{"id":4820,"date":"2015-08-21T20:24:12","date_gmt":"2015-08-21T20:24:12","guid":{"rendered":"https:\/\/courses.candelalearning.com\/chemistryformajorsxmaster\/?post_type=chapter&p=4820"},"modified":"2016-08-09T18:39:50","modified_gmt":"2016-08-09T18:39:50","slug":"assignment-thermodynamics","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/chapter\/assignment-thermodynamics\/","title":{"raw":"Assignment\u2014Thermodynamics","rendered":"Assignment\u2014Thermodynamics"},"content":{"raw":"To download a copy of the assignment, please click on the link Sample Questions<\/a>.\r\n\r\nAs you work these matter and measurement problems, consider and explain:\r\n
    \r\n \t
  1. What type of question is it?<\/li>\r\n \t
  2. How do you know what type of question it is?<\/li>\r\n \t
  3. What information are you looking for?<\/li>\r\n \t
  4. What information do they give?<\/li>\r\n \t
  5. How will you go about solving this?<\/li>\r\n \t
  6. Show how to solve the problem.<\/li>\r\n \t
  7. Be able to answer for a different reaction, number, set of conditions, etc.<\/li>\r\n<\/ol>\r\n

    Sample Questions<\/h2>\r\n
      \r\n \t
    1. A gas absorbs 0.0 J of heat and then performs 31.7 J of work. What is the change in internal energy of the gas?\r\nA) 63.4 J\r\nB) 31.7 J\r\nC) \u201363.4 J\r\nD) \u201331.7\r\nE) none of these<\/li>\r\n \t
    2. Which of the following statements correctly describes the signs of q<\/i> and w<\/i> for the following exothermic process at P<\/i> = 1 atm and T<\/i> = 370 K?\r\nH2<\/sub>O(g<\/i>) \u2192 H2<\/sub>O(l<\/i>)\r\nA) q<\/i> and w<\/i> are negative\r\nB) q<\/i> is positive, w<\/i> is negative\r\nC) q<\/i> is negative, w<\/i> is positive\r\nD) q<\/i> and w<\/i> are both positive\r\nE) q<\/i> and w<\/i> are both zero<\/li>\r\n \t
    3. Which of the following statements is correct?\r\nA) The internal energy of a system increases when more work is done by the system than heat was flowing into the system.\r\nB) The internal energy of a system decreases when work is done on the system and heat is flowing into the system.\r\nC) The system does work on the surroundings when an ideal gas expands against a constant external pressure.\r\nD) All statements are true.\r\nE) All statements are false.<\/li>\r\n \t
    4. One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 3.10 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem. (T = 300 K; 1 L\u00b7atm = 101.3 J)\r\nA) 106 J\r\nB) 213 J\r\nC) 6.38 \u00d7 102<\/sup> J\r\nD) 314 J\r\nE) none of these<\/li>\r\n \t
    5. A fuel-air mixture is placed in a cylinder fitted with a piston. The original volume is 0.285-L. When the mixture is ignited, gases are produced and 805 J of energy is released. To what volume will the gases expand against a constant pressure of 635 mmHg, if all the energy released is converted to work to push the piston?\r\nA) 9.22 L\r\nB) 6.92 L\r\nC) 9.79 L\r\nD) 9.51 L\r\nE) 1.55 LUse the following to answer question 6 and 7:\r\nConsider a gas in a 1.0 L bulb at STP that is connected via a valve to another bulb that is initially evacuated. Answer the following concerning what occurs when the valve between the two bulbs is opened.<\/li>\r\n \t
    6. What is true about the value of w<\/i>?\r\nA)\u00a0It is greater than zero.\r\nB)\u00a0It is equal to zero.\r\nC)\u00a0It is less than zero.\r\nD)\u00a0More information is needed.\r\nE)\u00a0None of these.<\/li>\r\n \t
    7. What is true about the value of \u0394H?\r\nA)\u00a0It is greater than zero.\r\nB)\u00a0It is equal to zero.\r\nC)\u00a0It is less than zero.\r\nD)\u00a0More information is needed.\r\nE)\u00a0None of these.<\/li>\r\n \t
    8. Which of the following properties is (are) intensive properties?\r\nI. mass\r\nII. temperature\r\nIII. volume\r\nIV. concentration\r\nV. energy\r\nA)\u00a0I, III, and V\r\nB)\u00a0II only\r\nC)\u00a0II and IV\r\nD)\u00a0III and IV\r\nE)\u00a0I and V<\/li>\r\n \t
    9. Which one of the following statements is false?\r\nA)\u00a0The change in internal energy, \u0394E, for a process is equal to the amount of heat absorbed at constant volume,\u00a0qv<\/sub><\/i>.\r\nB)\u00a0The change in enthalpy, \u0394H, for a process is equal to the amount of heat absorbed at constant pressure,\u00a0qp<\/sub><\/i>.\r\nC)\u00a0A bomb calorimeter measures \u0394H directly.\r\nD)\u00a0If\u00a0qp<\/sub><\/i>\u00a0for a process is negative, the process is exothermic.\r\nE)\u00a0The freezing of water is an example of an exothermic reaction.<\/li>\r\n \t
    10. Consider this reaction:\r\nC2<\/sub>H5<\/sub>OH(l<\/i>) + 3O2<\/sub>(g<\/i>) \u2192 2CO2<\/sub>(g<\/i>) + 3H2<\/sub>O(l<\/i>); \u0394 H<\/i> = \u20131.37 \u00d7 103<\/sup> kJ\r\nConsider the following propositions:\r\nI. The reaction is endothermic\r\nII. The reaction is exothermic.\r\nIII. The enthalpy term would be different if the water formed was gaseous.\r\nWhich of these propositions is (are) true?\r\nA) I\r\nB) II\r\nC) III\r\nD) I, II\r\nE) II, III<\/li>\r\n \t
