FinalF2000FormA - Chemistry 12 – Final Exam December 14,...

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Unformatted text preview: Chemistry 12 – Final Exam December 14, 2000 FORM A ----------------------------------------------------------------------------------------------------1. For the following reaction at 1000 K, Kp = 3.9×10−2. CO(g) + Cl2 (g) COCl2(g) A. 4.69 × 10−6 B. 5.79 × 10−6 C. 2.75 × 10−4 D. 3.20 E. 324 ------------------------------------------------------------------------------------------------------2. Consider the following reaction at a constant temperature for which Kp = 2.7. CO2(g) + H2(g) If 0.153 mole of CO, 0.546 mole of H2O, 0.262 mole of CO2 and 0.743 mole of H2 are introduced into a 2 L vessel, which of the following statements will be true? A. The system is at equilibrium and no change will occur. B. The system is not at equilibrium and will proceed to the right to achieve equilibrium. C. The system is not at equilibrium and will proceed to the left to achieve equilibrium. D. The system is not at equilibrium and it cannot achieve equilibrium. E. The system is at equilibrium, but the addition of a catalyst will cause the reaction to proceed to the right. ------------------------------------------------------------------------------------------------------3. At high temperature, 1.0 mole of ICl is allowed to decompose in a 2.0 L flask. 2ICl(g) A. 0.2 M NaBr B. 0.2 M NH4OH C. 0.2 M Ba(NO3)2 D. 0.2 M AlCl3 E. 0.2 M C12H22O12 (sugar) ------------------------------------------------------------------------------------------------------- What is the value of Kc for this reaction? CO(g) + H2O(g) 4. Which one of the following aqueous solutions will have the highest vapor pressure? I2(g) + Cl2(g) The equilibrium constant for this reaction at the temperature of interest is Kc = 0.110. What is the equilibrium concentration of ICl(g)? A. 0.10 M B. 0.20 M C. 0.30 M D. 0.50 M E. 0.60 M ________________________________________________________________________ 5. A solution of isopropanol (C3H5OH) is made by dissolving 0.250 mole of isopropanol in 0.950 mole of water. What is the molality of the solution? A. 0.0146m B. 0.209m C. 0.459m D. 0.791m E. 14.6m ------------------------------------------------------------------------------------------------------6. The normal boiling point of an aqueous solution made by dissolving 145.0 g of caffeine in 250.0 g of water is 101.55 °C. Kb of water is 0.52 oC/m. What is the molar mass of caffeine? A. 10.44 g/mole B. 580.0 g/mole C. 123.2 g/mole D. 335.5 g/mole E. 194.2 g/mole ----------------------------------------------------------------------------------------------------7. For the following reaction, what will happen if the volume of the system is decreased? 2 C(s) + O2(g) 2 CO(g) 1. The equilibrium will shift to the left. 2. The equilibrium will shift to the right. 3. The mass of C(s) will increase. A. 1 only B. 2 only C. 3 only D. 1 and 3 E. 2 and 3 ----------------------------------------------------------------------------------------------------- 8. What is the osmotic pressure of a 0.100 M solution of a nonelectrolyte at 20 °C ? A. 1.00 atm B. 2.41 atm C. 0.164 atm D. 4.82 atm E. 1.64 atm ----------------------------------------------------------------------------------------------------9. If a sample of CCl4 at constant pressure of 1 atm was heated starting at point A and ending at point B, what phase transition(s) would be observed? 11. Which of the following intermolecular forces are present in the molecule shown? 1. London dispersion forces 2. Dipole-dipole forces 3. Hydrogen bonding O A. 1 and 2 C B. 1 and 3 CH3 CH3 C. 2 and 3 D. 1 only E. 2 only ----------------------------------------------------------------------------------------------------12. Consider a closed vessel with a pure liquid inside that is at equilibrium with its vapor. Increasing the total pressure above the liquid will cause the boiling point of the liquid to B A 1 atm P 13. Which one of the following substances would be the most soluble in CCl4 ? T A. melting B. vaporization C. freezing D. condensation E. sublimation A. increase B. decrease C. remain constant D. it depends on the liquid E. all of the above ----------------------------------------------------------------------------------------------------- ----------------------------------------------------------------------------------------------------- A. CH3CH2OH B. H2O C. NH3 D. C10H22 E. NaCl ----------------------------------------------------------------------------------------------------- 10. The balanced homogeneous gas-phase reaction 14. The value of Kc for the following reaction is 0.25. Z+R G+Q has an equilibrium constant value Kc = 6.2 × 10 −4 . At equilibrium A. products dominate B. reactants dominate C. approximately equal amounts of reactants and products are present D. only products exist E. only reactants exist ----------------------------------------------------------------------------------------------------- SO2 (g) + NO2 (g) SO3 (g) + NO (g) What is the value of Kc for the reaction shown below assuming both reactions are at the same temperature? 