Chemistry 106 Fall 2006 Exam 1 Form A 1. Does this molecule have both cis and trans isomers?

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1 1. Does this molecule have both cis and trans isomers? Cl A. No, it has only the cis isomer. B. Yes, this is the cis isomer. C. Yes, this is the trans isomer. D. No. E. No, it has only the trans isomer 2. The attractive forces between hydrocarbons tend to be dominated by A. London dispersion forces. B. dipole-dipole interactions. C. ion-ion interactions D. ion-dipole interactions. E. hydrogen bonding. 3. Name the compound A. 4-octene B. 3-heptene C. 5-heptene D. 3-octene E. 5-octene 4. What is the systematic name of the following molecule? A. 2,3-dipropyl-4,4,-dimethylpentane B. 2,2-dimethyl-3-sec-pentylhexane C. 1,1,4-trimethyl-3-propylheptane D. 4-tert-butyl-5-methylocatane E. 2,3-dipropyl-4,4-dimethylnonane 5. Which of the following is the chemical formula of pentane? A. CH 3 CH 2 CH 2 CH 2 CH 3 B. CH 3 CH 2 CH 2 CH 3 C. CH 3 CH 3 D. CH 3 CHCHCHCH 2 E. CH 3 CH 2 CH 2 CH 2 CH 2 CH 3 Page 1

2 6. Pick the answer that has the correct names for both of the aromatic hydrocarbons shown below. A. I. xylene II. 1, 3, 4-trimethylbenzene B. I. 1-ethyl-3, 4-dimethylbenzene II. 1, 2, 4-trimethylbenzene C. I. 1-ethyl-3,4-dimethylbenzene II. 1, 3, 4-trimethylbenzene D. I. 1,2-dimethyl-4-ethylbenzene II. 1, 2, 4-trimethylbenzene E. I. ethyldimethylbenzene II. trimethylbenzene 7. Name this molecule. The black spheres represent C and the light grey spheres H. A. cyclopentane B. cyclohexane (boat conformation) C. puckerane D. dodecane E. cyclohexane (chair conformation) Page 2

3 8. Amino acids are the building blocks from which organisms make proteins. Below is a Lewis structure for the amino acid threonine. What organic functional groups does it contain? CH 3 HCOH H 2 N C COH H O A. alcohol B. amine C. carboxylic acid D. b and c E. a, b and c 9. The C-O-C bonding arrangement is called the functional group A. alcohol B. amine C. ether D. ester E. carboxylic acid 10. Which of the following is true about normal alkanes? A. They all contain carbon, hydrogen, and oxygen in consistent ratios. B. Some are gases, some are liquids, and some are solids at room temperature. C. They all exhibit strong hydrogen bonding with one another and with water. D. They all make good lubricants. E. Some are yellow, some are red, and some are blue, depending on the chain length. 11. A pot of water is heated with 10 J of heat at constant pressure. What is the enthalpy change (ΔH) for this process? A. 15 J B. 5 J C. -10 J D. -5 J E. 10 J 12. Indicate which of the following bonds will require the most energy to dissociate. A. C=N B. C-N C. they are all the same. D. there are no trends, so cannot tell without measuring. E. C N Page 3

4 13. For which of the following processes will ΔH be much less than ΔE? A. B. C. D. E. ΔH is much less than ΔE in all cases. 14. Use average bond enthalpies to determine the amount of energy released when 250 g of propane (CH 3 CH 2 CH 3 ) gas are burned. The combustion reaction is CH 3 CH 2 CH 3 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O (g). SOME AVERAGE BOND ENERGIES ARE LISTED BELOW Bond Energy kj/mol Bond Energy kj/mol C-C 348 C=C 612 C-O 360 C=O 743 C-H 413 O-O 146 O=O 497 O-H 463 A kj B kj C X 10 3 kj D kj E. 992 kj 15. A student dissolving some ammonium nitrate (NH 4 NO 3 ) in water notices that the beaker cools as the solid dissolves. This is an example of a(n). A. refrigeration B. combustion reaction C. exothermic process D. endothermic process E. thermodynamic cycle 16. If a book falls off a table, what type of energy does the book possess while it is falling? A. kinetic energy only B. thermal and potential energy C. potential and kinetic energy D. radiant and kinetic energy E. potential energy only Page 4

