmpossible to determine without the numerical value of Kc. J A particular reaction has units for the rate constant of M‘2 3“. What is the overall order for the . reaction? a) o b) 1 c) 2 @3 e) -1 The decomposition of dinitrogen pentaoxide has AH° m, = + 55kJ. The activation energy for the reverse reaction is 47 kJ/mol. What is the activation energy feethedecompesition of—R ,¥_- dinitrogen pentaoxide? a. 27 kJ/mol b. 33 kJ/mol c. 55 kJ/mol d. 47 kJ/mol @102 kJ/mol The following reaction is used to produce nitrogen gas from ammonia: 4 NH3(g) + 3 02(9) —+ 2 MG) + 6 H20(9) If the rate of formation of water is 3.90 M min", what is the rate of disappearance of ammonia? a) @390Mmh'E‘tl’y : ‘L wmfl Ll 0. 60 M min' c) 5.85Mmin1 l’\L= 9 [9.0 d) 1.95 M min'1 e) lndeterrninate When a chemical system is at equilibrium, a the concentrations of the reactants are equal to the concentrations of the products. he concentrations of the reactants and products have reached constant values. c) the fowvard and reverse reactions have stopped. d) the reaction quotient, Q, has reached a maximum. e) the rate constants of the forward and reverse reactions are equal. PAGE 2 SECTION 2. PROBLEMS (10 points each). 6. Sulfur dioxide and oxygen are mixed in a container of fixed volume at 1000 K. Their initial concentrations are 0.0600 M and 0.0500 M, respectively. When the reaction has come to equilibrium the concentration of 803(9) was 0.0400 M. What is the value of Kc for this reaction? . . 1; 2302(9)+029) H 2803(9) CO”) = «00“ A a) 0.00250 1 .00 ‘0 O (099 £05 b) 4.23 C - .90, _,ou Q . «3 E .th9~ 4 .O\ :0\-‘r\ e) 66.7 _3 :0 . lb -9\6 \ Um +9“ 19% ? 7. Kc = 32.0 for the reaction ZBrCl (g) H Brz (g) + CI2 (g) _ 6 1.40 x 10'3 mol of BrCI is placed in a 1.0 — L flask and the reaction occurs. WhAf @1190 = $14- concentration of-BFSI at equilibrium 3~BrU e €(9 7\ CA8 Q (3 O U .. ~a _ —. ,ont I L‘ a) 0.00140 M I, \ of 1x *3 y- leb ' b) 7.56x104M W - ‘ 6.43 x 10“ M 100% - 7.11 x 10“ M e) 7.00 x 10“ M 8. The following data were obtained for the reaction: 20102 (aq) + 20H'--> C|03'(aq) + 0102- (aq) + H20 (I) Exgeriment |C|O_2 | | OH ' | initial rate (M/s) 1 0.0500 M 0.100 M 5.75 x 10‘2 2 _ .100M 0.100M [2.30x10‘1 3 0.100M 0.0500M 1.15x10'1 What is the rate law for the reaction? a) rate = k[Cl02] [ OH ']-1 b) rate = k[Cl02]2[ OH '12 c) rate = k[Cl02] [OH '12 d) rate = k[Cl02] [OH '] rate = k[Cl02]2[ OH '] ANSWER THE FOLLOWING QUESTIONS ON THE TEST PAPER 1. Kc for the following reaction is 1.58 x 10‘8 at 523 K. Calculate Kp. (5 points) (R = .0821 L atm/mol K) NHZCOONH4(S) H 2NH3(g) + C02(g) \C?‘ [a {TAR PAGE 3 2. An equilibrium mixture for the reaction below contains 0.0602 mol iodine monochloride, and 0.0199 mol each of chlorine and iodine. An additional 0.0200 mol of lCl is added to the mixture. What is the concentration of all species after equilibrium is reeestablished? (15 points) m Z'CKQ) H '2(9) "' CI2(9) I Y. .0000 .0001 .01qu C —.OQOO +.Q\ +.O\ 5— 0109 .0910 .0904 WCoaOaBCOM“) 3.010 1110‘” 3. The reaction 2 NO (9) + 2 H2 (9) —> N2 (9) + 2 H20 (9) gives the following initial rates at high temperature: X1 2/ Experiment [NO] (mgllL) [Hg] (moi/L) initial rate (Mls) \Ig 1 / 1 0.420 0.122 0.124 ' 2 4 0.210 0.122 0.0310 , 4 0.105 0.488 0.0310 Determine the rate of this reaction for an experiment where [N0] = 0.450 M and [H2] = 0.161 M. (15 points) 7 9 X .lQH __— ‘49’0 Y .0099 : \Qqq WM: \[email protected](63 DER) ~9lO .oao “Tb—3’ ...
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