    11. Two metals of equal mass with different heat capacities are subjected to the same amount of heat. Which undergoes the smallest change in temperature?\r\nA)\u00a0The metal with the higher heat capacity.\r\nB)\u00a0The metal with the lower heat capacity.\r\nC)\u00a0Both undergo the same change in temperature.\r\nD)\u00a0You need to know the initial temperatures of the metals.\r\nE)\u00a0You need to know which metals you have.<\/li>\r\n \t
    12. A 48.2 g sample of a metal is heated to 97.5\u00b0C and then placed in a calorimeter containing 120.0 g of water (c<\/em> = 4.18 J\/g\u00b0C) at 21.3\u00b0C. The final temperature of the water is 24.5\u00b0C. Which metal was used?\r\nA)\u00a0Aluminum (c<\/em> = 0.89 J\/g\u00b0C)\r\nB)\u00a0Iron (c<\/em> = 0.45 J\/g\u00b0C)\r\nC)\u00a0Copper (c<\/em> = 0.20 J\/g\u00b0C)\r\nD)\u00a0Lead (c<\/em> = 0.14 J\/g\u00b0C)\r\nE)\u00a0none of these<\/li>\r\n \t
    13. The enthalpy of fusion of ice is 6.020 kJ\/mol. The heat capacity of liquid water is 75.4 J\/mol\u00b7\u00b0C. What is the smallest number of ice cubes at 0\u00b0C, each containing one mole of water, necessary to cool 500 g of liquid water initially at 20\u00b0C to 0\u00b0C?\r\nA)\u00a01\r\nB)\u00a07\r\nC)\u00a014\r\nD)\u00a015\r\nE)\u00a0126<\/li>\r\n \t
    14. Consider the reaction\r\nH2<\/sub>(g<\/em>) + O2<\/sub>(g<\/em>) \u2192 H2<\/sub>O(l<\/em>) \u0394H<\/em>\u00b0 = \u2013286 kJ\r\nWhich of the following is true?\r\nA)\u00a0The reaction is exothermic.\r\nB)\u00a0The reaction is endothermic.\r\nC)\u00a0The enthalpy of the products is less than that of the reactants.\r\nD)\u00a0Heat is absorbed by the system.\r\nE)\u00a0Both A and C are true.<\/li>\r\n \t
    15. If 5.0 kJ of energy is added to a 15.5-g sample of water at 10\u00b0C, the water is _______.\r\nA)\u00a0boiling\r\nB)\u00a0completely vaporized\r\nC)\u00a0frozen solid\r\nD)\u00a0decomposed\r\nE)\u00a0still a liquid<\/li>\r\n \t
    16. A chunk of lead at 91.3\u00b0C was added to 200.0 g of water at 15.5\u00b0C. The specific heat of lead is 0.129 J\/g\u00b0C, and the specific heat of water is 4.18 J\/g\u00b0C. When the temperature stabilized, the temperature of the mixture was 20.5\u00b0C. Assuming no heat was lost to the surroundings, what was the mass of lead added?\r\nA)\u00a01.88 kg\r\nB)\u00a0355 g\r\nC)\u00a0427 g\r\nD)\u00a0458 g\r\nE)\u00a0none of these<\/li>\r\n \t
    17. What is the specific heat capacity of graphite if it requires 266 J to raise the temperature of 15 grams of graphite by 25\u00b0C?\r\nA)\u00a01.4 J\/g\u00b0C\r\nB)\u00a00.71 J\/g\u00b0C\r\nC)\u00a00.43 J\/g\u00b0C\r\nD)\u00a00.60 J\/g\u00b0C\r\nE)\u00a0none of these<\/li>\r\n \t
    18. Consider this reaction:\r\nWhen a 11.6-g sample of ethyl alcohol (molar mass = 46.07 g\/mol) is burned, how much energy is released as heat?\r\nA)\u00a00.252 kJ\r\nB)\u00a00.345 kJ\r\nC)\u00a03.45 \u00d7 102<\/sub> kJ\r\nD)\u00a01.59 \u00d7 104<\/sub> kJ\r\nE)\u00a03.97 kJ<\/li>\r\n \t
    19. Given the equation S(s<\/i>) + O2<\/sub>(g<\/i>) \u2192 SO2<\/sub>(g<\/i>), \u0394H = \u2013296 kJ, which of the following statement(s) is (are) true?\r\nI. The reaction is exothermic.\r\nII. When 0.500 mole sulfur is reacted, 148 kJ of energy is released.\r\nIII. When 32.0 g of sulfur are burned, 2.96 \u00d7 105 J of energy is released.\r\nA)\u00a0All are true.\r\nB)\u00a0None is true.\r\nC)\u00a0I and II are true.\r\nD)\u00a0I and III are true.\r\nE)\u00a0Only II is true.<\/li>\r\n \t
    20. Consider the following specific heats of metals.\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      Metal<\/strong><\/td>\r\nSpecific Heat<\/strong><\/td>\r\n<\/tr>\r\n
      Zinc<\/td>\r\n0.387 J\/(g\u00b0C<\/td>\r\n<\/tr>\r\n
      Magnesium<\/td>\r\n1.02 J\/(g\u00b0C<\/td>\r\n<\/tr>\r\n
      Mercury<\/td>\r\n0.138 J\/(g\u00b0C<\/td>\r\n<\/tr>\r\n
      Silver<\/td>\r\n0.237\u00a0J\/(g\u00b0C<\/td>\r\n<\/tr>\r\n
      Bismuth<\/td>\r\n0.123\u00a0J\/(g\u00b0C<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nIf the same amount of heat is added to 25.0 g of each of the metals, which are all at the same initial temperature, which metal will have the highest temperature?\r\nA)\u00a0Zinc\r\nB)\u00a0Magnesium\r\nC)\u00a0Mercury\r\nD)\u00a0Silver\r\nE)\u00a0Bismuth<\/li>\r\n \t
    21. The specific heat capacities of metals are relatively low.\r\nA)\u00a0True\r\nB)\u00a0False<\/li>\r\n \t
    22. At 25\u00b0C, the following heats of reaction are known:\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      <\/td>\r\n\u0394H (kJ\/mol)<\/td>\r\n<\/tr>\r\n
      2ClF + O2<\/sub> \u2192 Cl2<\/sub>O + F2<\/sub>O<\/td>\r\n167.4<\/td>\r\n<\/tr>\r\n
      2ClF + O2<\/sub> \u2192 Cl2<\/sub>O + F2<\/sub>O<\/td>\r\n341.4<\/td>\r\n<\/tr>\r\n