5 17. Indicate which of the following compounds is most stable relative to its elements. A. H 2 Se (g), ΔH f 0 = 29.7 kj/mol B. SO 2 (g), ΔH f 0 = kj/mol C. O 3 (g), ΔH f 0 = kj/mol D. PbBr 2 (s), ΔH f 0 = kj/mol E. NH 3 (g), ΔH f 0 =-46.1 kj/mol 18. If the enthalpy change in a system is positive, then A. the total enthalpy of the universe increases. B. heat is lost by the system. C. the total energy of the universe decreases. D. the enthalpy change in the surroundings is positive. E. the enthalpy change in the surroundings is negative. 19. Given the enthalpies of formation for the following substances, determine ΔH rxn for Cl 2 (g) + C 2 H 2 Cl 2 (g) + 2 O 2 (g) 2 CO 2 (g) + 4 HCl (g). Substance ΔH 0 f (kj/mol) Cl 2 0 C 2 H 2 Cl HCl CO A kj/mol B kj/mol C kj/mol D kj/mol E kj/mol 20. Use the following reactions to determine ΔH rxn for the reaction of ethylene (C 2 H 4 ) with chlorine (Cl 2 ): H 2 (g) + Cl 2 (g) 2HCl (g); ΔH = kj C (s) + 2Cl 2 (g) CCl 4 (g); ΔH = kj 2C (s) + 2H 2 (g) C 2 H 4 (g); ΔH = 52.3 kj C 2 H 4 (g) + 6Cl 2 (g) 2CCl 4 (g) + 4HCl (g); ΔH =? A kj B kj C kj D kj E kj 21. How much work is done on a gas when it is compressed by a constant pressure of atm from a volume of ml to a volume of ml? A J B J C. 279 J D J E J Page 5

6 22. During a calorimetry experiment, a positive change in temperature corresponds to A. an endothermic reaction. B. an exothermic reaction. C. heat transfer from the calorimeter. D. the enthalpy of formation of the compound being studied. E. none of the above. 23. The heating curves for four different liquids are shown below. Which of the substances has the greatest molar heat capacity? A. V B. III C. II D. I E. IV 24. What is the heat capacity of a calorimeter if the temperature of the calorimeter rises by 5.678ºC when g of benzoic acid was combusted (benzoic acid produces kj of heat when one gram is combusted). A kj/ºc B kj/ºc C kj/ºc D kj/ºc E kj/ºc 25. Which of the following objects will warm the slowest, assuming you supply heat energy at 10.0 J/s and have equal grams of each? A. A container of water (c p = 75.3 J/K mol) B. An iron skillet (c p = 25.1 J/K mol) C. They will all warm at the same rate. D. A copper pot (c p = 24.4 J/K mol) E. An aluminum pan (c p = 24.3 J/K mol) 26. What will be the final temperature of a 10.0 g piece of iron (c p = J/K mol), initially at 25ºC, if it is supplied with 9.5 J from a stove? A. 101ºC B. 23ºC C. 1,356ºC D. 25ºC E. 27ºC Page 6

