CHEM1040-f15practicefinal.pdf CHEM 1040 - 001
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This 10 page Study Guide was uploaded by Meredith Notetaker on Saturday December 5, 2015. The Study Guide belongs to CHEM 1040 - 001 at Auburn University taught by Michael E Squillacote in Fall 2015. Since its upload, it has received 88 views. For similar materials see Fundamental Chemistry II in Chemistry at Auburn University.
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Date Created: 12/05/15
Chemistry 1040 Practice Final Exam Professor Michael Squillacote Fall, 2015 Name:________________________________________________________________ E-mail:_______________________________________________________________ See attached last page for Constants and Equations Score: 1. What is the enthalpy change for the reaction: 2C(graphite) + 3H (g) → C H (g) 2 2 6 Data For Reactions Reaction ∆H° rxn(kJ) C(graphite) + O (g) → CO (g -393.5 z 2 H 2g) + ½O (2) → H O(l2 -285.8 2C H (g) + 7O (g) → 4CO (g) + 6H O(l) -3119.6 2 6 2 2 2 A. +1475.2 kJ C. -2804.2 kJ B. -84.6 kJ D. -3798.9 kJ 2. Which oxide will form a basic solution when dissolved in water? A. P 2 5 C. CO 2 B. NO 2 D. KO 2 3. What can be concluded about the relative polarities of compounds A and B? Compound AB Molar mass 152 g·mol -114g·mol -1 Vapor Pressure at 25 °C 15 mmHg 245 mmHg A. B is more polar than A. B. A is more polar than B. C. Vapor pressure at the normal boiling point is needed D. Solubility information is needed. 4. Ammonium sulfide solution, when mixed with a copper(Il) nitrate solution, reacts to give a copper(Il) sulfide precipitate. Which is the correct net-ionic equation? + 2- 2+ ¯ + ¯ A. 2NH (4q) + S (aq) + Cu (aq) + 2NO (aq) → 3uS(s) + 2NH (aq) + 2NO (4q) 3 B . (NH ) S(aq) + Cu (aq) → CuS(s) + 2NH (aq) + 2-2 2+ 4 C. SO 4 (aq) + Cu (aq) → CuSO (s) 4 D. S2-(aq) + Cu (aq) → CuS(s) 5. Which is a statement of the second law of thermodynamics? A. The entropy of the universe is increasing. B. The entropy of the universe is constant. C. The enthalpy of the universe is constant. D. The energy of the universe is decreasing. 6. Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO (s)3→ Na CO (s2 + 3O (g) + H 2(g) 2 At 25°C, for this reaction, ∆H° rxn 128.9 kJ/mol and ∆G° rxn= 33.1 kJ/mol. Above what minimum temperature will the reaction become spontaneous under standard state conditions? A. 0.4 K B. 3.9 K C. 321 K D. 401 K 7. What is the freezing point of a solution made by dissolving 56.0 g of sucrose (C H O ) 12 22 11 225 g of water? (Molar Mass of sucrose = 342 g·mol and K for water = 1.86 °C·mol -1 f A. 1.35 °C B. 0.305 °C C. -0.305 °C D. -1.35 °C 8. Which molecule does not exhibit hydrogen bonding? A. CH 4 B. NH 3 C. HF D. CH O3 9. Calculate the mass of (NH ) SO4 2) n4eded to prepare 1.75 L of a 0.250 M solution. Molar Mass of (NH ) SO = 132.9 g·mol . -1 4 2 4 A. 302 g B. 57.8 g C. 18.9 g D. 3.31 g 10. Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10 –3M Ba(NO ) 3 2 added to 80.0 mL of –4 8.4 × 10 M Na CO 2 3 A. Yes, the ppt is Ba(NO ) 3 2 B. Yes, the ppt is NaNO . 3 C. Yes, the ppt is BaCO . 3 D. No, a precipitate will not form. 11. For the reaction; 2SO (g) ⇌ 2SO (g) + O (g), the correct expression for K is: 3 2 2 p 2 2P SO2x PO 2 P SO2x P O2 2P SO 2+P O2 P 2SO2 + PO2 A. B. C. D. 2P SO3 P 2SO3 2P P 2 SO3 SO3 12. Ice cubes made from ground water rich in dissolved limestone produce extra "fizzing" when a soft drink is poured over them. Choose the pair of ions primarily responsible for this fizzing. + 2- A. H , CO 3 B. H , PO 43- + - C. H , NO 3 D. Ca , OH - -4 13. What is the pH of 0.30 M hydrofluoric acid (HF)? K for HFa= 7.2 x 10 A. 3.67 B. 1.83 C. 1.57 D. 0.52 14. At the end point of a titration, 31.6 mL of HNO (aq)3neutralizes 25.0 mL of a 0.157 M NaOH(aq) solution. What is the concentration of HNO (aq)? 