Chemistry 185 Exam #2 - A November 5, Lab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
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1 Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this exam. 3. Use the spaces provided to write down your answers. To receive full credit, you must show all work. Do not write answers on any other pieces of paper. If you need more room, write on the back of the exam and be sure to include a note describing where the work is located. 4. When solving numerical problems, make sure you include the proper units in your final answer. 5. If a question asks for a response in sentence or paragraph form, make sure you respond in that format. 6. Useful data for the exam and a periodic table are provided on the last page of the exam. Carefully tear out these sheets if you wish. Page # Points possible Points awarded Page # Points possible Points awarded MC Total 100 1
2 Multiple Choice Unless otherwise directed, choose the single best answer for each question. Please use the space provided to do your calculations. Make sure your answers have the proper number of significant figures. 1. Use the given information to calculate the equilibrium constant for the reaction below. H 2 CO 3 (aq) + 2NH 3 (aq) 2NH 4 + (aq) + CO 3 2- (aq) K =? Given H 2 CO 3 (aq) + 2H 2 O(l) 2H 3 O + (aq) + CO 2-3 (aq) K = 2.1x10-17 NH + 4 (aq) + H 2 O(l) H 3 O + (aq) + NH 3 (aq) K = 5.6x10-10 a.) 1.2x10-26 b.) 3.8x10-8 c.) 2.7x10 7 d.) 6.7x10 1 e.) None of the above. 2. The reaction shown below occurs at 25. At the beginning of the reaction the [N 2 ] = M, the [H 2 ] = M, and the [NH 3 ] = M. As the reaction progresses towards equilibrium, which way does the reaction shift and what happens to the equilibrium constant? 2NH 3 (g) N 2 (g) + 3H 2 (g) K = 16.6 a.) The reaction will shift right and K increases. b.) The reaction will shift left and K decreases. c.) The reaction will shift right and K remains constant. d.) The reaction will shift left and K remains constant e.) The reaction will shift left and K increases. 3. Which of the following would you expect to be the most acidic? a.) AgClO 4 (aq) b.) Be(ClO 4 ) 2 (aq) c.) NaClO 4 (aq) d.) Ti(ClO 4 ) 3 (aq) e.) None of the above is acidic. 2
3 4. a.) Next to the soluble ionic compounds listed below, indicate whether they will produce an acidic, basic, or neutral solution in water. If the compound is acidic or basic, also write a balanced chemical equation showing how the compound reacts in water on the line provided. If it is acidic or basic, calculate or write the Ka or Kb of the compound in the space just below the formula. (10 points) LiHSO 4 KCN b.) If moles of each compound were added to a separate beaker of deionized water, which solution would have the biggest change in ph? (3 points) 5. A sample of Co(OH) 2 (s) is added to a container of deionized water and allowed to reach equilibrium. Co(OH) 2 (s) Co 2+ (aq) + 2OH - (aq) H > 0 a.) If this system is initially at equilibrium, in what direction will it shift in each of the following cases? (9 points) i.) Co 2+ is removed. ii.) NaOH(aq) is added. iii.) The temperature is increased. b.) The mass of Co(OH) 2 at equilibrium is g. When KCl(aq) is added to the equilibrium mixture, the magnitude of the equilibrium constant doesn t change but the mass of Co(OH) 2 at equilibrium drops to g. Explain why the mass drops. (5 points) 3
4 6. The following mechanism has been proposed for the reaction between nitric oxide and bromine. Step 1 NO(g) + Br 2 (g) NOBr 2 (g) slow Step 2 NOBr 2 (g) + NO NOBr(g) + NOBr(g) fast In the space below, draw the reaction profile for the mechanism. The overall reaction is exothermic. Identify the intermediate(s) and place them where they should appear, label any transition state(s) (as T.S.), and use an arrow to identify the magnitude of the activation energy for the overall reaction. (9 points) 7. How would the addition of a catalyst change the diagram above? (3 points) 8. At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen. 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) When the rate of formation of NO 2 is 3.8x10-4 M/s, what is the rate of change in the N 2 O 5 concentration? (4 points) 4