      2F2 + O2<\/sub> \u2192 2F2<\/sub>O<\/td>\r\n\u201343.4<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nAt the same temperature, calculate \u0394H for the reaction: ClF + F2<\/sub> \u2192 ClF3<\/sub>\r\nA)\u00a0\u2013217.5 kJ\/mol\r\nB)\u00a0\u2013130.2 kJ\/mol\r\nC)\u00a0+217.5 kJ\/mol\r\nD)\u00a0\u2013108.7 kJ\/mol\r\nE)\u00a0none of these<\/li>\r\n \t
    23. Given the heats of the following reactions:\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      <\/td>\r\n<\/td>\r\n\u0394H\u00b0(kJ)<\/td>\r\n<\/tr>\r\n
      I.<\/td>\r\nP4<\/sub>(s<\/i>) + 6Cl2<\/sub>(g<\/i>) \u2192 4PCl3<\/sub>(g<\/i>)<\/td>\r\n\u20131225.6<\/td>\r\n<\/tr>\r\n
      II.<\/td>\r\nP4<\/sub>(s<\/i>) + 5O2<\/sub>(g<\/i>) \u2192 P4<\/sub>O10<\/sub>(s<\/i>)<\/td>\r\n\u20132967.3<\/td>\r\n<\/tr>\r\n
      III.<\/td>\r\nPCl3<\/sub>(g<\/i>) + Cl2<\/sub>(g<\/i>) \u2192 PCl5<\/sub>(g<\/i>)<\/td>\r\n\u201384.2<\/td>\r\n<\/tr>\r\n
      IV.<\/td>\r\nPCl3<\/sub>(g<\/i>) + O2<\/sub>(g<\/i>) \u2192 Cl3<\/sub>PO(g<\/i>)<\/td>\r\n\u2013285.7<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nCalculate the value of\u00a0\u0394H\u00b0 for the reaction below:\r\n\r\nP4<\/sub>O10<\/sub>(s<\/i>) + 6PCl5<\/sub>(g<\/i>)\r\nA)\u00a0\u2013110.5 kJ\r\nB)\u00a0\u2013610.1 kJ\r\nC)\u00a0\u20132682.2 kJ\r\nD)\u00a0\u20137555.0 kJ\r\nE)\u00a0None of these is within 5% of the correct answer.<\/li>\r\n \t
    24. Using the following thermochemical data, calculate \u0394Hf<\/sub>\u00b0 of Er2<\/sub>O3<\/sub>(s<\/i>).\r\n\r\n\r\n\r\n\r\n\r\n
      2ErCl3<\/sub>(s<\/i>) + 3H2<\/sub>O(l<\/i>) \u2192 Er2<\/sub>O3<\/sub>(s<\/i>) + 6HCl(g<\/i>)<\/td>\r\nH<\/i>\u00b0 = 403.1 kJ\/mol<\/td>\r\n<\/tr>\r\n
      2Er(s) + 3Cl2(g) \u2192 2ErCl3(s)<\/td>\r\nH<\/em>\u00b0 = \u20131997.4 kJ\/mol<\/td>\r\n<\/tr>\r\n
      4HCl(g) + O2(g) \u2192 2Cl2(g) + 2H2O(l)<\/td>\r\nH<\/em>\u00b0 = \u2013202.4 kJ\/mol<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nA)\u00a0\u20131897.9 kJ\/mol\r\nB)\u00a0\u20131796.7 kJ\/mol\r\nC)\u00a02602.9 kJ\/mol\r\nD)\u00a0\u20132198.1 kJ\/mol\r\nE)\u00a01391.9 kJ\/mol<\/li>\r\n \t
    25. Given the following:\r\n\r\n\r\n\r\n\r\n
      Cu2<\/sub>O(s<\/i>) + O2<\/sub>(g<\/i>) \u2192 2CuO(s<\/i>)<\/td>\r\n\u0394H<\/i>\u00b0 = \u2013144 kJ<\/td>\r\n<\/tr>\r\n
      Cu2<\/sub>O(s<\/i>) \u2192 Cu(s<\/i>) + CuO(s<\/i>)<\/td>\r\n\u0394H<\/i>\u00b0 = +11 kJ<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nCalculate the standard enthalpy of formation of CuO(s<\/i>).\r\nA) \u2013166 kJ\r\nB) \u2013299 kJ\r\nC) +299 kJ\r\nD) +155 kJ\r\nE)\u00a0\u2013155 kJ<\/li>\r\n \t
    26. The heat combustion of acetylene, C2<\/sub>H2<\/sub>(g<\/i>), at 25\u00b0C is \u20131299 kJ\/mol. At this temperature, \u0394H<\/i>f<\/sub>\u00b0 values for CO2<\/sub><\/i>(g<\/i>) and H2<\/sub><\/i>O(l<\/i>) are \u2013393 and \u2013286 kJ\/mol, respectively. Calculate \u0394H<\/i>f<\/sub>\u00b0 for acetylene.\r\nA) 2376 kJ\/mol\r\nB) 625 kJ\/mol\r\nC) 227 kJ\/mol\r\nD) \u2013625 kJ\/mol\r\nE) \u2013227 kJ\/mol<\/li>\r\n \t
    27. For the reaction:\r\nAgI(s<\/i>) + Br2<\/sub>(g<\/i>) \u2192 AgBr(s<\/i>) + I2<\/sub>(s<\/i>), \u0394H\u00b0= \u201354.0 kJ\r\n\u0394Hf<\/sub>\u00b0 for AgBr(s<\/i>) = \u2013100.4 kJ\/mol\r\n\u0394Hf<\/sub>\u00b0 for Br2<\/sub>(g) = +30.9 kJ\/mol\r\nWhat is the value of \u0394Hf<\/sub>\u00b0 for AgI(s<\/i>)?\r\nA)\u00a0\u2013123.5 kJ\/mol\r\nB) +77.3 kJ\/mol\r\nC) +61.8 kJ\/mol\r\nD)\u00a0\u201377.3 kJ\/mol\r\nE)\u00a0\u201361.8 kJ\/mol<\/li>\r\n \t
    28. For which of the following reaction(s) is the enthalpy change for the reaction not<\/i> equal to \u0394H<\/i>f<\/sub>\u00b0 of the product?\r\nI. 2H(g<\/i>) \u2192 H2<\/sub>(g<\/i>)\r\nII. H2<\/sub>(g<\/i>) + O2<\/sub>(g<\/i>) \u2192 H2<\/sub>O2<\/sub>(l<\/i>)\r\nIII. H2<\/sub>O(l<\/i>) + O(g<\/i>) \u2192 H2<\/sub>O2<\/sub>(l<\/i>)\r\nA) I\r\nB) II\r\nC) III\r\nD) I and III\r\nE) II and III<\/li>\r\n \t
    29. The following statements concerning petroleum are all true except<\/em>:\r\nA)\u00a0It is a thick, dark liquid composed mostly of hydrocarbons.\r\nB)\u00a0It must be separated into fractions (by boiling) in order to be used efficiently.\r\nC)\u00a0Some of the commercial uses of petroleum fractions include gasoline and kerosene.\r\nD)\u00a0It was probably formed from the remains of ancient marine organisms.\r\nE)\u00a0All of its hydrocarbon chains contain the same number of carbon atoms.<\/li>\r\n \t
    30. What is the coal with the highest energy available per unit burned?\r\nA) Lignite\r\nB) Subbituminous\r\nC) Bituminous\r\nD) Anthracite\r\nE) They are equal in energy value.<\/li>\r\n \t
    31. Which of the following is both a greenhouse gas and a fuel?\r\nA) carbon dioxide\r\nB) coal\r\nC) freon\r\nD) methane\r\nE) nitrogen<\/li>\r\n \t
    32. Which of the following is not<\/em> being considered as an energy source for the future?\r\nA) ethanol\r\nB) methanol\r\nC) seed oil\r\nD) shale oil\r\nE) carbon dioxide<\/li>\r\n<\/ol>\r\n

