Test Bank For Chemistry And Chemical Reactivity International Edition 8th Edition By John C. Kotz

Chapter 3—Chemical Reactions MULTIPLE CHOICE 1. Nitroglycerin decomposes violently according to the balanced chemical equation below. 2 C3H5(NO3)3( )  3 N2(g) + 1/2 O2(g) + 6 CO2(g) + 5 H2O(g) Which of the following statements concerning this reaction is/are CORRECT? 1. Two moles of nitroglycerine will produce three moles of nitrogen and five moles of water. 2. Four molecules of nitroglycerine will produced one molecule of oxygen and twelve molecules of carbon dioxide. 3. Six grams of nitroglycerine will produce nine grams of nitrogen and fifteen grams of water. a. 1 only b. 2 only c. 3 only d. 1and2 e. 1,2,and3 ANS: D 2. The reaction of tetraphosphorus decaoxide with water produces phosphoric acid. __ P4O10 + __ H2O  __ H3PO4 What are the respective coefficients when the equation is balanced with the smallest integer values? a. 1,1,1 b. 1,3,1 c. 2,4,1 d. 2,6,2 e. 1,6,4 ANS: E 3. When propane undergoes complete combustion, the products are carbon dioxide and water. __ C3H8(g) + __ O2(g)  __ CO2(g) + __ H2O(g) What are the respective coefficients when the equation is balanced with the smallest whole numbers? a. 1,1,1,1 b. 1,3,1,3 c. 1,3,3,1 d. 1,5,3,4 e. 2,5,3,4 ANS: D 4. The reaction of elemental chlorine with potassium iodide yields elemental iodine and potassium chloride. Write a balanced chemical equation for this reaction. a. Cl2(g) + KI(s)  I(s) + KCl2(s) b. Cl2(g) + 2 KI(s)  I2(s) + 2 KCl(s) c. Cl2(g) + KI2(s)  I2(s) + KCl2(s) d. Cl(g) + KI(s)  I(s) + KCl(s) e. Cl2(g) + 2 K2I(s)  I2(s) + 2 K2Cl(s) ANS: B 5. Metals react with oxygen gas to produce oxides with the general formula MxOy. Write a balanced chemical equation for the reaction of titanium with oxygen to yield titanium(IV) oxide. a. 4 Ti(s) + O2(g)  2 Ti2O(s) Kotz CCR 8e Test Bank 1 b. Ti(s) + O2(g)  TiO2(s) c. 2 Ti(s) + O2(g)  2 TiO(s) d. Ti(s) + O(g)  TiO(s) e. 8 Ti(s) + O2(g)  2 Ti4O(s) ANS: B 6. The products of the complete combustion of octane, C8H18, are carbon dioxide and water. Write a balanced chemical equation for this reaction. a. C8H18()8C(s)+9H2(g) b. C8H18( ) + 25 O2(g)8 CO2 (g) + 9 H2O(g) c. 2 C8H18( ) + 25 O2(g)  16 CO2(g) + 18 H2O(g) d. C8H18()+16O2(g)8CO2(g)+9H2(g) e. 2C8H18()+17O2(g)16CO(g)+18H2O(g) ANS: C 7. What is the balanced chemical equation for the complete combustion of benzoic acid, C6H5CO2H, to form carbon dioxide and water? a. C6H5CO2H(s)  6 C(s) + CO2(g) + 3 H2(g) b. C6H5CO2H(s)  7 CO2(g) + 3 H2O(g) c. C6H5CO2H(s) + O2(g)  CO2(g) + H2O(g) d. C6H5CO2H(s) + 8 O2(g)  7 CO2(g) + 3 H2O(g) e. 2 C6H5CO2H(s) + 15 O2(g)  14 CO2(g) + 6 H2O(g) ANS: E 8. Which of the following statements is/are CORRECT? 1. A solution is a homogeneous mixture of two or more substances. 