2c - my 2 «- c l. (5 pts) For the reaction and rate law...

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Unformatted text preview: my 2 «- c l. (5 pts) For the reaction and rate law given below, which of the statements is true? 5. (7 ms) The reaction CHrNC to CHTCN which we used in class to illustrate transition 2 state theory is a first order reaction. At 230°C, k was determined to be 6.29 x 10" see“. A + 2 B + 2 C _) 3 D + 2 E Rate = klA] [B] If the initial concentration of CH3-NC, [CH3-NC10, is 0.0575 M, what is the final . . . concentration of [CH3—NC10 afier 10 minutes? a) Doubling [B] wrll increase the rate by a factor of four. b) Tripling [C] will increase the rate by a factor of nine. a) 0_00575 M c) Doubling [A] will increase the rate by a factor of four. b) 00137 M d) Tripling [C] will decrease the rate by a factor of three. ' c) 0.0215 M \e) Tripling [B] will increase the rate by a factor of nine. d) 0.0394 M e) 0.0520 M The following rate data were obtained for the reaction of hemoglobin (Hb) and carbon monoxide (CO). 4 Hb + 3 C0 "" Hb4(co)3 6. (7 pts) The second order rate constant for a reaction is 0.013 M's". A 0.250 L _ reactor is charged with 1.5 mol of reactant. How many seconds will it take for the M Rate 0f Hb d1“ em“ Sec amount of reactant to drop to 0.950 mol? 1.00 x 10 ' 2.25 x10‘ 6.47 x 10 mm— a) 55 see b) 42sec c) 23 see 2. (6 pts) The order of the reaction with respect to hemoglobin (Hb) is d) 14 sec e) 7.4 see a) 0 b) 1/2 c) 1 d) 2 7. (5 pts) The following graph illustrates the relationship between concentration and c) 3 . ' time for the chemical reaction 2X -‘ Y. The slope of this line is equal to 3. (6 pts) The order of the reaction with respect to carbon monoxide (CO) is = \ . a) l/k ln[X] a) 0 b) -k b) 1/2 c) ln[X]o c) l / d) -1/k d) 2 e) k time e) 3 ‘ 8. (6 pts). The decomposition of N205(g)§is a first order process with a rate constant of 4. (6 pts) The rate law for the following reaction is rate = k[NO][Hz]2. What are the 6.82 x 10" sec‘I at 70°C. A reactor of volume 3.25 L was filled with 0.795 mol of units of the rate constant? N205. What is the half-life (minutes) of N205 at 70°C? 2NO+2H29N2+2H20 a) M see" a) 0.693 minutes b) (M)2 sec'l b) 1.69 minutes c) (M)'2 sec'l e) 2.44 minutes (1) (M)3 sec“ d) 5.75 minutes e) (M)'3 sec" e) 9.56 minutes M524. 0,? q 9- ( 5 Pts) WhiCh Statement is false? 13. (6 pts) The first order rate constant for the hydrolysis of a particular organic compound in water increases with temperature. A plot of In R vs III gives a straight line with slope equal to -2.9 x 10‘. What is the activation energy, E. (kJ/mol)? t R = 8.314 J/mol a) The central idea of the collision model is that molecules must collide to react. lb) The energy of the collision and the orientation of the molecules at collision determine whether a reaction will occur in the collision model. c Temperature affects the rate constant as there are more collisions and each collision is a) 2 4 x 105 Ulmol more energetic. ' 1 4k” 1 d) All collisions that have sufficient energy lead to reaction. i 133 HIE; e) The activation energy is the minimum energy necessary to achieve a chemical d) 2‘4 x 102 kmnol ‘W‘m' e) 2.9 x 102 kJ/mol ‘10. (5 pts) For the uncatalyzed decomposition of H202(aq) to form H200) and 02(3), the activation energy and overall AE are 75.3 kJ/mol and 98.1 kJ/mol, respectively. What is the activation energy for the reverse reaction? 14. (5 pts) A catalyst increases reaction rate a) -22.8 kJ/mol b) -75.3 kJ/mol a) by decreasing the heat of the reaction 0) 22.8 kJ/mol ’ b) by lowering the activation energy of the forward reaction only. (1) -173.4 kJ/mol c) by increasing the activation energy of the reverse reaction. c) 173 .4 kJ/mol d) by an alternative pathway with a lower activation energy e) by supplying additional energy for the heat of reaction. 1 l. (6 pts) The activation energy, El, is a first order reaction is 155 lei/moi. The rate constant at 137.o°c is 8.325 x 10‘3 soc". What is the rate constant (s") at 247.0%? 15. (5 pts) At equilibrium R = 8.314 mm K . " a) 6.71x 106 a) All chemical processes have ceased. b) 4.91 x 105 , I b) The rate of the forward reaction equals the rate of the reverse reaction. ct) 1-24 X 102 c) The rate constant for the forward reaction equals the rate constant of the. reverse (I) 7.91 x 103 reaction. 6) 3.5611106 d) K=(k¢)(k.) .