      Sample Answers<\/h2>\r\n
        \r\n \t
      1. D<\/li>\r\n \t
      2. C<\/li>\r\n \t
      3. C<\/li>\r\n \t
      4. B<\/li>\r\n \t
      5. C<\/li>\r\n \t
      6. B<\/li>\r\n \t
      7. B<\/li>\r\n \t
      8. C<\/li>\r\n \t
      9. C<\/li>\r\n \t
      10. E<\/li>\r\n \t
      11. A<\/li>\r\n \t
      12. B<\/li>\r\n \t
      13. B<\/li>\r\n \t
      14. E<\/li>\r\n \t
      15. E<\/li>\r\n \t
      16. D<\/li>\r\n \t
      17. B<\/li>\r\n \t
      18. C<\/li>\r\n \t
      19. A<\/li>\r\n \t
      20. E<\/li>\r\n \t
      21. A<\/li>\r\n \t
      22. D<\/li>\r\n \t
      23. B<\/li>\r\n \t
      24. A<\/li>\r\n \t
      25. E<\/li>\r\n \t
      26. C<\/li>\r\n \t
      27. E<\/li>\r\n \t
      28. D<\/li>\r\n \t
      29. E<\/li>\r\n \t
      30. D<\/li>\r\n \t
      31. D<\/li>\r\n \t
      32. E<\/li>\r\n<\/ol>","rendered":"