2. A solute is a mixture of a solvent and a soluble compound. 3. Aqueous solutions are solutions in which water is a solvent. a. 1 only b. 2 only c. 3 only d. 1and2 e. 1and3 ANS: E Kotz CCR 8e Test Bank 2 9. Which of the following statements is/are CORRECT? 1. All ionic compounds that are soluble in water are electrolytes. 2. All ionic compounds dissolve in water. 3. Molecular compounds are never soluble in water. a. 1 only b. 2 only c. 3 only d. 1and2 e. 2and3 ANS: A 10. Which of the following statements is/are CORRECT? 1. Water soluble ionic compounds, such as NaCl, are strong electrolytes. 2. Some molecular compounds, such as HCl, are strong electrolytes. 3. Some molecular compounds, such as acetic acid, are weak electrolytes. a. 1 only b. 2 only c. 3 only d. 1and2 e. 1,2,and3 ANS: E 11. Which one of the following compounds is a nonelectrolyte when dissolved in water? a. HCl b. CaCl2 c. CCl4 d. Cu(NO3)2 e. NaCH3CO2 ANS: C 12. Which of the following statements is/are CORRECT? 1. Most ionic compounds containing nitrate ion are soluble in water. 2. Most ionic compounds containing sulfate ion are insoluble in water. 3. Most ionic compounds containing carbonate ion are soluble in water. a. 1 only b. 2 only c. 3 only d. 1and2 e. 1,2,and3 ANS: A Kotz CCR 8e Test Bank 3 13. Which of the following statements is/are CORRECT? 1. Most ionic compounds containing phosphate ion are insoluble in water. 2. Most ionic compounds containing potassium ion are insoluble in water. 3. Most ionic compounds containing hydroxide ion are soluble in water. a. 1 only b. 2 only c. 3 only d. 1and2 e. 1,2,and3 ANS: A 14. Which of the following compounds are soluble in water: K2CO3, CaCO3, NiCO3, and Fe2(CO3)3? a. K2CO3 only b. K2CO3 and CaCO3 c. CaCO3 and NiCO3 d. NiCO3 and Fe2(CO3)3 e. CaCO3, NiCO3, and Fe2(CO3)3 ANS: A 15. Which of the following compounds are soluble in water: NH4NO3, Fe2S3, CuCO3, and SrCl2? a. NH4NO3 only b. NH4NO3 and Fe2S3 c. Fe2S3 and CuCO3 d. CuCO3 and SrCl2 e. NH4NO3 and SrCl2 ANS: E 16. All of the following compounds are insoluble in water except ____. a. BaCO3 b. PbF2 c. Fe(OH)3 d. Ni(ClO4)2 e. PbCrO4 ANS: D 17. A precipitate will form when aqueous Pb(NO3)2 is added to an aqueous solution of ____. a. Cu(NO3)2 b. NaI c. NaCH3CO2 d. Pb(ClO4)2 e. KNO3 ANS: B Kotz CCR 8e Test Bank 4 18. A precipitate will form when aqueous nickel(II) chloride is added to an aqueous solution of ____. a. SrI2 b. Cu(NO3)2 c. KOH d. Na2SO4 e. NaBr ANS: C 19. If an aqueous solution of ____ is added to a mixture of Pb the barium ion will remain in solution. a. NaOH b. Na2SO4 c. K3PO4 d. KCO3 e. Ca(CH3CO2)2 ANS: A 20. If an aqueous solution of ____ is added to a mixture of F but the sulfate ion will remain in