{"id":313,"date":"2017-12-14T21:32:32","date_gmt":"2017-12-14T21:32:32","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/end-of-chapter-material-6\/"},"modified":"2017-12-14T21:32:32","modified_gmt":"2017-12-14T21:32:32","slug":"end-of-chapter-material-6","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-introductory-chemistry\/chapter\/end-of-chapter-material-6\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"
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Additional Exercises<\/h3>\n\u00a0\n
  1. \n
    \n

    What is the work when 124 mL of gas contract to 72.0 mL under an external pressure of 822 torr?<\/p>\n\n<\/div><\/li>\n\t

  2. \n
    \n

    What is the work when 2,345 mL of gas contract to 887 mL under an external pressure of 348 torr?<\/p>\n\n<\/div><\/li>\n\t

  3. \n
    \n

    A 3.77 L volume of gas is exposed to an external pressure of 1.67 atm. As the gas contracts, 156 J of work are added to the gas. What is the final volume of the gas?<\/p>\n\n<\/div><\/li>\n\t

  4. \n
    \n

    A 457 mL volume of gas contracts when 773 torr of external pressure act on it. If 27.4 J of work are added to the gas, what is its final volume?<\/p>\n\n<\/div><\/li>\n\t

  5. \n
    \n

    What is the heat when 1,744 g of Hg increase in temperature by 334\u00b0C? Express your final answer in kJ.<\/p>\n\n<\/div><\/li>\n\t

  6. \n
    \n

    What is the heat when 13.66 kg of Fe cool by 622\u00b0C? Express your final answer in kJ.<\/p>\n\n<\/div><\/li>\n\t

  7. \n
    \n

    What is final temperature when a 45.6 g sample of Al at 87.3\u00b0C gains 188 J of heat?<\/p>\n\n<\/div><\/li>\n\t

  8. \n
    \n

    What is final temperature when 967 g of Au at 557\u00b0C lose 559 J of heat?<\/p>\n\n<\/div><\/li>\n\t

  9. \n
    \n

    Plants take CO2<\/sub> and H2<\/sub>O and make glucose (C6<\/sub>H12<\/sub>O6<\/sub>) and O2<\/sub>. Write a balanced thermochemical equation for this process. Use data in Table 7.2 \"Enthalpies of Formation for Various Substances\"<\/a>.<\/p>\n\n<\/div><\/li>\n\t

  10. \n
    \n

    Exercise 9 described the formation of glucose in plants, which take in CO2<\/sub> and H2<\/sub>O and give off O2<\/sub>. Is this process exothermic or endothermic? If exothermic, where does the energy go? If endothermic, where does the energy come from?<\/p>\n\n<\/div><\/li>\n\t

  11. \n
    \n

    The basic reaction in the refining of aluminum is to take Al2<\/sub>O3<\/sub>(s) and turn it into Al(s) and O2<\/sub>(g). Write the balanced thermochemical equation for this process. Use data in Table 7.2 \"Enthalpies of Formation for Various Substances\"<\/a>.<\/p>\n\n<\/div><\/li>\n\t

  12. \n
    \n

    Is the enthalpy change of the reaction<\/p>\nH2<\/sub>O(\u2113) \u2192\u00a0H2<\/sub>O(g)<\/span><\/span>\n

    zero or nonzero? Use data in Table 7.2 \"Enthalpies of Formation for Various Substances\"<\/a> to determine the answer.<\/p>\n\n<\/div><\/li>\n\t

  13. \n
    \n

    What mass of H2<\/sub>O can be heated from 22\u00b0C to 80\u00b0C in the combustion of 1 mol of CH4<\/sub>? You will need the balanced thermochemical equation for the combustion of CH4<\/sub>. Use data in Table 7.2 \"Enthalpies of Formation for Various Substances\"<\/a>.<\/p>\n\n<\/div><\/li>\n\t