        To download a copy of the assignment, please click on the link Sample Questions<\/a>.<\/p>\n

        As you work these matter and measurement problems, consider and explain:<\/p>\n

          \n
        1. What type of question is it?<\/li>\n
        2. How do you know what type of question it is?<\/li>\n
        3. What information are you looking for?<\/li>\n
        4. What information do they give?<\/li>\n
        5. How will you go about solving this?<\/li>\n
        6. Show how to solve the problem.<\/li>\n
        7. Be able to answer for a different reaction, number, set of conditions, etc.<\/li>\n<\/ol>\n

          Sample Questions<\/h2>\n
            \n
          1. A gas absorbs 0.0 J of heat and then performs 31.7 J of work. What is the change in internal energy of the gas?
            \nA) 63.4 J
            \nB) 31.7 J
            \nC) \u201363.4 J
            \nD) \u201331.7
            \nE) none of these<\/li>\n
          2. Which of the following statements correctly describes the signs of q<\/i> and w<\/i> for the following exothermic process at P<\/i> = 1 atm and T<\/i> = 370 K?
            \nH2<\/sub>O(g<\/i>) \u2192 H2<\/sub>O(l<\/i>)
            \nA) q<\/i> and w<\/i> are negative
            \nB) q<\/i> is positive, w<\/i> is negative
            \nC) q<\/i> is negative, w<\/i> is positive
            \nD) q<\/i> and w<\/i> are both positive
            \nE) q<\/i> and w<\/i> are both zero<\/li>\n
          3. Which of the following statements is correct?
            \nA) The internal energy of a system increases when more work is done by the system than heat was flowing into the system.
            \nB) The internal energy of a system decreases when work is done on the system and heat is flowing into the system.
            \nC) The system does work on the surroundings when an ideal gas expands against a constant external pressure.
            \nD) All statements are true.
            \nE) All statements are false.<\/li>\n
          4. One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 3.10 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem. (T = 300 K; 1 L\u00b7atm = 101.3 J)
            \nA) 106 J
            \nB) 213 J
            \nC) 6.38 \u00d7 102<\/sup> J
            \nD) 314 J
            \nE) none of these<\/li>\n
          5. A fuel-air mixture is placed in a cylinder fitted with a piston. The original volume is 0.285-L. When the mixture is ignited, gases are produced and 805 J of energy is released. To what volume will the gases expand against a constant pressure of 635 mmHg, if all the energy released is converted to work to push the piston?
            \nA) 9.22 L
            \nB) 6.92 L
            \nC) 9.79 L
            \nD) 9.51 L
            \nE) 1.55 LUse the following to answer question 6 and 7:
            \nConsider a gas in a 1.0 L bulb at STP that is connected via a valve to another bulb that is initially evacuated. Answer the following concerning what occurs when the valve between the two bulbs is opened.<\/li>\n
          6. What is true about the value of w<\/i>?
            \nA)\u00a0It is greater than zero.
            \nB)\u00a0It is equal to zero.
            \nC)\u00a0It is less than zero.
            \nD)\u00a0More information is needed.
            \nE)\u00a0None of these.<\/li>\n
          7. What is true about the value of \u0394H?
            \nA)\u00a0It is greater than zero.
            \nB)\u00a0It is equal to zero.
            \nC)\u00a0It is less than zero.
            \nD)\u00a0More information is needed.
            \nE)\u00a0None of these.<\/li>\n
          8. Which of the following properties is (are) intensive properties?
            \nI. mass
            \nII. temperature
            \nIII. volume
            \nIV. concentration
            \nV. energy
            \nA)\u00a0I, III, and V
            \nB)\u00a0II only
            \nC)\u00a0II and IV
            \nD)\u00a0III and IV
            \nE)\u00a0I and V<\/li>\n
          9. Which one of the following statements is false?
            \nA)\u00a0The change in internal energy, \u0394E, for a process is equal to the amount of heat absorbed at constant volume,\u00a0qv<\/sub><\/i>.
            \nB)\u00a0The change in enthalpy, \u0394H, for a process is equal to the amount of heat absorbed at constant pressure,\u00a0qp<\/sub><\/i>.
            \nC)\u00a0A bomb calorimeter measures \u0394H directly.
            \nD)\u00a0If\u00a0qp<\/sub><\/i>\u00a0for a process is negative, the process is exothermic.
            \nE)\u00a0The freezing of water is an example of an exothermic reaction.<\/li>\n
          10. Consider this reaction:
            \nC2<\/sub>H5<\/sub>OH(l<\/i>) + 3O2<\/sub>(g<\/i>) \u2192 2CO2<\/sub>(g<\/i>) + 3H2<\/sub>O(l<\/i>); \u0394 H<\/i> = \u20131.37 \u00d7 103<\/sup> kJ
            \nConsider the following propositions:
            \nI. The reaction is endothermic
            \nII. The reaction is exothermic.
            \nIII. The enthalpy term would be different if the water formed was gaseous.
            \nWhich of these propositions is (are) true?
            \nA) I
            \nB) II
            \nC) III
            \nD) I, II
            \nE) II, III<\/li>\n
          11. Two metals of equal mass with different heat capacities are subjected to the same amount of heat. Which undergoes the smallest change in temperature?
            \nA)\u00a0The metal with the higher heat capacity.
            \nB)\u00a0The metal with the lower heat capacity.
            \nC)\u00a0Both undergo the same change in temperature.
            \nD)\u00a0You need to know the initial temperatures of the metals.
            \nE)\u00a0You need to know which metals you have.<\/li>\n
          12. A 48.2 g sample of a metal is heated to 97.5\u00b0C and then placed in a calorimeter containing 120.0 g of water (c<\/em> = 4.18 J\/g\u00b0C) at 21.3\u00b0C. The final temperature of the water is 24.5\u00b0C. Which metal was used?
            \nA)\u00a0Aluminum (c<\/em> = 0.89 J\/g\u00b0C)
            \nB)\u00a0Iron (c<\/em> = 0.45 J\/g\u00b0C)
            \nC)\u00a0Copper (c<\/em> = 0.20 J\/g\u00b0C)
            \nD)\u00a0Lead (c<\/em> = 0.14 J\/g\u00b0C)
            \nE)\u00a0none of these<\/li>\n
          13. The enthalpy of fusion of ice is 6.020 kJ\/mol. The heat capacity of liquid water is 75.4 J\/mol\u00b7\u00b0C. What is the smallest number of ice cubes at 0\u00b0C, each containing one mole of water, necessary to cool 500 g of liquid water initially at 20\u00b0C to 0\u00b0C?
            \nA)\u00a01
            \nB)\u00a07
            \nC)\u00a014
            \nD)\u00a015
            \nE)\u00a0126<\/li>\n
          14. Consider the reaction
            \nH2<\/sub>(g<\/em>) + O2<\/sub>(g<\/em>) \u2192 H2<\/sub>O(l<\/em>) \u0394H<\/em>\u00b0 = \u2013286 kJ
            \nWhich of the following is true?
            \nA)\u00a0The reaction is exothermic.
            \nB)\u00a0The reaction is endothermic.
            \nC)\u00a0The enthalpy of the products is less than that of the reactants.
            \nD)\u00a0Heat is absorbed by the system.
            \nE)\u00a0Both A and C are true.<\/li>\n
          15. If 5.0 kJ of energy is added to a 15.5-g sample of water at 10\u00b0C, the water is _______.
            \nA)\u00a0boiling
            \nB)\u00a0completely vaporized
            \nC)\u00a0frozen solid
            \nD)\u00a0decomposed
            \nE)\u00a0still a liquid<\/li>\n
          16. A chunk of lead at 91.3\u00b0C was added to 200.0 g of water at 15.5\u00b0C. The specific heat of lead is 0.129 J\/g\u00b0C, and the specific heat of water is 4.18 J\/g\u00b0C. When the temperature stabilized, the temperature of the mixture was 20.5\u00b0C. Assuming no heat was lost to the surroundings, what was the mass of lead added?
            \nA)\u00a01.88 kg
            \nB)\u00a0355 g
            \nC)\u00a0427 g
            \nD)\u00a0458 g
            \nE)\u00a0none of these<\/li>\n
          17. What is the specific heat capacity of graphite if it requires 266 J to raise the temperature of 15 grams of graphite by 25\u00b0C?
            \nA)\u00a01.4 J\/g\u00b0C
            \nB)\u00a00.71 J\/g\u00b0C
            \nC)\u00a00.43 J\/g\u00b0C
            \nD)\u00a00.60 J\/g\u00b0C
            \nE)\u00a0none of these<\/li>\n
          18. Consider this reaction:
            \nWhen a 11.6-g sample of ethyl alcohol (molar mass = 46.07 g\/mol) is burned, how much energy is released as heat?
            \nA)\u00a00.252 kJ
            \nB)\u00a00.345 kJ
            \nC)\u00a03.45 \u00d7 102<\/sub> kJ
            \nD)\u00a01.59 \u00d7 104<\/sub> kJ
            \nE)\u00a03.97 kJ<\/li>\n
          19. Given the equation S(s<\/i>) + O2<\/sub>(g<\/i>) \u2192 SO2<\/sub>(g<\/i>), \u0394H = \u2013296 kJ, which of the following statement(s) is (are) true?
            \nI. The reaction is exothermic.
            \nII. When 0.500 mole sulfur is reacted, 148 kJ of energy is released.
            \nIII. When 32.0 g of sulfur are burned, 2.96 \u00d7 105 J of energy is released.
            \nA)\u00a0All are true.
            \nB)\u00a0None is true.
            \nC)\u00a0I and II are true.
            \nD)\u00a0I and III are true.
            \nE)\u00a0Only II is true.<\/li>\n
          20. Consider the following specific heats of metals.
            \n\n\n\n\n\n\n\n\n
            Metal<\/strong><\/td>\nSpecific Heat<\/strong><\/td>\n<\/tr>\n
            Zinc<\/td>\n0.387 J\/(g\u00b0C<\/td>\n<\/tr>\n
            Magnesium<\/td>\n1.02 J\/(g\u00b0C<\/td>\n<\/tr>\n
            Mercury<\/td>\n0.138 J\/(g\u00b0C<\/td>\n<\/tr>\n
            Silver<\/td>\n0.237\u00a0J\/(g\u00b0C<\/td>\n<\/tr>\n
            Bismuth<\/td>\n0.123\u00a0J\/(g\u00b0C<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