-., e) K = W 16. (6 pts) Calculate the equilibrium/constant for the following reaction at 500°C given the following equilibrium concentrations: ‘ 12. (6 pts) The reaction 2 N0 + 02 -' 2 N02 is believed to occur according to the ' [CE] = 0.855 M; {I128} = 0.225 M; [C82] 1= 0.685 M; [H2] = 0.375 M. following mechanism. What would be the rate expression? , ' s ' CS:($)"'432(3) ‘3 Cflttg)+2H25_(g) Mechanism: NO + 02 S M); (fast) N0‘3- + N0 —~ 2N0; (slow) a) 3.20 b) 0.749 a) rate=k[N0][02] c) 0.169 b) rate=k[N031[Oz] d) 5.93 c) rate=k[NO] [Oz]2 . e) 1.74 d.) rate = k[NO]2[021 e) rate = k[NO][Oz] 17. (7 pts) The equilibrium constant for the following reaction is 70 at 350°C. At equilibrium, concentrations of 0.500 M N; and 0.175 M H2 were measured. What is equilibrium concentration of NH3? N2(g) + 3 H209 ’5 2 NHa(g) a) 0.17 b) 0.43 c) 0.69 d) 0.74 e) 0.87 18. (6 pts) The Kc for the following reaction at 350°C is 66.9. Given the concentrations for H; of 0.0362 M, I; of 0.0818 M and HI of 0.645 M, you can conclude H2(g)+12(g) ‘5 2 HHS) a) The concentration of H1 will decrease to reach equilibrium. b) Equal amounts of products and reactants are present at equlibrium. c) The system is at equilibrium. d) The reaction will proceed to the right to reach equilibrium. e) The concentration of Hz will increase to reach equilibrium. 19. (6 pts) The equilibrium constant K, for the following reaction at 2127 K is 2.5 x 10". What is Kc? R = 0.08206 L atm/mol K mm) + 02(g) ‘5 2 N0(g) a) 2.5x10'3 b) 4.4x10'1 c) 1.4::10‘s d) 5.2x10‘ e) 6.1::10‘2 20. (7 pts) The equilibrium constant for the following reaction is 7.0 at 400 K. If 0.45 mol of Br; and 0.45 mol of C12 are introduced into a 1.00 L container at 400 K, what will be the equilibrium concentration of BrCl? a) 0.90M b) 0.26M c) 0.71M d) 0.45M e) 0.51M Br; (g) + c12(g) S i Brcmg) 0 21. (7 pts) The following reaction has 3 KC = 1.80. If a 0.060 M solution of PC15 is placed in the reactor and allowed to reach equilibrium, what is the equilibrium concentration of PC13? {This is a more challenging problem, so return to it if you have time) a) 0.058 M b) 0.042 M c) 0.036 M d) 0.018 M e) 0.012 M PC1504) 3 C120!!!) + PC13(3€D 22. (6 pts) Which of the following procedures will maximize product formation? 9999.“.— 2 802(3) + 02(3) 3-7 2_ 803(8) AH < 0 02(g) is added to the system. ' The reaction mixture is heated. The volume of the reaction vessel is doubled. A catalyst is added to the mixture. The total pressure of the system is increased by adding a noble gas 803(3) is removed fi’om the system. a)l,2,4,6 b)l,4,5,6 c)2,3,5 d)2,3 e)1,6 23. (5 ‘pts) Consider the following reactions at equilibrium. Determine which of the indicated changes will cause the reaction to proceed to the right. 1) C0(g) + 3 H2(g) ‘3 CH4(g) + H20(g) (remove H20) 2) N2(g) + 3 H2(g) 17» 2 W304) (add NHs) 3) H2(g) + Ms) S 2 HF(g) (add HF) 4) N2(g) + 2 02(g) 1: 2 N02(g) (remove N02) 5) Ba0(s) + 803(g) 1: BaSO4(s) (add 3:20) a) 2, 3, 5 b) 3, 4 c) 1, 4 d) 2,3 c) 1,3 24. (5 pts) Consider the following reactions at equilibrium. In which cases will the reaction proceed more to the lefi by decreasing the pressure? 1)CO(g) + 3 Hz(g) ‘5‘ CH4(g) + H20(g) 2) C02(g) + C(s) ‘-'~ 2C0(g) - 3) N2(g) + 3 Me) ‘-'> 2NH3(g) 4)2C02(g) S 2C0(:g) + 02(g) 5)C0(g) + 2H2(g) =3 CH30H(g) a)2 b) 1,5 c)2,4 d) 1,3,5 e)1,3 25. (6 pts) Consider the following reaction at equilibrium. The yield of 00(3) in the reaction can be maximized by carrying out the reaction: 2c02(g) s: 2 C0(g) + 02( g) AH" = -514 1d a) in the presence of solid carbon. b) at low temperature and high pressure c) at low temperature and low pressure d) at high temperature and low pressure e) at high temperature and high pressure 26. (6 pts) At equilibrium in a 1.00 liter container were present 0.750M H2(g), 0.750 M Mg) and 3.54 MyHI(g;). An additional amount of 0.500 mol HI was added. What is the value of Q and in which direction does the reaction proceed to reestablish equilibrium? H2(g)+12(g) 1'» 2HI(g) a) 18 left b) 20 right c) 23 [ch d) 26 right e) 29 lefi 27. (5 pts) Which ofthe following is not a strong acid?) 3) KC] b) stot c)HF more, e) H0104 28. (5 pts) Which of the following is not a strong base? a) KOH b) NH; 0) 38(0H)2 d) NaQH e) Ca(OH)2 29. (5 pts) What is the pH of a 2.05 x 10" M aqueous solution of the strong acid l-IBr? a) 1.562 b) 2.256 c) 2.942 d) 3.345 e) 3.688 30. (6 pts) What is the pH of a 0.382 M aqueous solution of the strong base Ca(OH);? a) 13.88%) H.582 c) 7.00 d) 0.418 e) 0.117 ...
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This note was uploaded on 07/17/2008 for the course CHEM 122 taught by Professor Zellmer during the Winter '07 term at Ohio State.

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2c - my 2 «- c l. (5 pts) For the reaction and rate law...

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