5 The next problem continues on the following page. 9. A solution containing HBr(aq) has a ph equal to a.) What is the poh? (3 points) b.) What is the [H 3 O + ] in this solution? (4 points) c.) A solid sample of bromoacetic acid (CH 2 BrCOOH) is dissolved in 1.00 L of the above solution. If the sample contained 0.60 moles of bromoacetic acid, construct the ICE table that would allow you to calculate the ph of the mixture of HBr and bromoacetic acid. Assume the volume of the solution does not change. For simplicity, represent bromoacetic acid as HA. You do not need to solve anything, just set up the ICE table. (7 points) d.) Using the information from the ICE table, substitute the appropriate terms into the equilibrium constant expression. You do not need to solve the equation, just plug in the appropriate terms. (3 points) e.) What is the H 3 O + concentration of a neutral solution at a temperature of 25? (3 points) 5
6 f.) Use the information from the previous page to answer this question. What is the ph of the mixture of HBr and bromoacetic acid. You will have to make some assumptions to solve this problem. Clearly state your assumptions and check your assumptions when you are finished. Do not use the quadratic equation to solve this problem. (5 points) 10. The reaction shown below is an elementary reaction. Other than the presence of a catalyst, list as many things as you can think of that will affect the rate of the reaction. You do not need to write a sentence, just make a list. (4 points) NO 3 (g) + CO(g) NO 2 (g) + CO 2 (g) 6
7 11. The balanced chemical equation for the decomposition of A is: 3A(g) 2B(g) + C(g) a.) The concentration of A was monitored as a function of time. When 1/[A] was plotted as a function of time the relationship was linear and is shown to the right. What is the rate law for this reaction and what are the units of k? (5 points) b.) If the initial concentration of A is 1.00 mol/l, how long will it take for 85% of A to go away? (8 points) c.) The following mechanism has been proposed for the reaction above. Based on the rate law from part a, which step must be the slow step? In order to get full credit, you must show how the mechanism gives you the experimentally derived rate law. (5 points) Step 1 Step 2 Step 3 A D D + A 3B A + B C 7
8 12. The Lewis structures and Ka values for HNO 2 and HNO 3 are shown below. Ka = 7.2x10-4 Ka = 2.4x10 1 It has been suggested that the strength of an acid is primarily dependent on the properties of its conjugate base. Use Lewis structures and words to explain what it is about the conjugate bases of HNO 2 and HNO 3 that accounts for the difference in acid strength. (4 points) 8
9 Periodic Table and Other Useful Information Avogadro s Number: x particles/mole Formula Ka Dalton s Law: P A = χ A x P tot H 2 SO 4 1.0x HSO 4 1.1x10-2 Integrated Rate Laws: [A] t = -kt + [A] 0 HCN 6.2x10-10 CH 2 BrCOOH 1.3x10-3 ln[a] t = -kt + ln[a] 0 Temperature conversion: Ideal Gas Law: Arrhenius Equation: 1 = kt + 1 [A] t [A] 0 T [K] = T [ C] PV = nrt k = Ae Ea RT Kw 1.0x10-14 The common strong bases are the soluble ionic compounds with OH -. The following will form soluble ionic compounds with OH - : Group I metals, calcium, strontium, and barium -1 Gas constant R: J mol -1 K L atm K 1 mol 1 1 atmosphere: 760 torr (unlimited s.f.) 1 H Li Na K Rb Cs Fr (223) 4 Be Mg Ca Sr Ba Ra Sc Y La Ac Ti Zr Hf Rf (261) 23 V Nb Ta Db (262) 24 Cr Mo W Sg (263) 25 Mn Tc (98) 75 Re Bh (262) 26 Fe Ru Os Hs (265) 27 Co Rh Ir Mt (266) 28 Ni Pd Pt Ds (269) 29 Cu Ag Au Rg (272) 30 Zn Cd Hg Cn (277) 5 B Al Ga In Tl Uut 6 C Si Ge Sn Pb Fl (289) 7 N P As Sb Bi Uup 8 O S Se Te Po (209) 116 Lv (293) 9 F Cl Br I At (210) 117 Uus 2 He Ne Ar Kr Xe Rn (222) 118 Uuo 58 Ce Th Pr Pa Nd U Pm (145) 93 Np (237) 62 Sm Pu (244) 63 Eu Am (243) 64 Gd Cm (247) 65 Tb Bk (247) 66 Dy Cf (251) 67 Ho Es (252) 68 Er Fm (257) 69 Tm Md (258) 70 Yb No (259) 71 Lu Lr (260) 9
Lab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
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