Practice Final Exam. Important points:

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1 Practice Final Exam Important points: The format of this practice exam is different than is the format for the Spring Final. All questions on the Spring 2007 final will be multiple choice questions. The material covered on the practice exam is a subset of the possible questions and does NOT cover all of the possible questions for the upcoming 2007 final. If you are unable to answer one specific question on this practice exam, that represents a whole class of questions or a volume of material that you should refresh. In preparing for the final exam, you are strongly encouraged to utilize the following resources: Study guides for exams 1 3. Posted practice exams 1 3. This semester s exam 1 3. This semester s quizzes (available from 178 website: homework assignments. lecture notes & examples worked in lecture notes. Sample & Practice exercises embedded in the text. The most effective way to prepare for the exam is to answer questions and perform problems. To test your knowledge you need to actively engage and go through the thought processes. Simply reading solutions to problems and answers to questions is completely ineffective. (Watching a 10 K race is not a beneficial way to prepare for running a 10 K race.)

2 1. (3pts) If the units for rate are Ms -1, what are the units for the rate constant, k, if the overall order of the reaction is three? A) s -1 B) M 2 s -1 C) M -1 s -1 D) M -2 s -1 E) M 1 s (2pts) Which of the following statements is false regarding the equilibrium constant, K c? A) K c for a reaction at a particular temperature always has the same value. B) K c for the reverse reaction is the negative of K c for the forward reaction. C) The numerical value of K c depends on the form of the balanced equation. D) When quoting K c it is customary to omit units. 3. (3pts) The activation energy for the reaction O + O 3 2O 2 is 25 kj/mol, and the enthalpy change is H = -388 kj/mol. What is the activation energy for the decomposition of O 2 by the reverse reaction? A) 413 kj/mol B) 388 kj/mol C) 363 kj/mol D) 25 kj/mol E) -363 kj/mol 4. (2pts) The rate law for the reaction H 2 O 2 + 2H + + 2I - I 2 + 2H 2 O is rate=k[h 2 O 2 ][I - ]. The following mechanism has been suggested. H 2 O 2 + I - HOI + OH - slow OH - + H + H 2 O fast HOI + H + + I - I 2 + 2H 2 O fast Identify all intermediates in this proposed reaction mechanism. A) H + and I - B) H + and HOI C) HOI and OH - D) H + E) H 2 O and OH - 1

3 5. (4pts) The equilibrium constant is equal to 5.00 at 1300K for the reaction: 2SO 2 (g) + O 2 (g) 2SO 3 (g) If initial concentrations are [SO 2 ]=1.20M, [O 2 ]=0.55M, and [SO 3 ]=1.80M, the system is A) at equilibrium B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state D) not at equilibrium and will shift to the right to achieve an equilibrium state E) there is insufficient information provided to answer the question 6. (2pts) Which statement is true for the general rate law: Rate = k[a] m [B] n? A) It can be written from the stoichiometry of the overall reaction. B) The overall order of the reaction is equal to m times n. C) The values for the exponents must be determined by experiment. D) The exponents in the rate law must be positive integers. E) None of the above statements are true. 7. (3pts) A certain electrochemical cell has the following overall reaction: Zn + HgO ZnO + Hg Which is the half-reaction occurring at the anode? A) HgO + 2e - Hg + O 2- B) Zn e - Zn C) Zn Zn e - D) ZnO + 2e - Zn 8. (3pts) The overall reaction for photosynthesis can be represented by the following equation: 6CO 2 (g) + 6H 2 O(l) C 6 H 12 O 6 (s) + 6O 2 (g) The enthalpy change for this reaction is 2802 kj. Which of the following changes in condition will shift the equilibrium to the right? A) increase the pressure of O 2 (g) B) increase the temperature C) remove CO 2 (g) by reaction with CaO(s) D) remove one-half of C 6 H 12 O 6 (s) E) none of the above will shift the equilibrium to the right 2

4 9. (2pts) Which of the following statements is false? A) A catalyst increases the rate of the forward reaction, but does not alter the reverse rate. B) A catalyst alters the mechanism of the reaction. C) A catalyst alters the activation energy. D) A catalyst may be altered during the reaction, but is always regenerated. E) A catalyst increases the rate of reaction, but is not consumed. 10. (4pts) If K c = for the reaction: 2HBr(g) H 2 (g) + Br 2 (g), what is the value of K c for the reaction: ½H 2 (g) + ½Br 2 (g) HBr(g)? A) B) C) 3.77 D) 28.4 E) (3pts) Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant is Concentration (M) A B Time (min) A) K c < 1 B) K c = 0 C) K c = 1 D) K c > 1 E) K c = -1 3