solution. a. LiBr b. HNO3 c. Pb(ClO4)2 d. MgNO3 e. AlCl3 2+ and Ba 2+ , the lead ion will precipitate, but ANS: D 21. Write a balanced chemical equation for the reaction of aqueous solutions of sodium sulfide and zinc(II) chloride. a. Na2S(aq) + ZnCl2(aq)  ZnS(s) + 2 NaCl(aq) b. Na2S(aq) + ZnCl2(aq)  ZnS(s) + 2 NaCl(s) c. Na2S(aq) + ZnCl2(aq)  Na2Zn(s) + SCl2(aq) d. Na2S(aq) + ZnCl2(aq)  Na2Zn(aq) + SCl2(g) e. No reaction occurs. ANS: A 22. Write a balanced chemical equation for the reaction of aqueous solutions of magnesium chloride and potassium phosphate. a. MgCl2(aq) + K3PO4(aq)  K3Mg(s) + PO4Cl2(aq) b. 3 MgCl2(aq) + 2 K3PO4(aq)  3 K2Mg(s) + 2 PO4Cl3(aq) c. MgCl(aq) + KPO4(aq)  MgPO4(s) + KCl(aq) d. MgCl2(aq) + 2 KPO4(aq)  Mg(PO4)2(s) + 2 KCl(aq) e. 3 MgCl2(aq) + 2 K3PO4(aq)  Mg3(PO4)2(s) + 6 KCl(aq) ANS: E Kotz CCR 8e Test Bank 5 – 2– and SO4 , the fluoride ion will precipitate, 23. What is the net ionic equation for the reaction of aqueous nickel(II) acetate and aqueous sodium carbonate? 2+ – a. Ni (aq) + 2 CH3CO2 (aq)  Ni(CH3CO2)2(s) +– b. Na (aq) + CH3CO2 (aq)  NaCH3CO2(aq) +– c. Na (aq) + CH3CO2 (aq)  NaCH3CO2(s) d. Ni2+(aq) + CO32–(aq)  NiCO3(s) e. Ni2+(aq) + 2 Na+(aq)  NiNa2(s) ANS: D 24. What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous iron(II) chloride? a. Na+(aq) + OH–(aq)  NaOH(s) b. Na+(aq) + Cl–(aq)  NaCl(s) c. Fe2+(aq) + 2 OH–(aq)  Fe(OH)2(s) d. Fe2+(aq) + OH–(aq)  FeOH+(s) e. Fe2+(aq) + 2 Cl–(aq)  FeCl2(s) ANS: C 25. Which of the following compounds is a weak acid? a. HCl b. H3PO4 c. HNO3 d. HClO4 e. H2SO4 ANS: B 26. Which of the following compounds is a weak base? a. NaOH b. H2CO3 c. LiCl d. NH3 e. CH3CO2H ANS: D 27. Sulfuric acid is the product of the reaction of ____ and H2O. a. SO3 b. SO2 c. S8 d. H2S e. SO42– ANS: A Kotz CCR 8e Test Bank 6 28. Write a balanced equation for the reaction that occurs when hydrogen sulfate ion behaves as a Brønsted-Lowry acid in water. –+ a. HSO4 (aq) + H2O( ) H2SO4(aq) + H3O (aq) 2– –– b. SO4 (aq) + H2O( ) HSO4 (aq) + OH (aq) – 2–+ c. HSO4 (aq) + H2O( ) SO4 (aq) + H3O (aq) d. HSO4–(aq) + H2O( ) H2SO4(aq) + OH–(aq) –+ e. H2SO4(aq) + H2O( ) HSO4 (aq) + H3O (aq) ANS: C 29. What is the balanced equation for carbonate ion (CO32–) acting as a Brønsted base in a reaction with water? a. CO32–(aq) + 3 H2O( ) CO44–(aq) + 2 H3O+(aq) 2– –– b. CO3 (aq) + H2O( ) HCO3 (aq) + OH (aq) c. CO32–(aq) + H2O( ) CO2(g) + 2 OH–(aq) 2– –+ d. CO3 (aq)+2H2O( ) HCO3 (aq)+H3O (aq) e. CO32–(aq) + H2O( ) H2CO42–(aq) ANS: B 30. What is the net ionic equation for the reaction of aqueous hydrochloric acid and aqueous potassium hydroxide? a. HCl(aq) + OH–(aq)  H2O( ) + Cl–(aq) b. Cl–(aq) + K+(aq)  KCl(s) c. HCl(aq) + KOH(aq)  KCl(aq) + H2O( ) d. Cl–(aq) + K+(aq)  KCl(aq) e. H+(aq) + OH–(aq)  