CHEM 102 Final Mock Exam

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1 CHEM 102 Final Mock Exam 1. A system releases 300 J of heat and does 650 J of work on the surroundings. What is the change in internal energy of the system? a J b. 350 J c. 950 J d J 2. Which of the following substances will experience hydrogen bonding? A. HI B. HF C. CH 3 NH 2 D. CH 2 O E. All of the above F. B and C G. A and B H. B and D 3. A sample of pure CH 3 OCH 3 is held together with I. dipole-dipole forces II. hydrogen bonding III. London dispersion forces IV. Ionic bonds A. I, II, III B. I, and III C. only I D. none of the above (A-C) is correct 4. Which of the following would dissolve best in NH 3? a. CH 4 b. C 5 H 12 c. O 2 d. H 2 O 5. A liquid with a low vapor pressure with have a. Low intermolecular forces and a low viscosity b. High intermolecular forces and a high viscosity c. A high surface tension and low viscosity d. A low surface tension and high viscosity e. A low ΔH vap and a high boiling point f. A high ΔH vap and a low boiling point 6. Which of the following are exothermic? a. A process with a ΔH < 0 b. Sublimation c. Vaporization d. Freezing e. A and B f. B and C g. C and D h. A and D a. None of the above

2 Use the figure below to answer the following question Red Blue Black 7. What is the normal boiling point of the blue liquid? a. 80 b. 20 c. 50 d. 65 Indicate if the following are soluble in water (A) or not soluble in water (B) 8. K 2 SO 4 A 9. NaOH A 10. C 4 H 10 B 11. Ca(NO 3 ) 2 A 12. NH 4 Cl A 13. MgCO 3 B 14. O 2 B 15. Which of the following happens when Mg 3 (PO 4 ) 2 is added to water? a. Mg 3 (PO 4 ) 2 Mg 3+ + PO 4-2 b. Mg 3 (PO 4 ) 2 3Mg PO 4-3 c. Mg 3 (PO 4 ) 2 Mg 3+ + PO 4-2 d. Mg 3 (PO 4 ) 2 3Mg PO 4-3

3 16. Which of the following happens when HNO 2 is added to water? a. HNO 2 H + + NO 2 - b. HNO 2 + H 2 O H 3 O + + NO 2 - c. HNO 2 + H 2 O OH - + H 2 NO 2 + d. No reaction e. None of above Consider the following reaction CH 3 COOH(aq) + H 2 O (l) CH 3 COO - (aq) + H 3 O + (aq) ΔH= -10 kj 17. Which of the following actions will result in an increase of CH 3 COOH? a. Lower the temperature of the system b. Raise the temperature of the system c. Some hydronium is removed d. Decrease pressure e. Decrease volume 18. A dilute solution is prepared by transferring 50.0mL of a 2.00M stock solution to a 750mL flask. What is the molarity of this dilute solution? a. 30.0M b M c. 7.50M d. 2.00M 19. An aqueous solution is 16.0% by mass KCl and has a density of 1.06g/mL. The molarity of the solution is a M b M c M d. 30.8M 20. Which of the following aqueous solutions will have the highest freezing point? a. Pure water b m KCl c m Cu(CH 3 COO) 2 d m CH An aqueous solution with solute particles with have a lower a. More, boiling point b. Fewer, osmotic pressure c. Fewer, vapor pressure d. None of the above make the sentence true

4 22. Which of following has the lowest vant hoff factor? a. KCl b. Mg(OH) 2 c. CH 3 CH 2 CH What is the vapor pressure at 20 of a solution prepared by the addition of 8.87g of the nonvolatile solute urea, CO(NH 2 ) 2, to 57.6g of methanol, CH 3 OH? The vapor pressure of pure methanol at 20 is 89.0 mmhg. a. 6.75mmHg b. 69.1mmHg c. 77.1mmHg d. 82.2mmHg e. 19.9mmHg 24. The proper equilibrium expression for the following equation is Kc=. 3H 2 + N 2 2NH 3 a. [H 2 ]3 [N 2 ] [NH 3 ] b. [H 2 ][N 2 ] [NH 3 ] c. [NH 3] 2 [H 2 ] 3 [N 2 ] d. 2[NH 3] 3[H 2 ][N 2 ] 25. If the equilibrium constant for A + 2B C is Kc= 5, what is the equilibrium constant for 2C 2A + 4B? a. 25 b c d What is the freezing point of a 0.50m solution of ribose, C 5 H 10 O 5, in water? (K f for water is /m.) a b c d. 1.86

