1022_3rd Exam_

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1022_3rd Exam_1030521 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) For the following example, identify the following. H2O(l) H2O(g) A) a negative H and a negative S B) a positive H and a positive S C) a negative H and a positive S D) a positive H and a negative S E) It is not possible to determine without more information. 2) Place the following in order of increasing molar entropy at 298 K. CO2 C9H20 CO A) CO2 < C9H20 < CO B) CO2 < CO < C9H20 C) C9H20 < CO < CO2 D) C9H20 < CO2 < CO E) CO < CO2 < C9H20 3) Calculate the G rxn using the following information. 2 HNO3(aq) + NO(g) 3 NO2(g) + H2O(l) G rxn =? G f (kj/mol) -110.9 87.6 51.3-237.1 A) +51.0 kj B) +171.1 kj C) -162.5 kj D) -54.5 kj E) -87.6 kj 4) Which of the following reactions will have the largest equilibrium constant (K) at 298 K? A) CaCO3(s) CaO(s) + CO2(g) G =+131.1 kj B) Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g) G = -28.0 kj C) 2 Hg(g) + O2(g) 2 HgO(s) G = -180.8 kj D) 3 O2(g) 2 O3(g) G = +326 kj E) It is not possible to determine without more information. 1030521_1

5) Consider the following reaction at constant P. Use the information here to determine the value of Ssurr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N2(g) + 2 O2(g) 2 NO2(g) H = +66.4 kj A) Ssurr = +223 J/K, reaction is spontaneous spontaneous B) Ssurr = +2656 kj/k, reaction is not spontaneous C) Ssurr = -223 J/K, reaction is not spontaneous D) Ssurr = -66.4 J/K, reaction is not spontaneous E) Ssurr = -66.4 J/K, it is not possible to predict the spontaneity of this reaction without more information. 6) Given the following equation, C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g) G rxn = -2074 kj Calculate G rxn for the following reaction. 7 C3H8(g) + 35 O2(g) 21 CO2(g) + 28 H2O(g) A) -2074 kj B) -296 kj C) +14518 kj D) +2074 kj E) -14518 kj 7) For a given compound, list the decreasing order of entropy for a liquid, solid, and gas A) solid > liquid > gas B) solid > gas > liquid C) gas > solid > liquid D) gas > liquid > solid E) liquid > solid > gas 8) Under which of the following conditions would one mole of He have the highest entropy, S? A) 127 C and 15 L B) 17 C and 25 L C) 17 C and 15 L D) 127 C and 25 L 9) For a given reaction, H = -19.9 kj/mol and S = -55.5 J/Kmol. The reaction will have G = 0 at K. Assume that H and S do not vary with temperature. A) 0.359 B) 2.79 C) 359 D) 298 E) 2789 10) Calculate S rxn for the following reaction. The S for each species is shown below the reaction. C2H2(g) + 2 H2(g) C2H6(g) S (J/mol K) 200.9 130.7 229.2 A) -233.1 J/K B) -102.4 J/K C) 229.2 J/K D) +560.8 J/K E) +303.3 J/K 1030521_2

11) Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) ClO(g) + O2(g) G = - 34.5 kj A) 8.96 10-7 B) 0.986 C) 4.98 10-4 D) 1.12 106 E) 5.66 105 12) The Law of Thermodynamics states the entropy of a perfect crystal at absolute zero is zero. A) Zero B) First C) Second D) Third E) Fourth 13) Estimate G rxn for the following reaction at 825 K. 2 Hg(g) + O2(g) 2 HgO(s) H = -304.2 kj; S = -414.2 J/K A) -2.63 kj B) +37 kj C) +645 kj D) -645 kj E) -37 kj 14) Which one of the following has the highest standard molar entropy, S, at 25 C? A) Cl2(g) B) I2(g) C) O2(g) D) F2(g) E) Br2(l) 15) Place the following in order of decreasing standard molar entropy. NaF(s) Li3PO4(aq) NaF(aq) A) NaF(s) > Li3PO4(aq) > NaF(aq) B) Li3PO4(aq) > NaF(aq) > NaF(s) C) NaF(aq) > Li3PO4(aq) > NaF(s) D) NaF(aq) > NaF(s) > Li3PO4(aq) E) NaF(s) > NaF(aq) > Li3PO4(aq) 16) Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) 2 HgO(s) H = -304.2 kj; S = -414.2 J/K A) 8.10 1031 B) 1.87 1010 C) 5.34 10-11 D) 2.31 10-22 E) 4.33 1021 1030521_3