2 SO2 (g) + 2 NO2 (g) 2 SO3 + 2 NO (g) A. 0.50 B. 0.062 C. 0.12 D. 0.25 E. 0.37 ----------------------------------------------------------------------------------------------------- 15. How many kJ would it take to change 423.0 g of ice cubes at 0 oC to water at room temperature (25 oC)? ∆Hmelting = 6.01 kJ/mol and Cp(H2O) = 4.184 J/(g oC) 18. How many unpaired electrons are there in the ground state electronic configuration of atomic V? A. 185.4 kJ B. 141.2 kJ C. 2542. kJ D. 2456 kJ E. 4998. kJ ----------------------------------------------------------------------------------------------------- A. 1 B. 2 C. 3 D. 4 E. 5 ----------------------------------------------------------------------------------------------------- 16. Given the following information, calculate the enthalpy for the combustion of 19. Which of the following ionization energies is the largest (I1 = 1st ionization energy, I2 = 2nd ionization energy)? acetylene: 2C2H2(g) + 5O2(g) ! 4CO2(g) + 2H2O(!). 2C(s) + H2(g) ! C2H2(g) ∆H = +227 kJ C(s) + O2(g) ! CO2(g) ∆H = −394 kJ 2H2(g) + O2(g) ! 2H2O(!) ∆H = −572 kJ A. –1301 kJ B. –739 kJ C. –2602 kJ D. –1193 kJ E. 568 kJ ----------------------------------------------------------------------------------------------------17. Which of the following statements are true? 1. All s orbitals are spherically shaped. 2. In the hydrogen atom, electrons in orbitals that have the same principal quantum number have the same energy. 3. In a p orbital, there is a high probability that the electron will be found near the nucleus. A. 1 only B. 2 only C. 3 only D. 1 and 2 are true E. all of the statements are true ----------------------------------------------------------------------------------------------------- A. I1 of Li B. I2 of Ca C. I2 of Al D. I2 of Mg E. I2 of K ----------------------------------------------------------------------------------------------------20. Which of the following represents the correct ordering of lattice energies for NaCl, KCl, and CaO ? A. NaCl > KCl > CaO B. CaO > NaCl > KCl C. KCl > NaCl > CaO D. CaO > KCl > NaCl E. NaCl > CaO > KCl ----------------------------------------------------------------------------------------------------21. How many lone (nonbonded) electron pairs are found in the correct Lewis structure for formaldehyde (CH2O)? (Hint: carbon is the central atom.) A. 0 B. 1 C. 2 D. 3 E. 4 ----------------------------------------------------------------------------------------------------- 22. Using the information below, estimate the enthalpy of the reaction C2H4(g) + H2(g) ! C2H6(g) Some average Bond Enthalpies: C−H 413 kJ/mol C−C 348 kJ/mol C=C 614 kJ/mol C≡C 839 kJ/mol H−H 436 kJ/mol A. –124 kJ/mol B. +101 kJ/mol C. –390 kJ/mol D. –258 kJ/mol E. +213 kJ/mol ----------------------------------------------------------------------------------------------------23. Electrons in which of the following two sets of orbitals of a multielectron atom would have the same energy? 1. n=3, !=2, m! = 2, ms = +1/2 2. n=2, !=2, m! = −2, ms = +1/2 3. n=3, !=2, m! = −2, ms = −1/2 4. n=3, !=1, m! = −2, ms = −1/2 5. n=4, !=2, m! = −2, ms = −1/2 A. 1 and 3 only B. 2 and 3 only C. 3 and 5 only D. 1 and 2 only E. 3 and 4 only ----------------------------------------------------------------------------------------------------24. An unknown liquid has a density of 2.14 g/cm3. How many mm3 would a 6.42 mg sample of this liquid occupy if dispensed into a 10 mm3 UV/VIS spectrophotometer cuvette? A. 3.00 mm3 B. 0.300 mm3 C. 0.0300 mm3 D. 0.00300 mm3 E. none of the above ----------------------------------------------------------------------------------------------------- 25. Identify the functional groups present in the following structure. H 1. ester 2. ether 3. amine 4. ketone 5. amide N CH 3 O A. 1 and 5 B. 2 and 5 C. 2 and 3 D. 4 and 5 E. 3 and 4 ----------------------------------------------------------------------------------------------------26. The correct name for the following branched alkane is CH 3 CH 3 C C CH 2 CH 2 CH 3 CH 2 CH 3 H2 C C H2 CH 3 CH 3 A. 3-ethyl-2,2,3-trimethyloctane B. 2,2,3-trimethyl-3-ethyl-5-propylpentane C. 1-propyl-3-ethyl-3,4,4,-trimethylpentane D. 1,1,1-trimethyl-2-ethylmethylheptane E. 6-ethyl-6,7,7-trimethyloctane ----------------------------------------------------------------------------------------------------- 27. The percent mass of hydrogen in the following compound is H H2 C O H2C H A. Pb+2(aq) + 2 C2H3O2−(aq) → Pb(C2H3O2)2(s) CH3 B. 2 Na+(aq) + 2 C2H3O2−(aq) → 2 NaC2H3O2(s) CH N O 29. When an aqueous solution of Pb(C2H3O2)2(aq) and NaI(aq) are mixed, which of the following reactions is the correct net ionic equation that describes this reaction? C. Pb+(aq) + I−(aq) → PbI(s) CH3 D. Pb2+(aq) + 2 I−(aq) → PbI2(s) H E. Pb2+(aq) + 2 C2H3O2−(aq) + 2 Na+(aq) + 2 I−(aq) → 2 Na+(aq) + 2 C2H3O2−(aq) H + Pb2+(aq) + 2 I−(aq) A. 5.2% B. 7.8% C. 8.7% D. 7.2% E. 8.4% ----------------------------------------------------------------------------------------------------30. 