5 27. Consider the following chemical reaction: 2NH 3 (g) 3H 2 (g) + N 2 (g) Kc= 20.5 a. At equilibrium, the concentrations of H 2 and N 2 were 0.20M and 0.35M respectively. What is the equilibrium concentration of NH 3? b M c M d. 0.45M e M 28. At 100,the equilibrium constant (Kc) for the reaction below is 3.50 x COCl 2 (g) CO(g) + Cl 2 (g) A closed 2.00 L vessel is filled with 3.54 moles of COCl 2. At equilibrium, the concentration of Cl 2 is. a x 10-2 b x 10-5 c x 10-3 d x The following reaction was taking place in a 4.00L beaker. The concentrations of SO 3, SO 2, and O 2 were measured as 0.65M, 1.50M, and 0.75M respectively. 2SO 3 (g) 2SO 2 (g) + O 2 (g) Kc= 7.54x10-6 Which of the following statements is true? More than one may be chosen. a. Equilibrium lies to the left b. Equilibrium lies to the right c. The reaction is in equilibrium d. Equilibrium is reactant favored e. Equilibrium is product favored Use the theoretical acids below to answer the following questions. HX Ka= 5.7 x 10 2 HY Ka= 3.2 x 10-7 HZ Ka= 4.5 x Which of theoretical acids has the weakest conjugate base? a. HX b. HY c. HZ

6 31. Which of theoretical acids has the highest pka? a. HX b. HY c. HZ 32. Which of theoretical acids would produce the most hydronium ions if placed in water? a. HX b. HY c. HZ moles HClO 4 are placed in a 3 L beaker of water. What is the poh of the solution? a b c d moles of NH 3 are placed in a 5 L beaker of water. What is the ph of the aqueous solution? Ka = 5.6 x a b c d For the following combinations, determine if the following mixtures would create a buffer. If it creates a buffer directly, choose A. If the mixture creates a buffer indirectly, choose B. If the mixture does not create a buffer, choose C. 35. H 2 SO 4 + HF C NaOH + NH 4 B 37. CaCl 2 + LiOH C 38. NaF + HF A 39. CH 3 NH 2 + NH 4 Br C 40. HNO 3 + NH 3 B The next 3 are the same as the previous questions, except with molar amounts specified mol Sr(OH) mol H 3 PO 4 C mol H 2 SO mol K 2 SO 3 C mol NaClO mol HF C 44. The ph of a solution with the buffer NH 3 and NH 4 is found to be 4.7. Is this solution still effective at buffering the ph when HCl is added? Ka= 5.6 x a. No, it can t buffer added HCl. b. Yes, it can buffer added HCl.

7 45. The ph of a solution of [0.24]HF and [0.35]KF is measured to be What is the ph after 15mL of 0.5M KOH is added to the 2 L beaker? Ka= 7.2 x 10-4 a b c d An arrhenius acid always will always a. Create H 3 O + in water b. Create OH - in water c. Donate a proton d. Accept a proton 47. A solution with a poh of 2.4 is. a. Acidic b. Basic c. Neutral 48. If a buffer solution has a ph greater than its pk a,. a. The solution is better at neutralizing added acid. b. The solution is better at neutralizing added base. c. The solution is at equilibrium. 49. Which of the following ph s could be achieved with a buffer solution that has a K b of 5.2x10-6? a. 5.2 b. 6.2 c. 7.2 d. 8.2 e. Multiple above answers 50. What is the conjugate acid of HPO 4 2- a. H 3 PO 4 - b. PO 4 3- c. HPO 4 2- d. H 2 PO For a titration, the solution that is in the buret is called the. a. mobile phase b. eluant c. solvent d. titrant e. equivalent 52. Bromocresol green is yellow in its acidic form and blue in its basic form. When is it green? a. at the equivalence point of the titration b. in its neutral form c. when the solution ph equals its pka d. when the solution ph equals 7 e. at the midpoint of the titration