3 A. 0.503 M B. 0.180 M C. 0.145 M D. 0.124 M 15. Which expression is not equivalent to pH? A. 14.0 – pOH B. –log[H O 3 + - C. –log(K /[wO ]) D. –log K w -4 -1 16. What is the solubility product (K ) sp Mg(OH) if it2 solubility in water is 1.6 x 10 mol·L ? -11 A. 1.6 x 10 B. 2.6 x 10 -8 -4 C. 3.2 x 10 D. 4.1 x 10 -12 17. A monoprotic weak acid is titrated with a solution of sodium hydroxide. At the equivalence point, A. pH> 7.0 B. pH= 7.0 C. pH= pK a D. 50% of the acid is neutralized. 18. Which is a strong acid? A. H S2 3 B. HNO 2 C. HBr D. HF 19. The temperature at which the vapor pressure of a liquid is equal to 1.00 atm is the A. critical temperature. B. Curie temperature. C. normal boiling point. D. triple point. 20. For the constant pressure reaction, C(s) + CO (g) 2⇌ 2CO(g), ∆H = +120 kJ·mol which -1 change will increase the equilibrium concentration of CO 2(g)? A. A catalyst is added to the system. B. The temperature of the system is raised. C. CO(g) is added to the system. D. C(s) is added to the system. 21. What is the equilibrium constant, K , for the reaction N O (g) ⇌ 2NO (g), 'when 10.0 mol of c 2 4 2 N 2 (4) are initially placed in a 2.00 L container and 4.00 mol of NO (g) 2re found to be present at equilibrium? A. 4.00 B. 2.00 C. 1.00 D. 0.500 22. The equilibrium constant 2NO(g) + 2H (g) 2 N (g) +22H O(g) i2 1.19 x 10 -3. Which best describes the equilibrium mixture? A. more moles of N 2(g) than H 2g) B. equal moles of reactants and products C. mostly products D. mostly reactants 23. Which reaction coordinate diagram represents a reaction in which the activation energy, E , a is 50 kJ·mol and the ∆H rxnis -15 kJ·mo1 ?-1 A. B. C. D. 24. Using the thermochemical data given, what is the ∆H° rxnfor Substance ∆H° fkJ·mol ) -1 the following reaction? CH O3(l) -238 HC H2O 3l)2-487 2CH OH(l) + O (g) → HC H O (l) + 2H O(i) 3 2 2 3 2 2 H 2(l) -286 A. 583 kJ B. 535 kJ C. -583 kJ D. -535 kJ 25. Reactant A will spontaneously react at constant pressure to form product B according to the equation A → B at all temperatures if A. ∆H < 0 and ∆S > 0 B. ∆H > 0 and ∆S > 0 C. ∆H < 0 and ∆S < 0 D. ∆H > 0 and ∆S < 0 26. The rate law for the reaction between NO and Cl is rate= k[NO] [Cl ]. If the concentration of 2 2 NO is doubled at constant concentration of Cl , th2 rate is A. one-fourth the original rate. B. one-half the original rate. C. two times the original rate. D. four times the original rate. -1 27. Using the tabulated data, what is the rate law for the [H2 initialCl2 initiale(M·s ) reaction? 0.0020 0.0050 2.5 x 10 -3 H (g) + Cl (g) → 2HCl(g) -3 2 2 0.0020 0.0025 1.3 x 10 0.0015 0.0025 1.3 x 10 -3 A. rate = k[Cl 2 2 -3 0.0050 0.0010 0.5 x 10 B. rate = k[Cl 2 C. rate=k[H ]2 D. rate = k[H 2] [C2 ] 28. Under which set of conditions does bromine have the highest entropy? A. Br 2liquid, -7 °C, 1 atm) B. Br 2liquid, 58 °C, 1 atm) C. Br 2 (gas, 58 °C, 1 atm) D. Br (gas, 58 °C, 2 atm) 2 29. Under 1.00 atm pressure, at what temperature will this Thermodynamic Data at 298 K reaction become spontaneous? ∆kJ 230 P 4(g) → 2P (g2 ∆J·K156 -1 A. 74 K B. 436 K C. 1474 K D. There is no temperature at which this reaction is spontaneous. 30. The rate law for the reaction H O 2 22 + 2H + → I +22H O 2s rate = k[H O ] 2I 2. The overall order of the reaction is A. five. B. three. C. two. D. one. 31. The reaction 3Zn(s) + 2Cr (aq) → 3Zn (aq) + 2Cr(s) has a standard cell potential of 2+ +0.019 V. What happens to the potential if the concentration of Zn is increased from 1.0 M to 2.0 M while Cr 3+concentration remains unchanged? A. The cell potential is decreased. B. The cell potential is increased. C. The standard cell potential is decreased. D. The standard cell potential is increased. 