            If the same amount of heat is added to 25.0 g of each of the metals, which are all at the same initial temperature, which metal will have the highest temperature?
            \nA)\u00a0Zinc
            \nB)\u00a0Magnesium
            \nC)\u00a0Mercury
            \nD)\u00a0Silver
            \nE)\u00a0Bismuth<\/li>\n

          21. The specific heat capacities of metals are relatively low.
            \nA)\u00a0True
            \nB)\u00a0False<\/li>\n
          22. At 25\u00b0C, the following heats of reaction are known:
            \n\n\n\n\n\n\n
            <\/td>\n\u0394H (kJ\/mol)<\/td>\n<\/tr>\n
            2ClF + O2<\/sub> \u2192 Cl2<\/sub>O + F2<\/sub>O<\/td>\n167.4<\/td>\n<\/tr>\n
            2ClF + O2<\/sub> \u2192 Cl2<\/sub>O + F2<\/sub>O<\/td>\n341.4<\/td>\n<\/tr>\n
            2F2 + O2<\/sub> \u2192 2F2<\/sub>O<\/td>\n\u201343.4<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

            At the same temperature, calculate \u0394H for the reaction: ClF + F2<\/sub> \u2192 ClF3<\/sub>
            \nA)\u00a0\u2013217.5 kJ\/mol
            \nB)\u00a0\u2013130.2 kJ\/mol
            \nC)\u00a0+217.5 kJ\/mol
            \nD)\u00a0\u2013108.7 kJ\/mol
            \nE)\u00a0none of these<\/li>\n

          23. Given the heats of the following reactions:
            \n\n\n\n\n\n\n\n
            <\/td>\n<\/td>\n\u0394H\u00b0(kJ)<\/td>\n<\/tr>\n
            I.<\/td>\nP4<\/sub>(s<\/i>) + 6Cl2<\/sub>(g<\/i>) \u2192 4PCl3<\/sub>(g<\/i>)<\/td>\n\u20131225.6<\/td>\n<\/tr>\n
            II.<\/td>\nP4<\/sub>(s<\/i>) + 5O2<\/sub>(g<\/i>) \u2192 P4<\/sub>O10<\/sub>(s<\/i>)<\/td>\n\u20132967.3<\/td>\n<\/tr>\n
            III.<\/td>\nPCl3<\/sub>(g<\/i>) + Cl2<\/sub>(g<\/i>) \u2192 PCl5<\/sub>(g<\/i>)<\/td>\n\u201384.2<\/td>\n<\/tr>\n
            IV.<\/td>\nPCl3<\/sub>(g<\/i>) + O2<\/sub>(g<\/i>) \u2192 Cl3<\/sub>PO(g<\/i>)<\/td>\n\u2013285.7<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

            Calculate the value of\u00a0\u0394H\u00b0 for the reaction below:<\/p>\n

            P4<\/sub>O10<\/sub>(s<\/i>) + 6PCl5<\/sub>(g<\/i>)
            \nA)\u00a0\u2013110.5 kJ
            \nB)\u00a0\u2013610.1 kJ
            \nC)\u00a0\u20132682.2 kJ
            \nD)\u00a0\u20137555.0 kJ
            \nE)\u00a0None of these is within 5% of the correct answer.<\/li>\n

          24. Using the following thermochemical data, calculate \u0394Hf<\/sub>\u00b0 of Er2<\/sub>O3<\/sub>(s<\/i>).
            \n\n\n\n\n\n
            2ErCl3<\/sub>(s<\/i>) + 3H2<\/sub>O(l<\/i>) \u2192 Er2<\/sub>O3<\/sub>(s<\/i>) + 6HCl(g<\/i>)<\/td>\nH<\/i>\u00b0 = 403.1 kJ\/mol<\/td>\n<\/tr>\n
            2Er(s) + 3Cl2(g) \u2192 2ErCl3(s)<\/td>\nH<\/em>\u00b0 = \u20131997.4 kJ\/mol<\/td>\n<\/tr>\n
            4HCl(g) + O2(g) \u2192 2Cl2(g) + 2H2O(l)<\/td>\nH<\/em>\u00b0 = \u2013202.4 kJ\/mol<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

            A)\u00a0\u20131897.9 kJ\/mol
            \nB)\u00a0\u20131796.7 kJ\/mol
            \nC)\u00a02602.9 kJ\/mol
            \nD)\u00a0\u20132198.1 kJ\/mol
            \nE)\u00a01391.9 kJ\/mol<\/li>\n