7 27. A fuel value is A. the energy released when on mole of CO 2 is released. B. the energy released when one gram of a substance is formed (kj/g). C. the amount of energy contained in one mole of a substance (kj/mol). D. the energy released when one gram of a substance is burned (kj/g). E. the cost of energy in kj/$. 28. The function of gasoline additives like ethanol are A. to decrease octane rating. B. to make it less volatile. C. to promote complete combustion. D. to decrease odor. E. none of the above 29. The enthalpy of combustion of sucrose (C 12 H 22 O 11 ) is kj/mol. What is the fuel value of sucrose? A kj/g B kj/g C kj/g D kj/g E x 10-2 kj/g 30. The fraction of crude oil that is used for gasoline consists primarily of normal alkanes. Refineries spend extra money to convert some of these normal alkanes to branched alkanes (raise the octane rating). Why? A. to make the fuel easier to ignite. B. to make the fuel harder to ignite. C. to increase the energy content of the fuel. D. to make the fuel smell better. E. to decrease the energy content of the fuel. 31. Storage of hydrogen for use as a fuel is made difficult by A. its corrosive nature. B. its tendency to undergo nuclear fusion. C. its tendency to make storage tanks float away. D. its high density E. its extremely low boiling point. 32. As plant tissue is converted to coal by heat and pressure deep underground H and O are lost from the material. Thus older coal usually A. contains fewer aromatic rings. B. is lower in energy content. C. is higher in energy content. D. is softer. E. is diamond like. Page 7

8 33. Rank the following according to their fuel values in order of decreasing energy/mass. C 8 H 14, CO, CH 3 OH, CH 3 CH 2 OCH 3 A. C 8 H 14 > CH 3 CH 2 OCH 3 > CH 3 OH > CO B. CO > CH 3 OH > CH 3 CH 2 OCH 3 > C 8 H 14 C. CH 3 CH 2 OCH 3 > CO > CH 3 OH > C 8 H 14 D. C 8 H 14 > CO > CH 3 OH > CH 3 CH 2 OCH 3 E. CO > CH 3 CH 2 OCH 3 > CH 3 OH > C 8 H In fractional distillation of an ideal solution, which component is enriched in the vapor phase? A. the component originally in deficit B. the component originally in excess C. the composition is the same as the liquid phase D. the component with the lower vapor pressure, Pº E. the component with the higher vapor pressure, Pº 35. A polysaccharide is formed from monosaccharides A. through the hydrolysis process. B. by the addition of water molecules at each coupling site. C. that are in their straight-chain form. D. by their reaction to a polymerase. E. through condensation of C-1 and C-4 hydroxyls on adjacent units. 36. In the sketch of the fructose molecule, what organic functional groups are observed? HOCH 2 H H OH C C C C CH 2 OH OH OH H O A. aldehyde and alcohol groups B. ketone and alcohol groups C. alcohol groups D. aldehyde groups E. alcohol and carboxylic acid groups 37. The cyclization reaction of fructose is different from that of glucose because A. the cyclization reaction forms a ketone. B. instead of a six-membered ring a five-membered ring is formed. C. water is released D. the orientation of the cyclization is backward. E. the aldehyde group migrates to a new position. Page 8

9 38. What difference(s) is (are) there in an α-glycosidic bond and a β-glycosidic bond? A. Humans can digest α-glycosidic bonds but not β-glycosidic bonds. B. α-glycosidic bonds occur in starch and β-glycosidic bonds occur in cellulose. C. α-glycosidic bonds involve condensation of α-glucose units via C-1 hydroxyl group of one glucose and C-4 hydroxyl group of another. β-glycosidic bonds link β-glucose units in a similar fashion. D. all the above E. none of the above 39. A g sample of a hydrocarbon (that is, a compound that contains carbon and hydrogen only) is burned in oxygen and the carbon dioxide and water produced carefully collected and weighed. The mass of the carbon dioxide was grams, and the mass of the water was grams. What was the emprical formula of the hydrocarbon? A. C 2 H 6 B. C 6 H 7 C. C 5 H 12 D. C 1 H 6 E. C 5 H Combustion analysis of an organic compound to determine the percentages of carbon, hydrogen, and oxygen in the formula depends on the following assumption(s): A. the mass of the resulting carbon dioxide is equal to the mass of the carbon in the sample. B. the compound burns completely to form carbon dioxide and water. C. all the oxygen in the products comes from the added oxygen gas. D. all the above E. none of the above Page 9

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