5 12. (2pts) What is the approximate ph of a solution X that gives the following responses with the indicators shown? A) B) C) D) E) Indicators HIn-In - ph range Solution X methyl orange red-yellow yellow methyl red red-yellow yellow bromthymol blue yellow-blue green phenolphthalein colorless-pink colorless 13. (2pts) Which of the following is least able to behave as a Lewis base? A) CH 3 NH 2 B) (CH 3 ) 2 NH C) (CH 3 ) 3 N D) (CH 3 ) 3 NH (4pts) What is the ph of a 0.100M NH 3 solution that has K b = ? The equation for the dissociation of NH 3 is NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH - (aq) A) 1.87 B) 2.87 C) D) (2pts) Which of the following salts, when dissolved in water, produces the solution with the highest ph? A) KI B) KBr C) KCl D) KF 4

6 16. (4pts) A solution with a hydrogen ion concentration of M is and has a hydroxide concentration of. A) acidic, M B) acidic, M C) basic, M D) basic, M 17. (3pts) During an electrochemical reaction, electrons move through the external circuit toward the and positive ions in the cell move toward the. A) anode, anode B) anode, cathode C) cathode, anode D) cathode, cathode 18. (3pts) What is the [CH 3 CO 2 - ]/[CH 3 CO 2 H] ratio necessary to make a buffer solution with a ph of 4.44? K a = for CH 3 CO 2 H. A) 0.50 : 1.0 B) 0.94 : 1.0 C) 1.1 : 1.0 D) 2.0 : (2pts) What is the expression for the equilibrium constant for the dissociation of formic acid in water? HCOOH(aq) + H 2 O(l) H 3 O + (aq) + HCOO - (aq) A) B) C) K K K c c c + [H 3O ][HCOO ] = [HCOOH][H O] [HCOOH][H 2O] = + [H O ][HCOO ] 3 [HCOOH] = + [H O ][HCOO 3 2 ] D) K c [H = 3 O + ][HCOO [HCOOH] ] 5

7 20. (3pts) The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(ii) oxide HgO(s) Hg(l) + ½O 2 (g), H = kj/mol. Estimate the temperature at which this reaction will become spontaneous under standard state conditions. S (Hg) = J/molK S (O 2 ) = J/molK S (HgO) = J/molK A) 108K B) 430K C) 620K D) 775K E) 840K 21. (3pts) If an equal number of moles of the weak acid CH 3 CO 2 H and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral? A) acidic B) basic C) neutral D) there is insufficient information provided to answer the question 22. (2pts) Which of the following sets of compounds is not characteristic of a buffer? A) NaH 2 PO 4 with Na 2 HPO 4 B) NH 3 with NH 4 Cl C) CH 3 CO 2 H with NaCH 3 CO 2 D) HNO 3 with NaNO 3 E) all of the above are characteristic of a buffer 23. (3pts) Which of the following titrations results in a basic solution at the equivalence point? A) HI titrated with NaCH 3 CO 2 B) HOCl titrated with NaOH C) HBr titrated with KOH D) Pb(NO 3 ) 2 titrated with NaI 6

8 24. (2pts) What is the most soluble salt in the following set? A) Ba(OH) 2 with K sp = B) Ca(OH) 2 with K sp = C) Cd(OH) 2 with K sp = D) Fe(OH) 2 with K sp = (2pts) What is the common ion in a solution prepared by mixing 0.10M NaCH 3 CO 2 with 0.10M CH 3 CO 2 H? A) H 3 O + B) CH 3 CO 2 - C) CH 3 CO 2 H D) H 2 O 26. (2pts) Consider the following standard reduction potentials in acid solution: E (V) Al e - Al AgBr + e - Ag + Br Sn e - Sn Fe 3+ + e - Fe The strongest reducing agent among those shown above is A) Fe 3+ B) Fe 2+ C) Br - D) Al 3+ E) Al 27. (3pts) Arrange the following substances in order of increasing entropy at 25 C. HF(g), NaF(s), SiF 4 (g), SiH 4 (g), Al(s) A) SiF 4 (g) < SiH 4 (g) < NaF(s) < HF(g) < Al(s) B) HF(g) < Al(s) < NaF(s) < SiF 4 (g) < SiH 4 (g) C) Al(s) < NaF(s) < HF(g) < SiH 4 (g) < SiF 4 (g) D) Al(s) < HF(g) < NaF(s) < SiF 4 (g) < SiH 4 (g) E) NaF(s) < Al(s) < HF(g) < SiF 4 (g) < SiH 4 (g) 7