  14. \n
    \n

    What mass of H2<\/sub>O can be heated from 22\u00b0C to 80\u00b0C in the combustion of 1 mol of C2<\/sub>H6<\/sub>? You will need the balanced thermochemical equation for the combustion of C2<\/sub>H6<\/sub>. Use data in Table 7.2 \"Enthalpies of Formation for Various Substances\"<\/a>. Compare your answer to Exercise 13.<\/p>\n\n<\/div><\/li>\n\t

  15. \n
    \n

    What is the enthalpy change for the unknown reaction?<\/p>\nPb(s) +\u00a0Cl2<\/sub>(g) \u2192\u00a0PbCl2<\/sub>(s) \u0394H<\/em>\u00a0=\u00a0\u2212359 kJ<\/span><\/span>\nPbCl2<\/sub>(s) +\u00a0Cl2<\/sub>(g) \u2192\u00a0PbCl4<\/sub>(\u2113) \u0394H<\/em>\u00a0=\u00a0?<\/span><\/span>\nPb(s) +\u00a02 Cl2<\/sub>(g) \u2192\u00a0PbCl4<\/sub>(\u2113) \u0394H<\/em>\u00a0=\u00a0\u2212329 kJ<\/span><\/span>\n\n<\/div><\/li>\n\t

  16. \n
    \n

    What is the enthalpy change for the unknown reaction?<\/p>\nP(s) +\u00a03\/2 Br2<\/sub>(\u2113) \u2192\u00a0PBr3<\/sub>(\u2113) \u0394H<\/em>\u00a0=\u00a0\u2212185 kJ<\/span><\/span>\nPI3<\/sub>(s) \u2192\u00a0P(s) +\u00a03\/2 I2<\/sub>(s) \u0394H<\/em>\u00a0=\u00a0?<\/span><\/span>\nPI3<\/sub>(s) +\u00a03\/2 Br2<\/sub>(\u2113) \u2192\u00a0PBr3<\/sub>(\u2113) +\u00a03\/2 I2<\/sub>(s) \u0394H<\/em>\u00a0=\u00a0\u2212139 kJ<\/span><\/span>\n\n<\/div><\/li>\n\t

  17. \n
    \n

    What is the \u0394H<\/em> for this reaction? The label gra<\/em> means graphite, and the label dia<\/em> means diamond. What does your answer mean?<\/p>\nC(s, gra) \u2192\u00a0C(s, dia)<\/span><\/span>\n\n<\/div><\/li>\n\t

  18. \n
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    Without consulting any tables, determine the \u0394H<\/em> for this reaction. Explain your answer.<\/p>\nH2<\/sub>O(\u2113, 25\u00b0C) \u2192\u00a0H2<\/sub>O(\u2113, 25\u00b0C)<\/span><\/span>\n\n<\/div><\/li>\n<\/ol><\/div>\n

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    Answers<\/h3>\n
    \n\n1.<\/strong>\n\n5.70 J\n\n3.<\/strong>\n\n4.69 L\n\n5.<\/strong>\n\n80.97 kJ\n\n7.<\/strong>\n\n91.9\u00b0C\n\n9.<\/strong>\n\n6 CO2<\/sub>(g) +\u00a06 H2<\/sub>O(\u2113) \u2192\u00a0C6<\/sub>H12<\/sub>O6<\/sub>(s) +\u00a06 O2<\/sub>(g) \u0394H<\/em>\u00a0=\u00a02,799 kJ\n\n11.<\/strong>\n\n2 Al2<\/sub>O3<\/sub>(s) \u2192\u00a04 Al(s) +\u00a03 O2<\/sub>(g) \u0394H<\/em>\u00a0=\u00a03351.4 kJ\n\n13.<\/strong>\n\n3,668 g\n\n15.<\/strong>\n\n\u0394H<\/em>\u00a0=\u00a030 kJ\n\n17.<\/strong>\n\n\u0394H<\/em>\u00a0=\u00a01.897 kJ; the reaction is endothermic.\n\n<\/div>\n<\/div>\n\u00a0\n\n<\/div>\n<\/div>\n<\/div>","rendered":"
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    Additional Exercises<\/h3>\n