H2O( ) ANS: E 31. What are the spectator ions in the reaction between aqueous hydrobromic acid and aqueous sodium hydroxide? a. Na+ only b. H+ and OH– c. Na+ and Br– d. Br– only +–+ – e. H ,Br ,Na ,andOH ANS: C 32. What are the spectator ions in the reaction between aqueous nitric acid and ammonia? a. H+ only b. NO3– only c. H+ and NH4+ –+ d. NO3 and NH4 +–+ e. H,NO3 ,andNH4 ANS: B Kotz CCR 8e Test Bank 7 33. Hydrocyanic acid, HCN, is a weak acid. Write a net ionic equation for the reaction of aqueous hydrocyanic acid and aqueous sodium hydroxide. a. HCN(aq) + NaOH(aq)  Na+(aq) + CN–(aq) + H2O( ) b. HCN(aq) + H2O(aq)  CN–(aq) + H3O+(aq) c. H+(aq) + OH–(aq)  H2O( ) d. HCN(aq) + OH–(aq)  CN–(aq) + H2O( ) e. H+(aq) + NaOH(aq)  Na+(aq) + H2O( ) ANS: D 34. Which of the following compounds will produce a basic solution when dissolved in water? a. CaO b. NaHSO4 c. CO2 d. SO2 e. KCl ANS: A 35. Metal oxides react with water to produce ____. a. bases b. hydrogen gas c. oxygen gas d. acids e. hydronium ions ANS: A 36. Write a balanced net ionic equation for the reaction of calcium sulfide and aqueous nitric acid. a. CaS(s) + 2 H+(aq)  Ca2+(aq) + S2–(aq) + H2(g) b. CaS(s) + 2 H+(aq)  Ca2+(aq) + H2S(g) c. CaS(s) + 2 HNO3(aq)  Ca(NO3)2(aq) + H2S(g) d. CaS(s) + 2 HNO3(aq)  Ca(NO3)2(s) + H2S(s) e. S2(aq) + 2 H+(aq)  H2S(g) ANS: B 37. Write a balanced net ionic equation for the reaction of aqueous solutions of baking soda (NaHCO3) and acetic acid. a. HCO3–(aq) + CH3CO2H(aq)  CH3CO2–(aq) + H2O( ) + CO2(g) b. 2 NaHCO3(aq) + CH3CO2H(aq)  2 Na2CO3(aq) + CH4(aq) + 2H2O( ) + CO2(g) c. NaHCO3(aq) + H+(aq)  H2CO3(s) + Na+(aq) –+ d. HCO3(aq)+H(aq)H2O()+CO2(g) –+ e. HCO3 (aq) + H (aq)  H2CO3(aq) ANS: A Kotz CCR 8e Test Bank 8 38. Write a balanced chemical equation for the reaction of aqueous solutions of ammonium sulfate and sodium hydroxide. a. (NH4)2SO4(aq) b. (NH3)2SO4(aq) c. (NH3)2SO4(aq) d. (NH4)2SO4(aq) e. (NH4)2SO4(aq) ANS: E 39. Which molecule in 2 C2H6(g) + 7 a. C2H6 b. O2 c. H2O d. CO2 e. None + 2 NaOH(aq)  2 NH4OH(aq) + SO3(g) + Na2O(aq) + NaOH(aq)  2 NH3(g) + NaOHSO4(aq) + 2 NaOH(aq)  2 NH3(g) + Na2SO4(aq) + 2 OH(aq) + 2 NaOH(aq)  2 NH4+(g) + Na2SO4(aq) + 2 OH(aq) + 2 NaOH(aq)  2 NH3(g) + 2 H2O( ) + Na2SO4(aq) the reaction below is the oxidizing agent? O2(g)  4 CO2(g) + 6 H2O(g) ANS: B 40. Which species in the reaction below undergoes reduction? H2O(g) + CO(g)  H2(g) + CO2(g) a. H2O b. CO c. H2 d. CO2 e. None ANS: A 41. Which species is reduced in the reaction below? I–(aq) + ClO–(aq)  IO–(aq) + Cl–(aq) a. I– b. H2O c. Cl– d. IO– e. ClO– ANS: E 42. What is the oxidation number of iodine in potassium iodate, KIO3? a. –1 b. 0 c. +3 d. +5 e. +7 ANS: D Kotz CCR 8e Test Bank 9 43. What is the oxidation number of sulfur in sulfur