9 28. (2pts) A salt bridge is used to A) provide reactants in a fuel cell B) determine the direction of the cell reaction C) control whether the cell is electrolytic or voltaic D) allow the ion flow necessary for cell neutrality 29. (2pts) Which of the following statements about positrons is false? A) The positron has the same mass as an electron. B) A positron is ejected from the nucleus during the conversion of a proton into a neutron. C) A positron is a positive electron. D) When positron emission occurs, the atomic number of the nucleus increases. 30. (3pts) Which of the following processes are accompanied by an increase in entropy? 1. I 2 (s) I 2 (g) 2. H 2 O(l) H 2 O(s) 3. 2NH 3 (g) N 2 (g) + 3H 2 (g) 4. Mg 2+ (aq) + 2OH - (aq) Mg(OH) 2 (s) A) 1,2 B) 1,3 C) 3,4 D) 3 E) 2,4 31. (3pts) The overall reaction 2Co 3+ (aq) + 2Cl - (aq) 2Co 2+ (aq) + Cl 2 (g) has the standard cell voltage of E = 0.46V. cell Given that Cl 2 (g) + 2e - 2Cl - (aq), E = 1.36V, Calculate the standard reduction potential for the following the half reaction at 25 C: A) 1.82V B) -0.90V C) 0.90V D) -1.82V E) -1.36V Co 3+ + e - Co 2+ 8

10 32. (5pts) Calculate the K sp for silver sulfate if the solubility of Ag 2 SO 4 in pure water is 4.5 g/l. A) M B) M C) M D) M 33. (3pts) What is the percent dissociation of acetic acid if the solution has a ph = 4.74 and a pka = 4.47? A) 100% B) 50% C) 10% D) 1% 34. (2pts) As a result of beta decay, the product nucleus is A) one atomic number lower than the original element B) two atomic numbers higher than the original element C) one atomic number higher than the original element D) two atomic numbers lower than the original element 35. (3pts) Using the following standard reduction potentials Fe 3+ (aq) + e - Fe 2+ (aq) E = +0.77V Pb 2+ (aq) + 2e - Pb(s) E = -0.13V Calculate the standard cell potential for the voltaic cell reaction given below and determine whether or not this reaction is spontaneous under standard conditions. Pb 2+ (aq) + 2Fe 2+ (aq) 2Fe 3+ (aq) + Pb(s) A) E = -0.90V, nonspontaneous B) E = -0.90V, spontaneous C) E = +0.90V, nonspontaneous D) E = +0.90V, spontaneous 9

11 36. (3pts) A radioisotope decays to give an alpha particle and 208 Pb. What was the original element? A) Se B) Bi C) Po D) Hg E) Rn 37. (2pts) The reaction rates of many spontaneous reactions are actually very slow. Which of the following is the best explanation for this observation? A) K p for the reaction is less than one. B) The activation energy of the reaction is large. C) G for the reaction is positive. D) Such reactions are endothermic. E) The entropy change is negative. 38. (2pts) What does the critical mass mean? It is the Not sure this will be covered this semester. A) amount of fissionable material which will self-sustain a nuclear chain reaction. B) difference between the mass of individual protons and neutrons and the mass of the nucleus. C) energy which holds the nucleus together. D) mass of fuel in a nuclear reactor core. 39. (3pts) What are the Bronsted-Lowry bases in the following chemical reaction? C 5 H 5 N(aq) + H 2 O(l) C 5 H 5 NH + (aq) + OH - (aq) A) C 5 H 5 N(aq), H 2 O(l) B) C 5 H 5 N(aq), C 5 H 5 NH + (aq) C) C 5 H 5 N(aq), OH - (aq) D) H 2 O(l), C 5 H 5 NH + (aq) 10

