{"id":1092,"date":"2016-01-11T20:02:52","date_gmt":"2016-01-11T20:02:52","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistryclone\/chapter\/end-of-chapter-material-34\/"},"modified":"2020-04-20T16:46:26","modified_gmt":"2020-04-20T16:46:26","slug":"end-of-chapter-18-material","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistryclone\/chapter\/end-of-chapter-18-material\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"
\r\n

Exercises<\/h3>\r\n1. Classify each of the following as spontaneous or nonspontaneous processes:\r\n

a)\u00a0 the browning of a cut apple slice on a snack tray over time<\/p>\r\n

b)\u00a0 the rolling of a ball uphill<\/p>\r\n

c)\u00a0\u00a0the formation of diamond from the graphite in your pencil<\/p>\r\n

d)\u00a0\u00a0the melting of ice cubes in a glass of water you are holding<\/p>\r\n2. State the second law of thermodynamics.\r\n\r\n3. What sign would you expect for \u0394S<\/em> for the following processes?\r\n

a)\u00a0\u00a0water\u00a0freezing in a lake during a cold Alberta winter<\/p>\r\n

b)\u00a0\u00a0AB(s) + CD(s) \u2192 AC(g) + BD(g)<\/p>\r\n

c)\u00a0\u00a0a balloon with a fixed amount of gas stretched to a larger volume<\/p>\r\n

d)\u00a0\u00a0the sublimation of dry ice<\/p>\r\n

e)\u00a0\u00a03 E2<\/sub>F2<\/sub>(g) \u2192 E6<\/sub>F6<\/sub>(g)<\/p>\r\n4. Which of the following would you expect to have the higher standard molar entropy, S<\/em>\u2070?\r\n

a)\u00a0\u00a0Br2<\/sub>(\u2113<\/span>) or Br2<\/sub>(g)<\/p>\r\n

b)\u00a0\u00a0NO2<\/sub>(g) or NO(g)<\/p>\r\n

c)\u00a0\u00a0C2<\/sub>H6<\/sub>(g) or C5<\/sub>H12<\/sub>(g)<\/p>\r\n5. Calculate the \u0394S<\/em>\u2070 of the following reactions using the values listed in the appendix.\r\n

a)\u00a0\u00a04 NH3<\/sub>(g) + 5 O2<\/sub>(g) \u2192 6 H2<\/sub>O(g)\u00a0 + 4 NO(g)<\/p>\r\n

b)\u00a0\u00a02 HgO(s) \u2192 2 Hg(\u2113<\/span>)\u00a0 + O2<\/sub>(g)<\/p>\r\n

c)\u00a0\u00a03 FeCl2<\/sub>(s) + KNO3<\/sub>(s) + 4 HCl (aq) \u2192 3 FeCl3<\/sub>(s) + KCl(s) + NO(g) + 2 H2<\/sub>O(\u2113<\/span>)<\/p>\r\n6. Draw a diagram showing the approximate entropy change of water from -100\u2070C to 250\u2070C.\r\n\r\n7. A chemical reaction has \u0394H<\/em>\u2070 = -43.5 kJ and \u0394S<\/em>\u2070 = -65.8 J\/K. Calculate \u0394G<\/em>\u2070 at 298 K. Is this a spontaneous process?\r\n\r\n8. Using data from the appendix, determine \u0394G<\/em>\u2070 for all reactions listed in question 5.\r\n\r\n9. Find the standard Gibbs energy change for the reaction\r\n\r\nCaCO3<\/sub>(s)\u00a0\u2192 CaO(s)\u00a0+ CO2<\/sub>(g)\r\n\r\nThe\u00a0\u0394Gf<\/sub>\u00b0<\/em>\u00a0values for the three components of this reaction system are CaCO3<\/sub>(s): \u20131128\u00a0kJ\u00a0mol\u20131<\/sup>; CaO(s): \u2013603.5\u00a0kJ\/mol; CO2<\/sub>(g): \u2013137.2\u00a0kJ\/mol.[footnote]Question and solution from Chem1 Virtual Textbook, Stephen Lower\/CC-BY-SA-3.0[\/footnote]\r\n\r\n10. Using the appendix data, determine the approximate temperature at which the following processes are at equilibrium:\r\n

a)\u00a0\u00a0CH2<\/sub>Cl2<\/sub>(\u2113<\/span>) \u2192 CH2<\/sub>Cl2<\/sub>(g)<\/p>\r\n

b)\u00a0\u00a0CH3<\/sub>OH(\u2113<\/span>) \u2192 CH3<\/sub>OH(g)<\/p>\r\n11. Determine if the following reactions would be spontaneous at any temperature, nonspontaneous at any temperature, spontaneous at low temperature but not high temperature, or spontaneous at high temperature but not low temperature:\r\n

