{"id":154,"date":"2016-01-11T19:59:35","date_gmt":"2016-01-11T19:59:35","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistryclone\/chapter\/end-of-chapter-material-20\/"},"modified":"2019-08-23T20:51:58","modified_gmt":"2019-08-23T20:51:58","slug":"end-of-chapter-4-material","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistryclone\/chapter\/end-of-chapter-4-material\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"
\r\n

Additional Exercises<\/p>\r\n\r\n<\/header>\r\n

\r\n
    \r\n \t
  1. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the boiling of water, including the proper phase labels.<\/li>\r\n \t
  2. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the freezing of water, including the proper phase labels.<\/li>\r\n \t
  3. Explain why 4Na(s) + 2Cl2<\/sub>(g) \u2192 4NaCl(s) should not be considered a proper chemical equation.<\/li>\r\n \t
  4. Explain why H2<\/sub>(g) + \u00bdO2<\/sub>(g) \u2192 H2<\/sub>O(\u2113) should not be considered a proper chemical equation.<\/li>\r\n \t
  5. Does the chemical reaction represented by 3Zn(s) + 2Al(NO3<\/sub>)3<\/sub>(aq) \u2192 3Zn(NO3<\/sub>)2<\/sub>(aq) + 2Al(s) proceed as written? Why or why not?<\/li>\r\n \t
  6. Does the chemical reaction represented by 2Au(s) + 2HNO3<\/sub>(aq) \u2192 2AuNO3<\/sub>(aq) + H2<\/sub>(g) proceed as written? Gold is a relatively useful metal for certain applications, such as jewellry and electronics. Does your answer suggest why this is so?<\/li>\r\n \t
  7. Explain what is wrong with the double-replacement reaction\r\nNaCl(aq) + KBr(aq) \u2192 NaK(aq) + ClBr(aq).<\/li>\r\n \t
  8. Predict the products of and balance the double-replacement reaction Ag2<\/sub>SO4<\/sub>(aq) + SrCl2<\/sub>(aq) \u2192 ?<\/li>\r\n \t
  9. Write the complete and net ionic equations for the double-replacement reaction\r\nBaCl2<\/sub>(aq) + Ag2<\/sub>SO4<\/sub>(aq) \u2192 ?<\/li>\r\n \t
  10. Write the complete and net ionic equations for the double-replacement reaction\r\nAg2<\/sub>SO4<\/sub>(aq) + SrCl2<\/sub>(aq) \u2192 ?<\/li>\r\n \t
  11. Identify the spectator ions in the reaction NaCl(aq) + KBr(aq) \u2192 NaBr(aq) + KCl(aq). What is the net ionic equation?<\/li>\r\n \t
  12. Complete the reaction 3H2<\/sub>SO4<\/sub>(aq) + 2Al(OH)3<\/sub>(s) \u2192 ? and identify the spectator ions. What is the net ionic equation?<\/li>\r\n \t
  13. Can a reaction be a composition reaction and a redox reaction at the same time? Give an example to support your answer.<\/li>\r\n \t
  14. Can a reaction be a combustion reaction and a redox reaction at the same time? Give an example to support your answer.<\/li>\r\n \t
  15. Can a reaction be a decomposition reaction and a redox reaction at the same time? Give an example to support your answer.<\/li>\r\n \t
  16. Can a reaction be a combustion reaction and a double-replacement reaction at the same time? Give an example to support your answer.<\/li>\r\n \t
  17. Why is CH4<\/sub> not normally considered an acid?<\/li>\r\n \t
  18. Methyl alcohol has the formula CH3<\/sub>OH. Why would methyl alcohol not normally be considered a base?<\/li>\r\n \t
  19. What are the oxidation numbers of the nitrogen atoms in these substances?\r\n
      \r\n \t
    1. N2<\/sub><\/li>\r\n \t
    2. NH3<\/sub><\/li>\r\n \t
    3. NO<\/li>\r\n \t
    4. N2<\/sub>O<\/li>\r\n \t
    5. NO2<\/sub><\/li>\r\n \t
    6. N2<\/sub>O4<\/sub><\/li>\r\n \t
    7. N2<\/sub>O5<\/sub><\/li>\r\n \t
    8. NaNO3<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
    9. What are the oxidation numbers of the sulfur atoms in these substances?\r\n
        \r\n \t
      1. SF6<\/sub><\/li>\r\n \t
      2. Na2<\/sub>SO4<\/sub><\/li>\r\n \t
      3. K2<\/sub>SO3<\/sub><\/li>\r\n \t
      4. SO3<\/sub><\/li>\r\n \t
      5. SO2<\/sub><\/li>\r\n \t
      6. S8<\/sub><\/li>\r\n \t
      7. Na2<\/sub>S<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
      8. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating in 2CuCl(aq) \u2192 CuCl2<\/sub>(aq) + Cu(s) and indicate the initial and final oxidation numbers of that element.<\/li>\r\n \t
      9. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating in\r\n3Cl2<\/sub>(g) + 6OH\u2212<\/sup>(aq) \u2192 5Cl\u2212<\/sup>(aq) + ClO3<\/sub>\u2212<\/sup>(aq) + 3H2<\/sub>O(\u2113) and indicate the initial and final oxidation numbers of that element.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
        \r\n

