Chemistry 1411 Practice Exam 1, Chapters 1-4 Chang

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1 Chemistry 1411 Practice Exam 1, Chapters 1-4 Chang Show your calculations clearly on show work problems. A periodic table is also attached to the end of the exam. Good luck! 1. Give the number of significant figures in the following numbers (2 pts each): a) X 10 2 ml b) mole 2. Carry out the following operations and give your answers with the correct number of significant figures (2 pts each): a) = b) X = 3. Make the following conversions (2 pts each, show all steps): a) 5 ft, 9 in to m (1 in = 2.54 cm) b) 77 F to Kelvin c) 7.92 lb/gal to g/ml (1 lb = g, 1 gal = L)

2 4. When an object claimed to be made of pure gold was immersed in a graduated cylinder containing water, the water level rose from 25.0 ml to 25.8 ml. The mass of the object was 7.1 g. What is the density of the object in grams per ml? (3 pts) 5. (3 pts) Isotopes are atoms that: a) have different atomic numbers b) have the same mass number c) have the same number of protons but different numbers of neutrons d) have different numbers of electrons 6. Which of the following is an extensive property? (3pts) a) volume b) boiling point c) density d) freezing point 7. What is the number of protons, neutrons, and electrons in the nitrogen-14 3 ion? (3 pts) a) 7 protons; 7 neutrons; 7 electrons b) 7 protons; 7 neutrons; 10 electrons c) 8 protons; 6 neutrons; 14 electrons d) 7 protons, 7 neutrons; 4 electrons 8. Which of the following elements is a nonmetal? (3 pts) a) calcium b) sulfur c) zinc d) mercury 9. Which of the following is a transition element? (3 pts) a) Br b) Pb c) Ba d) Os 10. Which of the following elements is a halogen? (3 pts) a) Fe b) K c) Br d) Te 11. Which of the following compounds is a molecular compound? (3 pts) a) barium chloride b) carbon dioxide c) ferric nitrate d) magnesium oxide 12. (3 pts) A set of measurements has good precision if a) the average is close to the true value b) the measurements are in close agreement with each other but are not necessarily correct c) a large number of measurements are made d) a small number of measurements are made

3 13. Name the following compounds (1 pt each): a) CuCl2 b) Li2CO3 c) NO2 (g) d) Na2SO3 14. Write the chemical formulas for the following compounds (1 pt each): a) aluminum oxide b) magnesium phosphate c) iron(iii) bromide d) sulfuric acid 15. Balance the following reactions (2 pts each): a) N2 (g) + H2 (g) NH3 (g) b) Al (s) + HBr (aq) AlBr3 (aq) + H2 (g) c) C8H18 (l) + O2 (g) CO2 (g) + H2O (l) 16. What is the mass percentage of sulfur in Na 2 SO 4? (3 pts) 17. How many moles of Na2SO4 are in 25.0 g of this compound? (3 pts) 18. A compound is 70.57% C, 5.94% H, and 23.49% O. What is the empirical formula of the compound? (3 pts)

4 19. Naturally-occurring copper is composed of 69.17% copper-63 with an atomic weight of amu, and 30.83% of another copper isotope. If the average (weighted average) atomic weight of copper is amu, what is the atomic weight of the other copper isotope? (3 pts) 20. Copper metal reacts with dilute nitric acid according to the following equation: 3Cu (s) + 8HNO3 (aq) 3Cu(NO3)2 (aq) + 2NO (g) + 4H2O (l) If we start with mol of copper metal, how many moles of water will be formed? (3 pts) 21. If 5.00 g of magnesium metal is burned in the presence of excess O2, how many grams of MgO will form? (3 pts)

5 ml of 12.0 M HCl solution is diluted with water to a final volume of 1.00 L. What is the molarity of the diluted solution? (3 pts) a) 3.75 M b) 1.50 M c) M d) M 23. What is the molarity of an NaCl solution prepared by dissolving 9.3 g of NaCl in 350 ml of solution? (3 pts) a) 18 M b) 0.16 M c) 0.45 M d) 27 M 24. How many grams of NaOH are in 500 ml of M NaOH solution? (3 pts) a) 2.19 X 10 3 g b) 114 g c) 14.0 g d) 3.50 g 25. When aqueous solutions of Ba(NO3)2 and K2SO4 are mixed, a precipitate of BaSO4 results. Write the molecular, ionic, and net ionic equation for this double displacement reaction. (6 pts) 26. What is the oxidation state of chlorine in the chlorate ion, ClO3? (3 pts) a) 1 b) +3 c) +5 d) +7

6 27. Based on the equations below, which metal is the most active? (3 pts) Ni(s) + Pb(NO3)2 (aq) Cu(s) + Pb(NO3)2 (aq) Cu(s) + 2Ag(NO3) (aq) Ni(NO3)2 (aq) + Pb(s) No reaction 2Ag(s) + Cu(NO3)2 (aq) a) Ni b) Ag c) Cu d) Pb 28. Calculate the molarity of hydrochloric acid, HCl, in a solution if ml of that solution required ml of M KOH for complete neutralization in a titration. (3 pts) a) M b) M c) M d) M 29. If a copper penny weighs 3.00 g, how many copper atoms are in the penny? (3 pts) 30. Classify the following reactions (combination, decomposition, single displacement, or double displacement). (1 pt each) HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) H2 (g) + CuO (s) Cu (s) + H2O (l) 2 KClO3 (s) 2 KCl (s) + 3 O2 (g) 2 Mg (s) + O2 (g) 2 MgO (s) 31. A compound has the empirical formula CH2 and molecular weight g/mol. What is the molecular formula of the compound? (3 pts)

7 Answers 1. a) 4 b) 5 2. a) 21 b) 1.0 X a) 1.8 m b) 298 K c) g/ml 4. 9 g/ml 5. c 6. a 7. b 8. b 9. d 10. c 11. b 12. b 13. a) copper(ii) chloride or cupric chloride b) lithium carbonate c) nitrogen dioxide d) sodium sulfite 14. a) Al2O3 b) Mg3(PO4)2 c) FeBr3 d) H2SO4 15. a) 1, 3, 2 b) 2, 6, 2, 3 c) 2, 25, 16, % mol 18. C4H4O amu mol H2O g of MgO will form 22. b 23. c

8 24. d 25. Molecular or formula equation: Ba(NO3)2 (aq) + K2SO4 (aq) BaSO4 (s) + 2 KNO3 (aq) Ionic equation: Ba 2+ (aq) + 2 NO3 (aq) + 2 K + (aq) + SO4 2 (aq) BaSO4 (s) + 2 K + (aq) + 2 NO3 (aq) Net ionic equation: Ba 2+ (aq) + SO4 2 (aq) BaSO4 (s) 26. c 27. a 28. c X Cu atoms 30. a) double displacement b) single displacement c) decomposition d) combination 31. C8H16

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