          25. Given the following:
            \n\n\n\n\n
            Cu2<\/sub>O(s<\/i>) + O2<\/sub>(g<\/i>) \u2192 2CuO(s<\/i>)<\/td>\n\u0394H<\/i>\u00b0 = \u2013144 kJ<\/td>\n<\/tr>\n
            Cu2<\/sub>O(s<\/i>) \u2192 Cu(s<\/i>) + CuO(s<\/i>)<\/td>\n\u0394H<\/i>\u00b0 = +11 kJ<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

            Calculate the standard enthalpy of formation of CuO(s<\/i>).
            \nA) \u2013166 kJ
            \nB) \u2013299 kJ
            \nC) +299 kJ
            \nD) +155 kJ
            \nE)\u00a0\u2013155 kJ<\/li>\n

          26. The heat combustion of acetylene, C2<\/sub>H2<\/sub>(g<\/i>), at 25\u00b0C is \u20131299 kJ\/mol. At this temperature, \u0394H<\/i>f<\/sub>\u00b0 values for CO2<\/sub><\/i>(g<\/i>) and H2<\/sub><\/i>O(l<\/i>) are \u2013393 and \u2013286 kJ\/mol, respectively. Calculate \u0394H<\/i>f<\/sub>\u00b0 for acetylene.
            \nA) 2376 kJ\/mol
            \nB) 625 kJ\/mol
            \nC) 227 kJ\/mol
            \nD) \u2013625 kJ\/mol
            \nE) \u2013227 kJ\/mol<\/li>\n
          27. For the reaction:
            \nAgI(s<\/i>) + Br2<\/sub>(g<\/i>) \u2192 AgBr(s<\/i>) + I2<\/sub>(s<\/i>), \u0394H\u00b0= \u201354.0 kJ
            \n\u0394Hf<\/sub>\u00b0 for AgBr(s<\/i>) = \u2013100.4 kJ\/mol
            \n\u0394Hf<\/sub>\u00b0 for Br2<\/sub>(g) = +30.9 kJ\/mol
            \nWhat is the value of \u0394Hf<\/sub>\u00b0 for AgI(s<\/i>)?
            \nA)\u00a0\u2013123.5 kJ\/mol
            \nB) +77.3 kJ\/mol
            \nC) +61.8 kJ\/mol
            \nD)\u00a0\u201377.3 kJ\/mol
            \nE)\u00a0\u201361.8 kJ\/mol<\/li>\n
          28. For which of the following reaction(s) is the enthalpy change for the reaction not<\/i> equal to \u0394H<\/i>f<\/sub>\u00b0 of the product?
            \nI. 2H(g<\/i>) \u2192 H2<\/sub>(g<\/i>)
            \nII. H2<\/sub>(g<\/i>) + O2<\/sub>(g<\/i>) \u2192 H2<\/sub>O2<\/sub>(l<\/i>)
            \nIII. H2<\/sub>O(l<\/i>) + O(g<\/i>) \u2192 H2<\/sub>O2<\/sub>(l<\/i>)
            \nA) I
            \nB) II
            \nC) III
            \nD) I and III
            \nE) II and III<\/li>\n
          29. The following statements concerning petroleum are all true except<\/em>:
            \nA)\u00a0It is a thick, dark liquid composed mostly of hydrocarbons.
            \nB)\u00a0It must be separated into fractions (by boiling) in order to be used efficiently.
            \nC)\u00a0Some of the commercial uses of petroleum fractions include gasoline and kerosene.
            \nD)\u00a0It was probably formed from the remains of ancient marine organisms.
            \nE)\u00a0All of its hydrocarbon chains contain the same number of carbon atoms.<\/li>\n
          30. What is the coal with the highest energy available per unit burned?
            \nA) Lignite
            \nB) Subbituminous
            \nC) Bituminous
            \nD) Anthracite
            \nE) They are equal in energy value.<\/li>\n
          31. Which of the following is both a greenhouse gas and a fuel?
            \nA) carbon dioxide
            \nB) coal
            \nC) freon
            \nD) methane
            \nE) nitrogen<\/li>\n
          32. Which of the following is not<\/em> being considered as an energy source for the future?
            \nA) ethanol
            \nB) methanol
            \nC) seed oil
            \nD) shale oil
            \nE) carbon dioxide<\/li>\n<\/ol>\n

            Sample Answers<\/h2>\n
              \n
            1. D<\/li>\n
            2. C<\/li>\n
            3. C<\/li>\n
            4. B<\/li>\n
            5. C<\/li>\n
            6. B<\/li>\n
            7. B<\/li>\n
            8. C<\/li>\n
            9. C<\/li>\n
            10. E<\/li>\n
            11. A<\/li>\n
            12. B<\/li>\n
            13. B<\/li>\n
            14. E<\/li>\n
            15. E<\/li>\n
            16. D<\/li>\n
            17. B<\/li>\n
            18. C<\/li>\n
            19. A<\/li>\n
            20. E<\/li>\n
            21. A<\/li>\n
            22. D<\/li>\n
            23. B<\/li>\n
            24. A<\/li>\n
            25. E<\/li>\n
            26. C<\/li>\n
            27. E<\/li>\n
            28. D<\/li>\n
            29. E<\/li>\n
            30. D<\/li>\n
            31. D<\/li>\n
            32. E<\/li>\n<\/ol>\n\n\t\t\t
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