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Chapters 19. Chapters 25. Chapters 12. Chapter 15/16. Chapter 13/14. 1pt. 1 pt. 1 pt. 1pt. 1 pt. 2 pt. 2 pt. 2pt. 2pt. 2 pt. 3 pt. 3 pt. 3 pt. 3 pt. 3 pt. 4 pt. 4 pt. 4pt. 4 pt. 4pt. 5pt. 5 pt. 5 pt. 5 pt. 5 pt. Which compound can act as both

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  1. Chapters 19 Chapters 25 Chapters 12 Chapter 15/16 Chapter 13/14 1pt 1 pt 1 pt 1pt 1 pt 2 pt 2 pt 2pt 2pt 2 pt 3 pt 3 pt 3 pt 3 pt 3 pt 4 pt 4 pt 4pt 4 pt 4pt 5pt 5 pt 5 pt 5 pt 5 pt

  2. Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base? a. water c. sodium hydroxide b. ammonia d. hydrochloric acid

  3. a. water

  4. the carbonate ion is acting as a(n) ___. In the reaction CO32- + H2O HCO3- + OH- a. Arrhenius base c. Bronsted-Lowry base b. Arrhenius acid d. Bronsted-Lowry acid

  5. c. Bronsted-Lowry base

  6. Which reaction illustrates amphoterism? a. H2O + H2O → H3O+ + OH– c. NaCl → Na+ + Cl– b. HCI + H2O → H3O+ + Cl– d. NaOH → Na+ + OH–

  7. a. H2O + H2O → H3O+ + OH–

  8. What are the acids in the following equilibrium reaction? CN- + H2O HCN + OH- a. CN- , H2O c. CN- , OH- b. H2O , HCN d. H2O, OH-

  9. b. H2O , HCN

  10. Which of the following represents a Bronsted-Lowry conjugate acid-base pair? a. SO32- and SO2 c. H3O and H2 b. CO32- and CO d. NH4+ and NH3

  11. d. NH4+ and NH3

  12. Which symbol is used for an alpha particle?

  13. 24He

  14. Which of the following materials is necessary to stop an alpha particle? a. three feet of concrete c. single sheet of aluminum foil b. three inches of lead d. single sheet of paper

  15. d. single sheet of paper

  16. Which of the following materials is necessary to stop a beta particle? a. three feet of concrete c. thin pieces of wood b. three inches of lead d. single sheet of paper

  17. c. thin pieces of wood

  18. Which of the following materials is most effective for stopping gamma radiation? a. several cm of lead c. single sheet of aluminum foil b. on cm of water d. single sheet of paper

  19. a. several cm of lead

  20. The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO2 is formed?

  21. 2.00 g

  22. . When glucose is consumed, it reacts with oxygen in the body to produce carbon dioxide, water, and energy . How many grams of carbon dioxide would be produced if 45 g of C6H12O6 completely reacted with oxygen? C6H12O6 + 6O2>> 6CO2 + 6H2O a. 1.5 g c. 11 g b. 1.8 g d. 66 g

  23. 45 g of C6H12O61 mol of C6H12O66 mol of CO244 g of CO2 = 66 g CO2 180 g of C6H12O6 1 mol of C6H12O6 1 mol of CO2 d. 66 g

  24. How many liters of hydrogen gas are needed to react with CS2 to produce 2.50 L of CH4 at STP? 4H2 (g) + CS2 (l) CH4 (g) + 2H2S(g) a. 2.50 L c. 7.50 L b. 5.00 L d. 10.0 L

  25. 2.50 L of CH41 mol of CH44 mol of H222.4 L of H2 = 10.0 L 22.4 L of CH4 1 mol of CH4 1 mol of H2 d. 10.0 L

  26. Glucose, C6H12O6 , is a good source of food energy. When it reacts with oxygen, carbon dioxide and water are formed. How many liters of CO2 are produced when 126 g of glucose completely react with oxygen? C6H12O6 (s) + 6O2 (g) 6CO2(g)+ 6H2O(l) + 673 kcal a. 4.21 L c. 15.7 L b. 5.33 L d. 94.1 L

  27. 126 g of C6H12O61 mol of C6H12O66 mol of CO222.4 L of CO2= 94.1 L 180 g of C6H12O6 1 mol of C6H12O6 1 mol of CO2 d. 94.1 L

  28. When two substances react to form products, the reactant which is used up is called the __. a. determining reagent c. excess reagent b. limiting reagent d. catalytic reagent

  29. b. limiting reagent

  30. What causes water’s low vapor pressure? a. Dispersion forces c. hydrogen bonding b. Covalent bonding d. ionic attractions

  31. c. hydrogen bonding

  32. The fact that ice is less dense than water is related to the fact that ___. • a. The molecular structure of ice is much less orderly than that of water • b. The molecules of ice are held to each other by covalent bonding • c. Ice has a molecular structure in which water molecules are arranged randomly • d. Ice has a molecular structure that is an open framework held together by hydrogen bonds

  33. d. Ice has a molecular structure that is an open framework held together by hydrogen bonds

  34. . Which of these would you expect to be soluble in the nonpolar solvent carbon disulfide? a. Water c. NaCl b. Carbon tetraiodide d. Stannous iodide

  35. b. Carbon tetraiodide

  36. What type of compound is always an electrolyte? a. Polar covalent c. ionic b. Nonpolar covalent d. network solid

  37. c. ionic

  38. Which symbol is used to connect the formula of the compound with the number of water molecules in a hydrate? a. A parenthesis c. a multiplication symbol b. An asterisk d. a dot

  39. d. a dot

  40. Which law can be used to calculate the number of moles of a contained gas? a. Boyle’s law c. ideal gas law b. combined gas law d. Charles’s law

  41. c. ideal gas law

  42. A box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0˙C. Which of the following statements is true? a. the total pressure in the box is 101kPa b. the partial pressures of N2 and H2 are equal. c. the total pressure is 202 kPa. d. the partial pressure of N2is 101 kPa.

  43. d. the partial pressure of N2is 101 kPa.

  44. If the volume of a container of air is reduced by one-half, what happens to the partial pressure of oxygen within the container? a. it is reduced by one-half. C. it is doubled b. it does not change d. it is reduced by one-fourth

  45. C. it is doubled

  46. . Which of the following gases is the best choice for inflating a balloon that must remain inflated for a long period of time? a. argon c. hydrogen b. oxygen d. neon

  47. c. hydrogen

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