7.2 g of a hydrocarbon is completely combusted in oxygen and found to yield 10.8 g of water and 22.0g of carbon dioxide. The empirical formula for the hydrocarbon is ----------------------------------------------------------------------------------------------------28. Which of the following is/are isomers of the structure below? Br C 2H5 H3C 31. When 47.3mL of 0.107 M HCl is added to 54.7 mL of 0.213 M Ca(OH)2, the resulting OH− concentration is Cl Br Br Cl 1 Cl H3C C2H5 2 A. C5H6 B. C3H7 C. C10H24 D. CH E. C5H12 ----------------------------------------------------------------------------------------------------- H3C Cl Br C 2H5 3 A. 1 B. 2 C. 3 D. 1 and 2 E. 1 and 3 ----------------------------------------------------------------------------------------------------- A. 0.0645 M B. 0.179 M C. 0.114 M D. 0.228 M E. 0.0500 M ----------------------------------------------------------------------------------------------------32. Haloethane has a formula C2HBrClF3. It is a nonflammable, nonexplosive, and nonirritating gas used for inhalation anesthetics. If you mix 15.0 g of haloethane vapor with 23.5 g oxygen gas and the total pressure of the mixture is 855 mm Hg, what is the partial pressure of the haloethane? A. 80.0 mm Hg B. 775 mm Hg C. 938 mm Hg D. 906 mm Hg E. 65.0 mm Hg ------------------------------------------------------------------------------------------------------- 33. Let us say you are asked to design an air bag for your car. What quantity of sodium azide, NaN3, is necessary to fill a 45.5 L airbag with N2 at 838 torr and 22.0 oC ? 2Na (s) + 3 N 2 (g) 2NaN 3 (s) A. 2.05 g B. 125 g C. 27.5 g D. 89.6 g E. 136 g ------------------------------------------------------------------------------------------------------34. The density of an unknown gas is 1.23 g/L at STP. Which of these would most likely be the unknown gas? A. Cl2 B. O2 C. CO D. NH3 E. C2H6 ------------------------------------------------------------------------------------------------------- 37. Which of the following molecules will have a zero dipole moment? A. SF4 B. BrF5 C. ClO2 D. C2F4 E. SO2Cl (Sulfur is the central atom.) ------------------------------------------------------------------------------------------------------38. Which of the following are weak electrolytes? 1. 2. 3. 4. CH3COOH (HC2H3O2) CH3OH C12H22O11 (table sugar) NaClO4 A. 1 and 2 are weak electrolytes B. 1 and 3 are weak electrolytes C. 1, 2 and 3 are weak electrolytes D. 4 is the only weak electrolyte E. 1 is the only weak electrolyte ------------------------------------------------------------------------------------------------------- 35. Which one of the following molecules will NOT have linear molecular geometry about the central atom? 39. Which one of the following is the electron configuration for the Fe+2 ion? A. SCO B. SCN− C. HCN D. C2H2 (HCCH) E. ClO2− (Chlorine is the central atom.) ------------------------------------------------------------------------------------------------------- A. [Ar] 3d6 B. [Ar] 4s2 3d4 C. [Ar] 3d8 D. [Ar] 4s2 3d8 E. [Ar] 4s2 3d6 ------------------------------------------------------------------------------------------------------- 36. Borazine B3N3H6 has been called inorganic benzene. What is the hybridization of H the boron atoms? 40. Which of the following properties do greenhouse gases have? H H N B B N N B H H H A. sp B. sp2 C. sp3 D. sp4 E. dsp3 ------------------------------------------------------------------------------------------------------- (1) They absorb infrared radiation (2) They block ultraviolet radiation from the sun (3) They photodissociate to form pollutant species in the atmosphere A. 1 only B. 2 only C. 3 only D. 1 and 2 E. 2 and 3 ------------------------------------------------------------------------------------------------------- Chem 12, Final Exam, December 14, 2000 Answer Key Form A 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. D B C E E E D B A B A A D B A C D C E B C A A A E A B D D E B A D C E B D E A A ...
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This note was uploaded on 05/24/2009 for the course CHEM 110 taught by Professor Hofmann,brucerob during the Fall '08 term at Pennsylvania State University, University Park.

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