a)\u00a0\u00a0\u0394H<\/em>\u2070 = -750 kJ and \u0394S<\/em>\u2070 = 250 J\/K<\/p>\r\n

b)\u00a0\u00a0\u0394H<\/em>\u2070 = -100 kJ and \u0394S<\/em>\u2070 = -300 J\/K<\/p>\r\n

c)\u00a0\u00a0\u0394H<\/em>\u2070 = 95 kJ and \u0394S<\/em>\u2070 = -70 J\/K<\/p>\r\n

d)\u00a0\u00a0\u0394H<\/em>\u2070 = 400 kJ and \u0394S<\/em>\u2070 = 500 J\/K<\/p>\r\n12. The K<\/em>a<\/sub> for acetic acid, CH3<\/sub>COOH, is 1.75 x 10-5<\/sup> at 25\u2070C.\r\n

a)\u00a0\u00a0Using the K<\/em>a<\/sub> value, determine the \u0394G<\/em>\u2070 for the dissociation of acetic acid in aqueous solution.<\/p>\r\n

b)\u00a0\u00a0What is the value of \u0394G <\/em>when [H+<\/sup>] is 7.5 x 10-2<\/sup> M, [CH3<\/sub>COO-<\/sup>] is 2.5 x 10-2<\/sup> M, and [CH3<\/sub>COOH] is 0.10 M?<\/p>\r\n13. Calculate the equilibrium constant for the reaction H+<\/sup>(aq)\u00a0+ OH-<\/sup>(aq)\u00a0\u2192\u00a0H2<\/sub>O(\u2113<\/span>)\u00a0from the following data:\r\n\r\n\r\n\r\n\r\n\r\n
<\/td>\r\nH+<\/sup>(aq)<\/strong><\/td>\r\nOH-<\/sup>(aq)<\/strong><\/td>\r\nH2<\/sub>(\u2113<\/span><\/em>)<\/strong><\/td>\r\n<\/tr>\r\n
\u0394H\u00b0<\/strong><\/span>f<\/sub><\/em>, kJ mol\u20131<\/strong><\/td>\r\n0<\/td>\r\n\u2013230.0<\/td>\r\n\u2013285.8<\/td>\r\n<\/tr>\r\n
S<\/em><\/strong>\u00b0, J K\u20131\u00a0mol\u20131<\/strong><\/td>\r\n0*<\/td>\r\n\u201310.9<\/td>\r\n70.0<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n* Note that the standard entropy of the hydrogen ion is zero by definition. This reflects the fact that it is impossible to carry out thermodynamic studies on a single-charged species. All ionic entropies are relative to that of H+<\/sup>(aq), which explains why some values (as for the aqueous hydroxide ion) are negative.[footnote]Question and solution from Chem1 Virtual Textbook, Stephen Lower\/CC-BY-SA-3.0[\/footnote]\r\n\r\n14. Using data from the appendix, calculate the equilibrium constants at 298 K for all the reactions in question 5.\r\n\r\n<\/div>\r\n
\r\n

Answers<\/h3>\r\n1.<\/strong>\r\n

a)\u00a0\u00a0spontaneous<\/p>\r\n

b)\u00a0nonspontaneous<\/p>\r\n

c)\u00a0\u00a0nonspontaneous<\/p>\r\n

d)\u00a0\u00a0spontaneous<\/p>\r\n3.<\/strong>\r\n

a)\u00a0\u00a0\u0394S =\u00a0-<\/p>\r\n

b)\u00a0\u00a0\u0394S = +<\/p>\r\n

c)\u00a0\u00a0\u0394S = +<\/p>\r\n

d)\u00a0\u00a0\u0394S = +<\/p>\r\n

e)\u00a0\u00a0\u0394S =\u00a0-<\/p>\r\n5.<\/strong>\r\n

a)<\/p>\r\n

\u0394S<\/em>\u2070 = \u2211nS<\/em>\u2070(products) - \u2211mS<\/em>\u2070(reactants)<\/p>\r\n

\u0394S<\/em>\u2070 = (6 S<\/em>\u2070 H2<\/sub>O(g) \u00a0+ 4 S<\/em>\u2070 NO(g)) - (4 S<\/em>\u2070 NH3<\/sub>(g) \u00a0+ 5 S<\/em>\u2070 O2<\/sub>(g))<\/p>\r\n

\u0394S<\/em>\u2070 = [(6 x 188.8 J\/mol K) + (4 x 210.8 J\/mol K)] - [(4 x 192.8 J\/mol K) + (5 x 205.2 J\/mol K)]<\/p>\r\n

\u0394S<\/em>\u2070 = 178.8 J\/mol K<\/p>\r\n

b)<\/p>\r\n

\u0394S<\/em>\u2070 = \u2211nS<\/em>\u2070(products) - \u2211mS<\/em>\u2070(reactants)<\/p>\r\n