        Answers<\/p>\r\n\r\n<\/header>\r\n

        \r\n
          \r\n \t
        1. H2<\/sub>O(\u2113) \u2192 H2<\/sub>O(g)<\/li>\r\n<\/ol>\r\n
            \r\n \t
          1. The coefficients are not in their lowest whole-number ratio.<\/li>\r\n<\/ol>\r\n
              \r\n \t
            1. No; zinc is lower in the activity series than aluminum.<\/li>\r\n<\/ol>\r\n
                \r\n \t
              1. In the products, the cation is pairing with the cation, and the anion is pairing with the anion.<\/li>\r\n<\/ol>\r\n
                  \r\n \t
                1. Complete ionic equation: Ba2+<\/sup>(aq) + 2Cl\u2212<\/sup>(aq) + 2Ag+<\/sup>(aq) + SO4<\/sub>2\u2212<\/sup>(aq) \u2192 BaSO4<\/sub>(s) + 2AgCl(s)\r\n\r\nNet ionic equation: The net ionic equation is the same as the complete ionic equation.<\/li>\r\n<\/ol>\r\n
                    \r\n \t
                  1. Each ion is a spectator ion; there is no overall net ionic equation.<\/li>\r\n<\/ol>\r\n
                      \r\n \t
                    1. Yes; H2<\/sub> + Cl2<\/sub> \u2192 2HCl (answers will vary)<\/li>\r\n<\/ol>\r\n
                        \r\n \t
                      1. Yes; 2HCl \u2192 H2<\/sub> + Cl2<\/sub> (answers will vary)<\/li>\r\n<\/ol>\r\n
                          \r\n \t
                        1. It does not increase the H+<\/sup> ion concentration; it is not a compound of H+<\/sup>.<\/li>\r\n<\/ol>\r\n
                            \r\n \t
                          1. \r\n
                              \r\n \t
                            1. 0<\/li>\r\n \t
                            2. \u22123<\/li>\r\n \t
                            3. +2<\/li>\r\n \t
                            4. +1<\/li>\r\n \t
                            5. +4<\/li>\r\n \t
                            6. +4<\/li>\r\n \t
                            7. +5<\/li>\r\n \t
                            8. +5<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n
                                \r\n \t
                              1. Copper is disproportionating. Initially, its oxidation number is +1; in the products, its oxidation numbers are +2 and 0, respectively.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>","rendered":"
                                \n
                                \n