12 40.Consider the following proposed reaction mechanism: (1) A(aq) + B(aq) X(aq) [fast] (2) X(aq) + C(aq) Y(aq) [slow] (3) Y(aq) D(aq) [fast] (5pts) Write the chemical equation for the overall reaction. (6pts) Write the rate law for and molecularity for each step of the reaction. Step 1: rate law Step 2: rate law Step 3: rate law molecularity molecularity molecularity (5pts) Is the proposed mechanism consistent with the actual rate law: rate=k[a][b][c]? Provide justification for your answer. (4pts) Is the following one-step mechanism equally valid? Provide justification for your answer. A(aq) + B(aq) + C(aq) D(aq) 11

13 41. (8pts) Hydrogen iodide decomposes according to the reaction 2HI(g) H 2 (g) + I 2 (g) K c = at 703K A sealed 1.50L container initially holds mol H 2, mol I 2, and mol HI at 703K. When equilibrium is reached, the concentration of H 2 (g) is M. What are the equilibrium concentrations of HI(g) and I 2 (g)? 42. (8pts) How many minutes would be required to electroplate 25.0 grams of Cr(s) by passing a constant current of 4.80 amperes through a solution containing CrCl 3? 43. (7pts) The heaviest known isotope of hydrogen is called tritium, H 3 1. It decays by beta emission, and has a half-life of 12.3 years. What fraction of a tritium sample will remain after 5.20 years? 12

14 44 (6pts) Does any solid Cu(OH) 2 form when 0.075g KOH is dissolved in 1.0L of M Cu(NO 3 ) 2? The K sp for Cu(OH) 2 is M. Justify your answer. This was not covered this semester; however, you ought be able to figure out the answer by applying concepts that we covered this semester. 45. (6pts) On the graph provided below, draw the titration curve that would result from the titration of a weak base (NH 3 ) with a strong acid (HCl); you may assume that both solutions are 0.10 M and that there is 50.0 ml of the weak base solution. (Hint: the pka of NH 4 + is 9.25) Label the region of the curve that is buffered. Label the equivalence point. Label the position on the curve in which [NH 3 ]=[NH 4 + ] ph ml HCL added 13

15 46. The equilibrium constant for the reaction below is K c = at 298K. 2Fe 3+ (aq) + Hg 2 2+ (aq) 2Fe 2+ (aq) + 2Hg 2+ (aq) (6pts) What is G at this temperature? (6pts) Calculate G when [Fe 3+ ] = 0.20M, [Hg 2 2+ ] = 0.010M, [Fe 2+ ] = 0.010M, and [Hg 2+ ] = 0.025M. (4pts) In which direction will the reaction proceed to achieve equilibrium? Justify your answer. 14

16 47. (6pts) HPO 4 - can act as either an acid or a base in water. Write two separate chemical equations, one in which HPO 4 - acts as an acid in water, the other in which HPO 4 - acts as a base in water. (6pts) Predict whether Na 2 HPO 4 will form an acidic solution or a basic solution on dissolving in water. K a = for HPO 4 2- and K a = for H 2 PO 4 -. Justify your answer. 48. A voltaic cell is constructed with an Fe/Fe 2+ half-cell ( E red = V ) and an Mn/Mn 2+ half-cell ( E red = 1. 18V ). (5pts) Write the balanced overall spontaneous reaction. (6pts) Diagram the cell, labeling the electrodes, the anode and cathode, showing the flow of electrons in the circuit, the cell emf, and the flow of cations and anions in the salt bridge. (2pts) Extra Credit: Briefly describe your favorite demonstration from Chemistry

17 EQUATIONS AND CONSTANTS R= (atm. L)/(mol. K) ph = -log [H 3 O + ] PV=nRT poh = -log[oh - ] K p =K c (RT) n [base] ph = pka + log [acid] ph + poh = pk w 1 st order process K a K b =K w = ln[a] t =-kt + ln[a] 0 t 1/2 =ln2/k R=8.314J/mol-K F=96485J/V-mol 2 nd order process G= H-T S 1 1 = kt + G= G +RTlnQ [A] [A t ] 0 t 1/2 =1/(k[A] 0 ) G =-RTlnK G =-nfe RT E = E lnq nf A=C/s 16

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