\u0394S<\/em>\u2070 = (2 S<\/em>\u2070 Hg(\u2113<\/span>) + S<\/em>\u2070 O2<\/sub>(g)) - (2 S<\/em>\u2070 HgO)<\/p>\r\n

\u0394S<\/em>\u2070 = [(2 x 75.9 J\/mol K) + (205.2 J\/mol K)] - (2 x 70.3 J\/mol K)<\/p>\r\n

\u0394S<\/em>\u2070 = 216.4 J\/mol K<\/p>\r\n

c)<\/p>\r\n

\u0394S<\/em>\u2070 = \u2211nS<\/em>\u2070(products) - \u2211mS<\/em>\u2070(reactants)<\/p>\r\n

\u0394S<\/em>\u2070 = (3 S<\/em>\u2070 FeCl3<\/sub>(s) + S<\/em>\u2070 KCl(s) + S<\/em>\u2070 NO(g) + 2 S<\/em>\u2070 H2<\/sub>O(\u2113<\/span>))- (3 S<\/em>\u2070 FeCl2<\/sub>(s) + S<\/em>\u2070 KNO3<\/sub>(s) + 4 S<\/em>\u2070 HCl (aq))<\/p>\r\n

\u0394S<\/em>\u2070 = [(3 x 142.3 J\/mol K) + (82.6 J\/mol K) + (210.8 J\/mol K) + (2 x 70.0 J\/mol K)] - [(3 x 118.0 J\/mol K) + (133.1 J\/mol K) + (4 x 56.5 J\/mol K)]<\/p>\r\n

\u0394S<\/em>\u2070 = 147.2 J\/mol K<\/p>\r\n7.<\/strong>\r\n\r\n\u0394G<\/em>\u2070 = \u0394H<\/em>\u2070 - T<\/em>\u0394S<\/em>\u2070\r\n\r\n\u0394G<\/em>\u2070 = -43.5 kJ \u2013 [(298 K)(-65.8 J\/K)]\r\n\r\n\u0394G<\/em>\u2070 = -23.9 kJ\r\n\r\n\u0394G<\/em>\u2070 is negative therefore this is a spontaneous process.\r\n\r\n9.<\/strong>\r\n\r\n\u0394G\u00b0<\/em>\u00a0= (\u2013603.5 \u2013137.2) \u2013 (\u20131128)\u00a0kJ\/mol =\u00a0+130.9\u00a0kJ\/mol,\u00a0<\/strong>indicating that the process is not spontaneous under standard conditions (i.e., solid calcium carbonate will not form solid calcium oxide and CO2<\/sub>\u00a0at 1 atm partial pressure at 25\u00b0C.)\r\n\r\n11.<\/strong>\r\n

a) \u00a0spontaneous at all temperatures<\/p>\r\n

b)\u00a0\u00a0spontaneous at low temperatures, nonspontaneous at high temperatures<\/p>\r\n

c)\u00a0\u00a0nonspontaneous at all temperatures<\/p>\r\n

d)\u00a0\u00a0spontaneous at high temperatures, nonspontaneous at low temperatures<\/p>\r\n13.<\/strong>\r\n\r\n\u0394H<\/em>\u00b0 = (\u2211\u0394H<\/em>\u00b0f<\/sub><\/em>,\u00a0products<\/em>) \u2013 (\u2211\u0394H<\/em>\u00b0f<\/sub><\/em>,\u00a0reactants<\/em>) = (\u2013285.8) \u2013 (\u2013230) = \u201355.8 kJ\/mol\r\n\r\n\u0394S<\/em>\u00b0 = (\u2211\u0394S<\/em>\u00b0,\u00a0products<\/em>) \u2013 (\u2211\u0394S<\/em>\u00b0,\u00a0reactants<\/em>) = (70.0) \u2013 (\u201310.9) = +80.8\u00a0J\/mol K\r\n\r\nThe value of \u0394G<\/em>\u00b0 at 298 K is \u0394H<\/em>\u00b0 \u2013 T<\/em>\u0394S<\/em>\u00b0 = (\u201355,800)\u00a0\u2013 (298)(80.8) = \u201379,900\u00a0J\/mol\r\n\r\nK<\/em>\u00a0= exp(\u201379,900\/(8.314\u00a0\u00d7\u00a0298) = e<\/em>-32.2<\/sup>\u00a0=\u00a01.01\u00a0\u00d7\u00a010-14<\/sup>\r\n\r\n<\/div>","rendered":"