17) Place the following in order of increasing molar entropy at 298 K. NO CO SO A) NO < CO < SO B) SO < CO < NO C) CO < NO < SO D) CO < SO < NO E) SO < NO < CO 18) Calculate the G rxn using the following information. 2 HNO3(aq) + NO(g) 3 NO2(g) + H2O(l) G rxn =? H f (kj/mol) -207.0 91.3 33.2-285.8 S (J/mol K 146.0 210.8 240.1 70.0 A) +50.8 kj B) -151 kj C) +222 kj D) -85.5 kj E) -186 kj 19) Identify the compound with the lowest standard free energy of formation. A) NaCl(s) B) NO(g) C) O3(g) D) O2(g) E) It is hard to determine. 20) Identify the compound with the highest standard free energy of formation. A) NO(g) B) H2(g) C) NaCl(s) D) O3(g) E) It is hard to determine. 21) Calculate Grxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g) + O2(g) 2 HgO(s) G = -180.8 kj P(Hg) = 0.025 atm, P(O2) = 0.037 atm A) +60.7 kj B) +207 kj C) -154.4 kj D) -26.5 kj E) -164 kj 1030521_4

22) Use Hess's law to calculate G rxn using the following information. NO(g) + O(g) NO2(g) G rxn =? 2 O3(g) 3 O2(g) G rxn = +489.6 kj O2(g) 2 O(g) G rxn = +463.4 kj NO(g) + O3(g) NO2(g) + O2(g) G rxn = - 199.5 kj A) +277.0 kj B) -225.7 kj C) -676.0 kj D) +753.5 kj E) -1152.5 kj 23) Which one of the following would be expected to have the lowest standard molar entropy, S, at 25 C? A) C14H30(s) B) C10H22(l) C) C10H22(s) D) C14H30OH(l) 24) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 C. 3 I2(s) + 2 Fe(s) 2 Fe3+(aq) + 6 I (aq) Fe3+(aq) + 3 e Fe(s) E = -0.036 V I2(l) + 2 e 2 I (aq) E = +0.54 V A) 8.9 10-18 B) 1.7 1029 C) 2.4 1058 D) 1.1 1017 E) 3.5 10-59 25) What is the reducing agent in the redox reaction represented by the following cell notation? Zn(s) Zn2+(aq) Ag+(aq) Ag(s) A) Pt B) Zn2+(aq) C) Ag+(aq) D) Zn(s) E) Ag(s) 26) What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s) Fe2+(aq) H+(aq) H2(g) Pt A) Fe(s) B) Fe2+(aq) C) H+(aq) D) H2(g) E) Pt 1030521_5

27) Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Br2 and OH in the balanced reaction? Br2(l) BrO3 (aq) + Br (aq) A) Br2 = 1, OH = 2 B) Br2 = 3, OH = 3 C) Br2 = 2, OH = 5 D) Br2 = 3, OH = 6 E) Br2 = 1, OH = 6 28) Given that E red = -0.40 V for Cd2+/Cd at 25 C, find E and E for the concentration cell expressed using shorthand notation below. Cd(s) Cd2+(1.0 10-5 M) Cd2+(0.100 M) Cd(s) A) E = 0.00 V and E = +0.12 V B) E = -0.40 V and E = -0.28 V C) E = -0.40 V and E = -0.16 V D) E = 0.00 V and E = +0.24 V 29) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 C. Sn(s) Sn2+(aq, 1.8 M) Ag+(aq, 0.055 M) Ag(s) Ag+ (aq) + e- Ag (s) E = +0.800 V Sn2+ (aq) + 2e- Sn(s) E = -0.14 V A) +0.98 V B) -0.94 V C) +1.02 V D) -0.85 V E) +0.86 V 30) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 C. (The equation is balanced.) Pb(s) + Br2(l) Pb2+(aq) + 2 Br (aq) Pb2+(aq) + 2 e Pb(s) Br2(l) + 2 e 2 Br (aq) E = -0.13 V E = +1.07 V A) -0.60 V B) -1.20 V C) -0.94 V D) +1.20 V E) +0.94 V 31) For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) Zn2+(aq) Ni2+(aq) Ni(s) A) Zn(s) Zn2+(aq) + 2 e- B) Ni2+(aq) + 2 e- Ni(s) C) Ni(s) Ni2+(aq) + 2 e- D) Zn2+(aq) + 2 e- Zn(s) 1030521_6