    \u00a0<\/p>\n

      \n
    1. \n
      \n

      What is the work when 124 mL of gas contract to 72.0 mL under an external pressure of 822 torr?<\/p>\n<\/div>\n<\/li>\n

    2. \n
      \n

      What is the work when 2,345 mL of gas contract to 887 mL under an external pressure of 348 torr?<\/p>\n<\/div>\n<\/li>\n

    3. \n
      \n

      A 3.77 L volume of gas is exposed to an external pressure of 1.67 atm. As the gas contracts, 156 J of work are added to the gas. What is the final volume of the gas?<\/p>\n<\/div>\n<\/li>\n

    4. \n
      \n

      A 457 mL volume of gas contracts when 773 torr of external pressure act on it. If 27.4 J of work are added to the gas, what is its final volume?<\/p>\n<\/div>\n<\/li>\n

    5. \n
      \n

      What is the heat when 1,744 g of Hg increase in temperature by 334\u00b0C? Express your final answer in kJ.<\/p>\n<\/div>\n<\/li>\n

    6. \n
      \n

      What is the heat when 13.66 kg of Fe cool by 622\u00b0C? Express your final answer in kJ.<\/p>\n<\/div>\n<\/li>\n

    7. \n
      \n

      What is final temperature when a 45.6 g sample of Al at 87.3\u00b0C gains 188 J of heat?<\/p>\n<\/div>\n<\/li>\n

    8. \n
      \n

      What is final temperature when 967 g of Au at 557\u00b0C lose 559 J of heat?<\/p>\n<\/div>\n<\/li>\n

    9. \n
      \n

      Plants take CO2<\/sub> and H2<\/sub>O and make glucose (C6<\/sub>H12<\/sub>O6<\/sub>) and O2<\/sub>. Write a balanced thermochemical equation for this process. Use data in Table 7.2 “Enthalpies of Formation for Various Substances”<\/a>.<\/p>\n<\/div>\n<\/li>\n

    10. \n
      \n

      Exercise 9 described the formation of glucose in plants, which take in CO2<\/sub> and H2<\/sub>O and give off O2<\/sub>. Is this process exothermic or endothermic? If exothermic, where does the energy go? If endothermic, where does the energy come from?<\/p>\n<\/div>\n<\/li>\n

    11. \n
      \n

      The basic reaction in the refining of aluminum is to take Al2<\/sub>O3<\/sub>(s) and turn it into Al(s) and O2<\/sub>(g). Write the balanced thermochemical equation for this process. Use data in Table 7.2 “Enthalpies of Formation for Various Substances”<\/a>.<\/p>\n<\/div>\n<\/li>\n

    12. \n
      \n

      Is the enthalpy change of the reaction<\/p>\n

      H2<\/sub>O(\u2113) \u2192\u00a0H2<\/sub>O(g)<\/span><\/span><\/p>\n

      zero or nonzero? Use data in Table 7.2 “Enthalpies of Formation for Various Substances”<\/a> to determine the answer.<\/p>\n<\/div>\n<\/li>\n

    13. \n
      \n

      What mass of H2<\/sub>O can be heated from 22\u00b0C to 80\u00b0C in the combustion of 1 mol of CH4<\/sub>? You will need the balanced thermochemical equation for the combustion of CH4<\/sub>. Use data in Table 7.2 “Enthalpies of Formation for Various Substances”<\/a>.<\/p>\n<\/div>\n<\/li>\n

    14. \n
      \n

      What mass of H2<\/sub>O can be heated from 22\u00b0C to 80\u00b0C in the combustion of 1 mol of C2<\/sub>H6<\/sub>? You will need the balanced thermochemical equation for the combustion of C2<\/sub>H6<\/sub>. Use data in Table 7.2 “Enthalpies of Formation for Various Substances”<\/a>. Compare your answer to Exercise 13.<\/p>\n<\/div>\n<\/li>\n