                                Additional Exercises<\/p>\n<\/header>\n

                                \n
                                  \n
                                1. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the boiling of water, including the proper phase labels.<\/li>\n
                                2. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the freezing of water, including the proper phase labels.<\/li>\n
                                3. Explain why 4Na(s) + 2Cl2<\/sub>(g) \u2192 4NaCl(s) should not be considered a proper chemical equation.<\/li>\n
                                4. Explain why H2<\/sub>(g) + \u00bdO2<\/sub>(g) \u2192 H2<\/sub>O(\u2113) should not be considered a proper chemical equation.<\/li>\n
                                5. Does the chemical reaction represented by 3Zn(s) + 2Al(NO3<\/sub>)3<\/sub>(aq) \u2192 3Zn(NO3<\/sub>)2<\/sub>(aq) + 2Al(s) proceed as written? Why or why not?<\/li>\n
                                6. Does the chemical reaction represented by 2Au(s) + 2HNO3<\/sub>(aq) \u2192 2AuNO3<\/sub>(aq) + H2<\/sub>(g) proceed as written? Gold is a relatively useful metal for certain applications, such as jewellry and electronics. Does your answer suggest why this is so?<\/li>\n
                                7. Explain what is wrong with the double-replacement reaction
                                  \nNaCl(aq) + KBr(aq) \u2192 NaK(aq) + ClBr(aq).<\/li>\n
                                8. Predict the products of and balance the double-replacement reaction Ag2<\/sub>SO4<\/sub>(aq) + SrCl2<\/sub>(aq) \u2192 ?<\/li>\n
                                9. Write the complete and net ionic equations for the double-replacement reaction
                                  \nBaCl2<\/sub>(aq) + Ag2<\/sub>SO4<\/sub>(aq) \u2192 ?<\/li>\n
                                10. Write the complete and net ionic equations for the double-replacement reaction
                                  \nAg2<\/sub>SO4<\/sub>(aq) + SrCl2<\/sub>(aq) \u2192 ?<\/li>\n
                                11. Identify the spectator ions in the reaction NaCl(aq) + KBr(aq) \u2192 NaBr(aq) + KCl(aq). What is the net ionic equation?<\/li>\n
                                12. Complete the reaction 3H2<\/sub>SO4<\/sub>(aq) + 2Al(OH)3<\/sub>(s) \u2192 ? and identify the spectator ions. What is the net ionic equation?<\/li>\n
                                13. Can a reaction be a composition reaction and a redox reaction at the same time? Give an example to support your answer.<\/li>\n
                                14. Can a reaction be a combustion reaction and a redox reaction at the same time? Give an example to support your answer.<\/li>\n
                                15. Can a reaction be a decomposition reaction and a redox reaction at the same time? Give an example to support your answer.<\/li>\n
                                16. Can a reaction be a combustion reaction and a double-replacement reaction at the same time? Give an example to support your answer.<\/li>\n
                                17. Why is CH4<\/sub> not normally considered an acid?<\/li>\n
                                18. Methyl alcohol has the formula CH3<\/sub>OH. Why would methyl alcohol not normally be considered a base?<\/li>\n
                                19. What are the oxidation numbers of the nitrogen atoms in these substances?\n
                                    \n
                                  1. N2<\/sub><\/li>\n
                                  2. NH3<\/sub><\/li>\n
                                  3. NO<\/li>\n
                                  4. N2<\/sub>O<\/li>\n
                                  5. NO2<\/sub><\/li>\n
                                  6. N2<\/sub>O4<\/sub><\/li>\n
                                  7. N2<\/sub>O5<\/sub><\/li>\n
                                  8. NaNO3<\/sub><\/li>\n<\/ol>\n<\/li>\n
                                  9. What are the oxidation numbers of the sulfur atoms in these substances?\n
                                      \n
                                    1. SF6<\/sub><\/li>\n
                                    2. Na2<\/sub>SO4<\/sub><\/li>\n
                                    3. K2<\/sub>SO3<\/sub><\/li>\n
                                    4. SO3<\/sub><\/li>\n
                                    5. SO2<\/sub><\/li>\n
                                    6. S8<\/sub><\/li>\n
                                    7. Na2<\/sub>S<\/li>\n<\/ol>\n<\/li>\n
                                    8. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating in 2CuCl(aq) \u2192 CuCl2<\/sub>(aq) + Cu(s) and indicate the initial and final oxidation numbers of that element.<\/li>\n
                                    9. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating in
                                      \n3Cl2<\/sub>(g) + 6OH\u2212<\/sup>(aq) \u2192 5Cl\u2212<\/sup>(aq) + ClO3<\/sub>\u2212<\/sup>(aq) + 3H2<\/sub>O(\u2113) and indicate the initial and final oxidation numbers of that element.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n
                                      \n
                                      \n

                                      Answers<\/p>\n<\/header>\n

                                      \n
                                        \n
                                      1. H2<\/sub>O(\u2113) \u2192 H2<\/sub>O(g)<\/li>\n<\/ol>\n
                                          \n
                                        1. The coefficients are not in their lowest whole-number ratio.<\/li>\n<\/ol>\n
                                            \n
                                          1. No; zinc is lower in the activity series than aluminum.<\/li>\n<\/ol>\n
                                              \n
                                            1. In the products, the cation is pairing with the cation, and the anion is pairing with the anion.<\/li>\n<\/ol>\n
                                                \n
                                              1. Complete ionic equation: Ba2+<\/sup>(aq) + 2Cl\u2212<\/sup>(aq) + 2Ag+<\/sup>(aq) + SO4<\/sub>2\u2212<\/sup>(aq) \u2192 BaSO4<\/sub>(s) + 2AgCl(s)\n

                                                Net ionic equation: The net ionic equation is the same as the complete ionic equation.<\/li>\n<\/ol>\n

                                                  \n
                                                1. Each ion is a spectator ion; there is no overall net ionic equation.<\/li>\n<\/ol>\n
                                                    \n
                                                  1. Yes; H2<\/sub> + Cl2<\/sub> \u2192 2HCl (answers will vary)<\/li>\n<\/ol>\n
                                                      \n
                                                    1. Yes; 2HCl \u2192 H2<\/sub> + Cl2<\/sub> (answers will vary)<\/li>\n<\/ol>\n
                                                        \n
                                                      1. It does not increase the H+<\/sup> ion concentration; it is not a compound of H+<\/sup>.<\/li>\n<\/ol>\n
                                                          \n
                                                        1. \n
                                                            \n
                                                          1. 0<\/li>\n
                                                          2. \u22123<\/li>\n
                                                          3. +2<\/li>\n
                                                          4. +1<\/li>\n
                                                          5. +4<\/li>\n
                                                          6. +4<\/li>\n
                                                          7. +5<\/li>\n
                                                          8. +5<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n
                                                              \n
                                                            1. Copper is disproportionating. Initially, its oxidation number is +1; in the products, its oxidation numbers are +2 and 0, respectively.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n","protected":false},"author":124,"menu_order":7,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-154","chapter","type-chapter","status-publish","hentry"],"part":130,"_links":{"self":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/154","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/users\/124"}],"version-history":[{"count":4,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/154\/revisions"}],"predecessor-version":[{"id":1324,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/154\/revisions\/1324"}],"part":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/parts\/130"}],"metadata":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/154\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/media?parent=154"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapter-type?post=154"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/contributor?post=154"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/license?post=154"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}