32) Describe how water can be a good conductor of current. A) add salt B) vaporize the water C) heat the water D) use pure water E) chill the water 33) What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq) + 2 Ag(s) Co(s) + 2 Ag+(aq) A) Co2+(aq) + 2 e- Co(s) B) Ag(s) + e- Ag+(aq) C) Ag+(aq) + e- Ag(s) D) Co2+(aq) + e- Co(s) 34) Determine the cell notation for the redox reaction given below. Sn(s) + 2 H (aq) Sn2+(aq) + H2(g) A) Sn(s) Sn2+(aq) H+(aq) H2(g) Pt B) Sn(s) H2(g) Sn2+(aq) H+(aq) Pt C) H+(aq) H2(g) Pt Sn(s) Sn2+(aq) D) H2(g) H+(aq) Pt Sn2+(aq) Sn(s) E) Sn2+(aq) Sn(s) H2(g) H+(aq) Pt 35) What element is being reduced in the following redox reaction? MnO4 (aq) + H2C2O4(aq) Mn2+(aq) + CO2(g) A) Mn B) C C) H D) O 36) Which of the following processes have a S > 0? A) N2(g) + 3 H2(g) 2 NH3(g) B) Na2CO3(s) + H2O(g) + CO2(g) 2 NaHCO3(s) C) CH3OH(l) CH3OH(s) D) CH4(g) + H2O(g) CO(g) + 3 H2(g) E) All of the above processes have a S > 0. 37) The Law of Thermodynamics states the energy is conserved in chemical processes. A) Zero B) First C) Second D) Third E) Fourth 1030521_7

38) How many electrons are transferred in the following reaction? 2 Al (s) + 6 H+ (aq) 2 Al3+ (aq) + 3 H2 (g) A) 1 B) 2 C) 3 D) 5 E) 6 Table 18.1 Selected Standard Electrode Potentials at 25 C Reaction E, V Mg2+ (aq) + 2 e- Mg (s) -2.356 Fe2+ (aq) + 2 e- Fe (s) -0.440 Pb2+ (aq) + 2 e- Pb (s) -0.125 2 H+ (aq) + 2 e- H2 (g) 0.0 Cu2+ (aq) + 2 e- Cu (s) +0.337 I2 (s) + 2 e- 2 I- (s) +0.535 Fe3+ (aq) + 2 e- Fe2+ (aq) +0.771 Ag+ (aq) + e- Ag (s) +0.800 O2 (g) + 4 H+ (aq) + 2 e- 2 H2O +1.229 Cl2 (g) + 2 e- 2 Cl- (aq) +1.358 F2 (g) + 2 e- 2 F- (aq) +2.866 39) (Refer to Table 18.1) Which is the best oxidizing agent? A) Cu2+ B) Cl2 C) Mg2+ D) F- E) Fe3+ 40) (Refer to Table 18.1) Which is the best reducing agent? A) F- B) Mg C) Fe2+ D) Ag E) Pb 41) (Refer to Table 18.1) Which is the most easily oxidized? A) Mg B) Cl- C) Cu D) H+ E) Fe 42) (Refer to Table 18.1) Which is the most easily reduced? A) Cl- B) Mg2+ C) Cl2 D) H+ E) Cu 43) (Refer to Table 18.1) Which of the following will reduce Fe3+ to Fe2+ but not H+ to H2 (g)? A) Fe B) Ag C) Mg D) Cl- E) Cu 1030521_8

44) (Refer to Table 18.1) Will the following reaction occur spontaneously as written? Cu2+ (aq) + Fe (s) Cu (s) + Fe2+ (aq) A) yes B) no C) impossible to tell 45) (Refer to Table 18.1) Calculate the value of Keq at 25 C for the reaction: F2 (g) + 2 I- 2 F- (aq) + I2 (g) A) 5.3 1039 B) 2.33 C) 2.6 1039 D) 6.0 1078 E) 1.4 10-79 46) Use the Nernst equation to determine Ecell at 25 C for the following voltaic cell. (E cell = +1.100 V ) Zn (s) / Zn2+ (0.10 M) // Cu2+ (1.0 M) / Cu (s) A) 1.16 B) 1.10 C) 1.07 D) 1.13 E) 1.04 47) Which of the following half-reactions is not correct? A) Pb2+ + e- Pb3+ B) Ag Ag+ + e- C) Cu+ + e- Cu D) Fe3+ + 2e- Fe+ E) Mg Mg2+ + 2e- 48) What mass, in g, of copper will be deposited from a solution of Cu2+ by a current of 2.50 A in 2.00 h? A) 1.65 B) 11.9 C) 5.93 D) 23.7 E) 0.187 49) In the process of electroplating a metal spoon with silver metal, the spoon is the A) anode. B) cathode. C) salt bridge. D) Both A nd B are correct. E) none of the above 50) Which two of the following half-reactions will combine to give the galvanic cell with the highest cell potential? 1) 2 H+(aq) + 2 e- H2(g) E = 0 2) Pb+2(aq) + 2 e- Pb(s) E = -0.125 V 3) I2(s) + 2 e- 2 I-(aq) E = +0.535 V 4) Zn+2(aq) + 2 e- Zn(s) E = -0.763 V A) 3 and 4 B) 1 and 3 C) 2 and 3 D) 2 and 4 E) 1 and 4 1030521_9

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