8 Consider the following plot: 53. It is most likely associated with a titration. a. SA/ Polygenic Base b. WA/ Polypeptide base c. Polytechnic acid/sb d. Polyprotic acid/ SB 54. The point when an indicator in an acid/base titration changes color is called the end point. a. True b. False 55. At the equivalence point of a SA/SB titration, what is typically present in the flask along with water? a. Leftover SA and salt b. Leftover SB and salt c. only the dissolved basic salt and water d. only the dissolved neutral salt and water e. only the dissolved acidic salt and water 56. In a acid/base titration of NaCN(aq) with HCl, the ph of the equivalence point will be. a. Less than 7 b. Equal to 7 c. Greater than 7 d. Can t be determined without more data 57. Which of the following equations will you solve to find the molar solubility of gold(i) phosphate, Au 3 PO 4? a. K sp = 27x 4 b. K sp = 2x 3 c. K sp =4x 3 d. K sp =x 2 e. K sp =9x 4 f. None of the above

9 58. Given the reactions below, what is the overall enthalpy change for the following reaction? C 4 H 4 (g) + 2H 2 (g) C 4 H 8 (g) ΔH 0 =??? Reaction ΔH o (kj) C 4 H 4 (g) + 5O 2 (g) 4CO 2 (g) + 2H 2 O(l) H 2 (g) + ½ O 2 (g) H 2 O(l) -286 C 4 H 8 + 6O 2 (g) 4CO 2 (g) + 5H 2 O(g) a kj b kj c kj d kj e kj 59. A system releases 300 J of heat and has 650 K of work done on it by the surroundings. What is that change in the internal energy of the system? a J b J c J d J Consider the following process and answer the next 3 questions with A for True and B for false. Fe 2 O 3 is commonly known as rust. 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) 60. The process is spontaneous. a. True b. False 61. The process has a positive ΔS (HINT: Look at the state of matter the reagents are in) a. True b. False 62. The process as written has the heat of reaction equal to the heat of formation of rust (ΔH rxn o =ΔH f o ). a. True b. False 63. A process that is spontaneous in the forward direction has to be nonspontaneous in the reverse direction. a. True b. False 64. A process that has a ΔG<0. This process is. a. exothermic b. spontaneous c. endothermic d. nonspontaneous e. at equilibrium

10 Use the following to answer the next two questions: Mg(s) + 2HCl(aq) MgCl 2 (aq) + H 2 (g) ΔH rxn = -460 kj 65. The thing written above is called a. a. Thermochemical equation b. Formation reaction c. Neutralization reaction d. Precipitation reaction 66. Using the information above, calculate the amount of heat transferred when 735 g of magnesium reacts completely (tell me in words which direction the heat goes). a. 14,000 kj heat given off b. 14,000 kj heat absorbed c. 340,000 kj heat given off d. 340,000 kj heat absorbed e. 15 kj heat absorbed f. 15 kj heat given off 67. A process has a positive ΔH and a negative ΔS. This process is. a. Spontaneous only at high temperatures b. Spontaneous only at low temperatures c. Spontaneous at all temperatures d. Nonspontaneous at all temperatures 68. What is the difference between ΔG and ΔG o? a. ΔG o refers to the formation of a compound from its elements; ΔG can be defined for any reaction b. ΔG o refers to the formation of a pure compound; ΔG can be defined for an impure compound c. ΔG o refers to a reaction that goes to completion; ΔG is defined for a reaction that goes to any extent d. ΔG o refers to the conversion of reactants in the standard state to products in their standard state; ΔG is defined for any reaction under any conditions e. ΔG o refers to reactions of one mole quantities of reactants; ΔG is defined for any quantity of reactants 69. The process of H 2 O(s) H 2 O(l) is. a. Endothermic because of a +ΔH b. Endothermic because of a +ΔS c. Endothermic because of a -ΔH d. Endothermic because of a -ΔS e. Exothermic because of a +ΔH f. Exothermic because of a +ΔS g. Exothermic because of a -ΔH h. Exothermic because of a -ΔS 70. Which of the following will have the greatest standard molar entropy (S o )? a. NH 3 (g) b. H 2 O(l) c. He(g) d. CaCO 3 (s) e. C(s, graphite) 71. For a certain process at 355 K, ΔG = kj and ΔH = -9.2 kj, therefore ΔS for the process is. a. 0 J/K d. 7.3 J/K b J/K e J/K c J/K

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