CHEM 1004 Final Exam Spring 2011 (Buckley)
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1 Name CHEM 1004 Final Exam Spring 2011 (Buckley) Multiple choice (2 points each). Circle the letter corresponding to the best answer to each question. You may omit two of the multiple choice questions. To omit a question, write OMIT in big letters across the problem to be omitted. 1. Which of the following is an example of a physical change? a. Water is decomposed by electricity into hydrogen and oxygen. b. A red substance is decomposed by heat to form mercury and oxygen. c. Ice melts at 0 ºC. d. Gasoline is burned to form hydrogen and oxygen. 2. Which of the following is a chemical property? a. Sodium reacts with water to form sodium hydroxide. b. Sugar is a solid at room temperature. c. Salt dissolves in water. d. Oil and water do not mix. 3. Vinegar is composed of approximately 5% acetic acid and 95% water. Which one of the following is the best classification of vinegar? a. pure substance b. homogeneous mixture c. heterogeneous mixture d. compound 4. Refined white table sugar is usually derived from either sugar cane or sugar beets. Regardless of the source of the table sugar, after refining it always has the same composition of carbon, hydrogen and oxygen. Sugar is best classified as which one of the following? a. mixture b. element c. compound d. pure substance 5. The fact that sugar (problem 5) always has the same composition of carbon, hydrogen, and oxygen is an example of which law? a. Law of conservation of mass b. Law of definite proportions c. Law of multiple proportions d. Law of conservation of energy Page 1 of 10
2 6. In the SI system of measurement, the unit of length is the a. kilogram b. meter c. yard d. liter 7. How many cm are in 12.5 m? a cm b cm c cm d cm 8. The prefix milli- means a b. 100 c d How many cg are in mg? a. 895 cg b cg c cg d cg 10. How many ml are in 750 cm 3? a. 750 ml b. 75 ml c ml d ml 11. The density of lead is 11.3 g/cm 3. What mass of lead is required to make a 1 cm 3 fishing sinker? a g b g c g d. 113 g Page 2 of 10
3 12. The symbol X represents an atom that contains: a. 37 protons, 17 neutrons, and 37 electrons b. 17 protons, 37 neutrons, and 17 electrons c. 17 protons, 20 neutrons, and 17 electrons d. 20 protons, 17 neutrons, and 20 electrons 13. The element represented by X in problem 13 is: a. rubidium b. chlorine c. calcium d. xenon 14. The phosphorous atom represented by P contains: a. 15 protons, 16 neutrons, and 18 electrons b. 15 protons, 16 neutrons, and 12 electrons c. 16 protons, 15 neutrons, and 19 electrons d. 16 protons, 15 neutrons, and 13 electrons 15. An example of an alkaline-earth metal is: a. Cs b. Cu c. Pb d. Mg 16. An example of a halogen is: a. O b. C c. Br d. Kr 17. The formula for the phosphate ion is: a. PO 3 2- b. PO 4 3- c. PO 4 2- d. PO The formula for the compound formed between Ba and S is: a. BaS b. Ba 2 S c. BaS 2 d. Ba 2 S The formula for the compound formed between the ammonium ion and P is: a. NH 4 P b. NH 4 P 3 c. (NH 4 ) 3 P d. (NH 3 ) 3 P Page 3 of 10
4 20. The name of the compound Na 2 O is: a. sodium oxide b. disodium oxide c. sodium (I) oxide d. sodium hydroxide 21. The name for the compound N 2 O 5 is: a. nitrogen oxide b. dinitrogen pentoxide c. nitrogen pentoxide d. nitrogen (II) oxide e. dinitrogen trioxide 22. The name for the compound CuCl 2 is: a. copper chloride b. copper dichloride c. copper (I) chloride d. copper (II) chloride 23. How many moles are contained in 51 g of NH 3? a. 3 moles b moles c moles d moles 24. How many atoms are contained in 20 molecules of PF 5? a. 100 atoms b. 6 atoms c. 120 atoms d atoms 25. How many grams are contained in 6.5 moles of CaBr 2? a. 6.5 g CaBr 2 b g CaBr 2 c g CaBr 2 d g CaBr 2 Page 4 of 10
5 26. What is the missing particle in the following equation? K? Cl He a. b. c. d e p p n 27. A radioactive isotope decays to give an alpha particle and bismuth-211. What was the original nucleus? a. b. c. d At Rn Bi Fr 28. A particular isotope decays with a half-life of 25 years. What fraction of the isotope will remain after 100 years of decay? a. one-half of the original amount of isotope b. one-fourth of the original amount of isotope c. one-eighth of the original amount of isotope d. one-sixteenth of the original amount of isotope 29. A gas is originally confined to a 15.0-L container at a pressure of 4.0-atm and a temperature of 250 ºC. If the volume of the container is changed to 30.0-L and the pressure changes to 8.0-atm, what is the new temperature of the container? a K b K c ºC d ºC 30. A party balloon filled with helium has a volume of 8.0-L and a pressure of 1.5-atm at a temperature of 25 ºC. How many moles of helium are contained in this balloon? a. 2.0 moles of helium b. 0.5 moles of helium c moles of helium d. 5.8 moles of helium Page 5 of 10
6 31. Which of the following species is an acid? a. NaOH b. BaO c. NH 3 d. HNO The ph of which of the following solutions would be greater than 7? a. HC 2 H 3 O 2 b. KOH c. HBr d. H 2 SO The formula for the salt made between the reaction of HBr with Sr(OH) 2 would be a. H 2 O b. SrBr c. SrBr 2 d. SrBr If the ph of a solution is 6.0, the concentration of H + is equal to a M b M c M d M 35. If the ph of a solution is 8.5, the H + concentration is between a M and M b M and M c M and M d M and M 36. In which of the reactions below (not written as complete reactions) is the reactant oxidized? a. Fe 3+ Fe 2+ b. Cr 3+ Cr c. O 2 O 2- d. Al Al What is the oxidizing agent in the following reaction? 2 Na (s) + Cl 2 (g) 2NaCl (s) a. Na b. Cl 2 c. NaCl d. can t tell from the information given Page 6 of 10
7 Short answer problems. You do not get to omit any of these. 38. (6 points) For each of the following species: a. Draw the Lewis structure b. Place an X in the box below each that corresponds to an intermolecular force that species would exhibit. Species: CBr 3 H CO 2 NH 2 Cl Lewis structure: Place an X in each box below that corresponds to an intermolecular force each compound would experience. dispersion dipole-dipole H-bonding 39. (6 points) Consider the following reaction (show your work): N 2 (g) + 3 H 2 (g) 2 NH 3 (g) a. If one starts with 56.0-g of N 2, how many grams of NH 3 could be produced? b. How many grams of H 2 would be required to react with the 56.0-g of N 2 from part a? Page 7 of 10
8 40. (4 points) A company markets a device it calls a water eneroxizer. The device is claimed to supply so much energy to drinking water that the mass of oxygen is increased, thereby providing more oxygen to the body. Apply information you have gained this semester along with the FLaReS principles (falsifiability, logic, reproducibility, and sufficiency) to evaluate this claim. Page 8 of 10
9 Potentially Useful Information Avogadro s number: Gas Laws: PV T PV T PV nrt L atm R mol K Page 9 of 10
10 Page 10 of 10
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