32. Calculate E° for the half-reaction Reaction Potentials, E° Pd (aq) + 2e → Pd(s) 2+ 2+ Cu(2+ + Pd (aq)-→ Cu (aq) + Pd(s) +0.650 V Cu (aq) + 2e → CV u(s) +0.337 A. +0.987 V C. +0.313 V B. -0.987 V D. -0.313 V 33. When the oxidation-reduction reaction ? Cr 2 72(aq) +? H 2(aq) → ? Cr (aq) + ? S(s) is balanced in acidic solution, the coefficient of S(s) is A. 4 B. 3 C. 2 D. 1 34. A current of 0.500 A is passed through an electrolytic cell containing molten MgCl for 2.02 hr. Calculate the quantity of Mg metal formed at the cathode. A. 1.81 g B. 0.907 g C. 0.453 g D. 3.07 x 10 g-3 35. In all electrolytic cells, A. the electric current within the electrolyte is a flow of electrons. B. chemical energy is converted into electrical energy. C. an oxidation half-reaction occurs at the anode. D. a salt bridge is used. 36. Which species could act as both an oxidizing agent and a reducing agent? A. Ca 2+ B. F 2- C. CI D. BrO 2- 37. The unusually high boiling point of water is due primarily to A. ionic bonding. B. hydrogen bonding. C. dipole-dipole interaction. D. London dispersion forces. 14 38. The C activity of some ancient Peruvian corn was found to be 10 disintegrations per minute per gram of carbon. If present-day plant life shows 15 dpm/g, how old is the Peruvian corn? (The half-life of4C is 5730 yr). A. 1,455 yr B. 1,910 yr C. 3,350 yr D. 3,820 yr 39. The only stable isotope of aluminum is aluminum-27. What type of radioactive decay should 23 be expected from 13Al ? 4 A. 2He 0 B. -1 1 C. n 0 0 D. +1 40. When atoms of aluminum-27 are bombarded with alpha particles, a neutron and an element are produced. Which particular isotope of this element is formed? A. B. C. D. 41. 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. 42. Which equation correctly represents electron capture by the nucleus? A. B. C. D. 43. Calculate the energy released in joules when one mole of polonium-214 decays according to the following equation. Particle Mass (amu) Pb-210 209.98284 Po-214 213.99519 He-4 4.00260 26 23 –1 8 [1 kg = 6.022 × 10 amu; N =A6.022 × 10 mol ; c = 2.99792458 × 10 m/s] 14 A. 8.78 × 10 14J/mol B. 7.20 × 10 J/mol C. 8.76 × 10 11J/mol –9 D. 1.46 × 10 J/mol 44. What statement below best describes the graph representing the integrated second-order rate law? A. A plot of 1/[A]tvs. t yields a straight line with a negative slope equal to k. B. A plot of ln[A]tvs. t yields a straight line with a positive slope equal to –k. C. A plot of ln[A] vs. t yields a straight line with a negative slope equal to –k. t D. A plot of 1/[A]tvs. t yields a straight line with a positive slope equal to k. 45. Calculate the pH of a buffer solution that contains 0.25 M b–5zoic acid (C H CO 6) 5nd 2 0.15 M sodium benzoate (C H COO6a5. [K = 6.5 × a0 for benzoic acid] A. 3.97 B. 4.83 C. 4.19 D. 4.41 Equation Sheet Chemistry 1040 – Fall 2015 0E C = 273 K R = 8.314 J/K ⋅ mol = 0.08206 L ⋅ atm/ K ⋅ mol F = 96,487 J/(V⋅mol) ln P = - (ΔH vap/RT) + C c = kP ln(P 1P 2 = (ΔH vap/R)(1/T 2 1/T )1 P = X P TE -T = ΔT = iK m A A A f f f f π = iMRT T b-T E b ΔT = bK m b k = Ae (-Ea/RT)ln (k1/k2) = (Ea/R)(1/T 2 1/T ) 1 First Order Second Order ln[A] = ln[A] okt 1/[A] = 1/[A] o kt t½= (ln2)/k ½ =1/ (k[A] )o 2 + - bb 4ac K w [H ][HO ] x 2a = 1.0 x 10 -14 = K Ka b pH = -log[H ]+ pK a -log K a + - Δn K a [H ][A ]/[HA] K p K (Rc) - ΔG = ΔH – TΔS pH = pK a+ log([A ]/[HA]) ΔG = ΔGE + RTlnQ ΔGE = -RTlnK ΔGE = -nFEE cell E = EE- (RT/nF)lnQ First order radioactive decay t = (-t½/ln2)(ln (N tN 0)
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