in H2S? a. –2 b. 0 c. +2 d. +4 e. +6 ANS: A 44. What is the oxidation number of each atom in sulfurous acid, H2SO3? a. H=+1,S=–2,O=–2 b. H=0,S=+6,O=–2 c. H=0,S=0,O=0 d. H=+1,S=+4,O=–2 e. H=–1,S=+8,O=–2 ANS: D 45. What is the oxidation number of each atom in sodium hydrogen carbonate, NaHCO3? a. Na=+1,H=–1,C=+6,O=–2 b. Na=+1,H=+1,C=+4,O=–2 c. Na=+1,H=–1,C=+2,O=–2 d. Na=–1,H=+1,C=0,O=–2 e. Na=0,H=0,C=0,O=0 ANS: B 46. Which of the following elements generally acts as an oxidizing agent? a. Br2 b. H2 c. Fe d. C e. Li ANS: A 47. Which of the following chemical equations show oxidation-reduction reactions? 1. Mg(s) + I2(aq)  MgI2(s) 2. Pb(ClO4)2(aq) + 2 KI(aq)  PbI2(s) + 2 KClO4(aq) 3. Fe2O3(s) + 3 CO(g)  2 Fe(s) + 3 CO2(g) a. 1 only b. 2 only c. 1and2 d. 1and3 e. 2and3 ANS: D Kotz CCR 8e Test Bank 10 48. Which of the following chemical equations is an acid-base reaction? a. Ba(OH)2(aq) + K2SO4(aq)  BaSO4(s) + 2 KOH(aq) b. 3 NaOH(aq) + AlCl3(aq)  Al(OH)3(s) + 3 NaCl(aq) c. 2 H+(aq) + Zn(s)  H2(g) + Zn2+(aq) d. 2 HCl(aq) + Pb(NO3)2(aq)  PbCl2(s) + 2 HNO3(aq) + e. H3PO4(aq) + NH3(aq)  NH4 (aq) + H2PO4 (aq) ANS: E 49. All of the following are oxidation-reduction reactions EXCEPT a. CaCO3(s)  CaO(s) + CO2(g) b. 2 Na(s) + Br2(g)  2 NaBr(g) c. Fe(s) + 2 HCl(aq)  FeCl2(aq) + H2(g) d. 2C(s)+O2(g)2CO(g) e. 2 H2O( )2 H2(g) + O2(g) ANS: A SHORT ANSWER 50. A(n) ________ agent loses electrons in an oxidation-reduction reaction. ANS: reducing 51. ________ acid is produced in a larger quantity than any other chemical in the United States. This chemical is used in the production of fertilizers, pigments, alcohol, paper and detergents. ANS: Sulfuric 52. The net ionic equation for the reaction of barium chloride and sodium sulfate is shown below. Ba2+(aq) + SO42–(aq)  BaSO4(s) Chloride and sodium ions are referred to as ________ ions because they are not involved in the reaction. ANS: spectator 53. A solution is a homogeneous mixture composed of one or more ____________ dissolved in a solvent. ANS: solutes Kotz CCR 8e Test Bank 11 54. Give the name of an acidic oxide and write a balanced chemical equation for the reaction of the oxide with water. ANS: Sulfur dioxide. SO2(g) + H2O( )  H2SO3(aq). Other examples include carbon dioxide forming carbonic acid, sulfur trioxide forming sulfuric acid, and nitrogen dioxide forming a mixture of nitrous acid and nitric acid. 55. If an aqueous sodium hydroxide solution is left in contact with air, the concentration of hydroxide ion gradually decreases. The process can be hastened if a person exhales over a sodium hydroxide solution. Write a balanced chemical equation that describes the process by which the hydroxide ion concentration decreases. ANS: OH–(aq) + CO2(aq)  HCO3–(aq) Kotz CCR 8e Test Bank 12