    15. \n
      \n

      What is the enthalpy change for the unknown reaction?<\/p>\n

      Pb(s) +\u00a0Cl2<\/sub>(g) \u2192\u00a0PbCl2<\/sub>(s) \u0394H<\/em>\u00a0=\u00a0\u2212359 kJ<\/span><\/span>
      \nPbCl2<\/sub>(s) +\u00a0Cl2<\/sub>(g) \u2192\u00a0PbCl4<\/sub>(\u2113) \u0394H<\/em>\u00a0=\u00a0?<\/span><\/span>
      \nPb(s) +\u00a02 Cl2<\/sub>(g) \u2192\u00a0PbCl4<\/sub>(\u2113) \u0394H<\/em>\u00a0=\u00a0\u2212329 kJ<\/span><\/span><\/p>\n<\/div>\n<\/li>\n

    16. \n
      \n

      What is the enthalpy change for the unknown reaction?<\/p>\n

      P(s) +\u00a03\/2 Br2<\/sub>(\u2113) \u2192\u00a0PBr3<\/sub>(\u2113) \u0394H<\/em>\u00a0=\u00a0\u2212185 kJ<\/span><\/span>
      \nPI3<\/sub>(s) \u2192\u00a0P(s) +\u00a03\/2 I2<\/sub>(s) \u0394H<\/em>\u00a0=\u00a0?<\/span><\/span>
      \nPI3<\/sub>(s) +\u00a03\/2 Br2<\/sub>(\u2113) \u2192\u00a0PBr3<\/sub>(\u2113) +\u00a03\/2 I2<\/sub>(s) \u0394H<\/em>\u00a0=\u00a0\u2212139 kJ<\/span><\/span><\/p>\n<\/div>\n<\/li>\n

    17. \n
      \n

      What is the \u0394H<\/em> for this reaction? The label gra<\/em> means graphite, and the label dia<\/em> means diamond. What does your answer mean?<\/p>\n

      C(s, gra) \u2192\u00a0C(s, dia)<\/span><\/span><\/p>\n<\/div>\n<\/li>\n

    18. \n
      \n

      Without consulting any tables, determine the \u0394H<\/em> for this reaction. Explain your answer.<\/p>\n

      H2<\/sub>O(\u2113, 25\u00b0C) \u2192\u00a0H2<\/sub>O(\u2113, 25\u00b0C)<\/span><\/span><\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n

      \n

      Answers<\/h3>\n
      \n

      1.<\/strong><\/p>\n

      5.70 J<\/p>\n

      3.<\/strong><\/p>\n

      4.69 L<\/p>\n

      5.<\/strong><\/p>\n

      80.97 kJ<\/p>\n

      7.<\/strong><\/p>\n

      91.9\u00b0C<\/p>\n

      9.<\/strong><\/p>\n

      6 CO2<\/sub>(g) +\u00a06 H2<\/sub>O(\u2113) \u2192\u00a0C6<\/sub>H12<\/sub>O6<\/sub>(s) +\u00a06 O2<\/sub>(g) \u0394H<\/em>\u00a0=\u00a02,799 kJ<\/p>\n

      11.<\/strong><\/p>\n

      2 Al2<\/sub>O3<\/sub>(s) \u2192\u00a04 Al(s) +\u00a03 O2<\/sub>(g) \u0394H<\/em>\u00a0=\u00a03351.4 kJ<\/p>\n

      13.<\/strong><\/p>\n

      3,668 g<\/p>\n

      15.<\/strong><\/p>\n

      \u0394H<\/em>\u00a0=\u00a030 kJ<\/p>\n

      17.<\/strong><\/p>\n

      \u0394H<\/em>\u00a0=\u00a01.897 kJ; the reaction is endothermic.<\/p>\n<\/div>\n<\/div>\n

      \u00a0<\/p>\n<\/div>\n<\/div>\n<\/div>\n\n\t\t\t

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