NAME ______________________________________________ © Keeney-Kennicutt, 2010 B1 CHEMISTRY 102 FALL 2010 EXAM 2 FORM B SECTION 501 DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and PART 2 of the exam where indicated. (2) Sign the Aggie Code on PART 2 of this exam. (3) Each multiple choice question is actually 2 questions on your scanning sheet. If you are sure of an answer, put the same answer down for both questions for 5 pts. If you cannot decide between two answers, put your best answer down for the first (odd) question and the other answer down for the second (even) question. If you get the first one correct you'll get 3 pts; if you get the second one correct you’ll get 2 pts. If there is an ambiguous multiple choice question, use the last page to explain your answer. (4) Do NOT write on the envelope. (5) When finished, put everything in the envelope and wait to be excused. At the table, take everything out of the envelope. You can pick up the multiple choice part with the answers outside my office after 3pm. (6) There are a total of 35 questions (19 actual questions). PART 1 1&2. Which is the correct Kc expression for the equilibrium: CH4(g) →← C(s) +2H2(g)? (a) Kc = [H2]2[CH4] (b) Kc = [C][H2]2[CH4] (c) Kc = [C][2H2]2[CH4] (d) Kc = 2[H2][CH4] (e) [C]2[H2][CH4] 3&4. This sketch represents which of the following situations where : is A and is B. (a) 2A →← B K >> 1 (b) B2 →← A K << 1 (c) B →← A2 K >> 1 (d) A2 →← B K << 1 (e) A →← B2 K << 1 5&6. The rate law for the chemical reaction, 5Br− + BrO3− + 6H+ → 3Br2 + 3H2O has been determined experimentally to be: −Δ[BrO3−] Δt = k[Br−][BrO3−][H+]2 The reaction order with respect to the bromide ion is (a) 1 (b) 2 (c) 6 (d) k[H+]2 (e) k[Br−][BrO3−][H+]2© Keeney-Kennicutt, 2010 B2 7&8. If a reaction has a slightly negative ΔG, like ΔG= −50 J, the reaction will occur: (a) slowly. (b) rapidly. (c) with a high activation energy. (d) with a low activation energy. (e) It is impossible to know from the ΔG information. 9&10. The principal reason for the increase in reaction rate with increasing temperature is: (a) the activation energy increases with increasing temperature. (b) molecules increase in size at high temperature. (c) the activation energy decreases with increasing temperature. (d) the fraction of high energy molecules increases with increasing temperature. (e) the pressure exerted by reactant molecules increases with increasing temperature. 11&12. Which CANNOT be true for the 1 step reaction: N=O + N=N=O Æ O=N-O + N≡N? (a) Rate = k[NO][N2O] (b) The rate determining step is a bimolecular collision. (c) The oxygen atom in NO must collide with the N in N2O for an effective collision. (d) As temperature increases, the rate of the reaction increases. (e) All the statements are true. 13&14. Which of the following statements is/are TRUE concerning the action of catalysts? (1) Catalysts participate in the reaction. (2) Their presence do not change the mechanism of the reaction. (3) The activation energy of the rate-determining step is raised and the reaction speeds up. (a) 1,2 (b) 1 only (c) 1,3 (d) 1,2,3 (e) none of these 15&16. The ΔH (=ΔE) for a reaction is −55 kJ. The activation energy for the reverse reaction is 200 kJ. What is the activation energy for the forward reaction? It might be helpful to sketch the potential energy diagram. (a) +145 kJ (b) +255 kJ (c) −255 kJ (d) −145 kJ (e) +55 kJ© Keeney-Kennicutt, 2010 B3 17&18. Rate data were collected for the following reaction at a particular temperature. What is rate law expression? A(g) + 2B(g) → C(g) + 2D(g) Experiment [A]initial [B]initial Initial Rate of Reaction 1 0.10 M 0.10 M 0.020 M/s 2 0.20 M 0.10 M 0.080 M/s 3 0.20 M 0.20 M 0.160 M/s (a) Rate = k[A][B] (b) Rate = k[A]2[B]2 (c) Rate = k[A][B]2 (d) Rate = k[A]2[B]3 (e) Rate = k[A]2[B] 19&20. At 445oC, the value for Kc for the following reaction is 49: H2(g) + I2(g) →← 2HI(g) A mixture of H2, I2 and HI in a vessel has the following concentrations: [H2] = 0.10 M [I2] = 0.010 M [HI] = 0.50 M Which one of the following statements concerning the reaction quotient, Qc, is TRUE for the above system? (a) Qc = Kc; and the system is at equilibrium. (b) Qc = 0.0040; more HI will be produced as the system proceeds to equilibrium. (c) Qc = 0.0040; more H2 and I2 will be produced as the system proceeds to equilibrium. (d) Qc = 250; more HI will be produced as the system proceeds to equilibrium. (e) Qc = 250; more H2 and I2 will be produced as the system proceeds to equilibrium© Keeney-Kennicutt, 2010 B4 21&22. Cyclobutane, C4H8, converts to ethylene, C2H4, by first order kinetics with half-life of 1.33 x 10–4 min at 1000oC. What percentage of cyclobutane will be converted to products after 0.035 s? C4H8 → 2 C2H4 (a) 31% (b) 8.1% (c) 4.3% (d) 95.2% (e) 92.1% 23&24. Consider the following equilibrium at 200oC: X + Y →← 2Z, with a Kc of 0.16. Initially, there is 3.00 M of Z in the container. What is the concentration of Z in the container after the system has reached equilibrium? (a) 0.10 M (b) 1.20 M (c) 0.50 M (d) 0.30 M (e) 2.80 M© Keeney-Kennicutt, 2010 B5 25&26. Consider the reaction: X → Y. What is the activation energy for the forward reaction (in kJ) when the rate constant at 10oC is 0.125 min-1 and the rate constant at 60oC is 2.11 min-1? ln⎝⎛⎠⎞k2k1 = – EaR ⎝⎛⎠⎞1T2 - 1T1 or ln⎝⎛⎠⎞k2k1 = EaR ⎝⎛⎠⎞T2 - T1T1T2 or ln⎝⎛⎠⎞k2k1 = EaR ⎝⎛⎠⎞1T1 - 1T2 R = 8.314 J/mol·K (a) 2.1 kJ (b) 15.9 kJ (c) 30.7 kJ (d) 42.9 kJ (e) 51.8 kJ 27&28. Estimate the sublimation temperature of solid sodium, Na, given the following data from thermodynamic tables. Assume that ΔHo f 298 and So do not change with temperature: Na(s) →← Na(g) ΔHo f 298 (kJ/mol) So (J/mol⋅K) ΔGo f 298 (kJ/mol) Na(s) 0 51.5 0 Na(g) 107.3 153.8 76.8 (a) 335oC (b) 776oC (c) 515oC (d) 1oC (e) 495oC© Keeney-Kennicutt, 2010 B6 29&30. Calculate ΔGo for the following reaction at 25oC in kJ: N2 (g) + O2(g) → 2 NO(g) at