\n

Exercises<\/h3>\n

1. Classify each of the following as spontaneous or nonspontaneous processes:<\/p>\n

a)\u00a0 the browning of a cut apple slice on a snack tray over time<\/p>\n

b)\u00a0 the rolling of a ball uphill<\/p>\n

c)\u00a0\u00a0the formation of diamond from the graphite in your pencil<\/p>\n

d)\u00a0\u00a0the melting of ice cubes in a glass of water you are holding<\/p>\n

2. State the second law of thermodynamics.<\/p>\n

3. What sign would you expect for \u0394S<\/em> for the following processes?<\/p>\n

a)\u00a0\u00a0water\u00a0freezing in a lake during a cold Alberta winter<\/p>\n

b)\u00a0\u00a0AB(s) + CD(s) \u2192 AC(g) + BD(g)<\/p>\n

c)\u00a0\u00a0a balloon with a fixed amount of gas stretched to a larger volume<\/p>\n

d)\u00a0\u00a0the sublimation of dry ice<\/p>\n

e)\u00a0\u00a03 E2<\/sub>F2<\/sub>(g) \u2192 E6<\/sub>F6<\/sub>(g)<\/p>\n

4. Which of the following would you expect to have the higher standard molar entropy, S<\/em>\u2070?<\/p>\n

a)\u00a0\u00a0Br2<\/sub>(\u2113<\/span>) or Br2<\/sub>(g)<\/p>\n

b)\u00a0\u00a0NO2<\/sub>(g) or NO(g)<\/p>\n

c)\u00a0\u00a0C2<\/sub>H6<\/sub>(g) or C5<\/sub>H12<\/sub>(g)<\/p>\n

5. Calculate the \u0394S<\/em>\u2070 of the following reactions using the values listed in the appendix.<\/p>\n

a)\u00a0\u00a04 NH3<\/sub>(g) + 5 O2<\/sub>(g) \u2192 6 H2<\/sub>O(g)\u00a0 + 4 NO(g)<\/p>\n

b)\u00a0\u00a02 HgO(s) \u2192 2 Hg(\u2113<\/span>)\u00a0 + O2<\/sub>(g)<\/p>\n

c)\u00a0\u00a03 FeCl2<\/sub>(s) + KNO3<\/sub>(s) + 4 HCl (aq) \u2192 3 FeCl3<\/sub>(s) + KCl(s) + NO(g) + 2 H2<\/sub>O(\u2113<\/span>)<\/p>\n

6. Draw a diagram showing the approximate entropy change of water from -100\u2070C to 250\u2070C.<\/p>\n

7. A chemical reaction has \u0394H<\/em>\u2070 = -43.5 kJ and \u0394S<\/em>\u2070 = -65.8 J\/K. Calculate \u0394G<\/em>\u2070 at 298 K. Is this a spontaneous process?<\/p>\n

8. Using data from the appendix, determine \u0394G<\/em>\u2070 for all reactions listed in question 5.<\/p>\n

9. Find the standard Gibbs energy change for the reaction<\/p>\n

CaCO3<\/sub>(s)\u00a0\u2192 CaO(s)\u00a0+ CO2<\/sub>(g)<\/p>\n

The\u00a0\u0394Gf<\/sub>\u00b0<\/em>\u00a0values for the three components of this reaction system are CaCO3<\/sub>(s): \u20131128\u00a0kJ\u00a0mol\u20131<\/sup>; CaO(s): \u2013603.5\u00a0kJ\/mol; CO2<\/sub>(g): \u2013137.2\u00a0kJ\/mol.[1]<\/sup><\/a><\/p>\n

10. Using the appendix data, determine the approximate temperature at which the following processes are at equilibrium:<\/p>\n

a)\u00a0\u00a0CH2<\/sub>Cl2<\/sub>(\u2113<\/span>) \u2192 CH2<\/sub>Cl2<\/sub>(g)<\/p>\n

b)\u00a0\u00a0CH3<\/sub>OH(\u2113<\/span>) \u2192 CH3<\/sub>OH(g)<\/p>\n

11. Determine if the following reactions would be spontaneous at any temperature, nonspontaneous at any temperature, spontaneous at low temperature but not high temperature, or spontaneous at high temperature but not low temperature:<\/p>\n

a)\u00a0\u00a0\u0394H<\/em>\u2070 = -750 kJ and \u0394S<\/em>\u2070 = 250 J\/K<\/p>\n

b)\u00a0\u00a0\u0394H<\/em>\u2070 = -100 kJ and \u0394S<\/em>\u2070 = -300 J\/K<\/p>\n

c)\u00a0\u00a0\u0394H<\/em>\u2070 = 95 kJ and \u0394S<\/em>\u2070 = -70 J\/K<\/p>\n

d)\u00a0\u00a0\u0394H<\/em>\u2070 = 400 kJ and \u0394S<\/em>\u2070 = 500 J\/K<\/p>\n

12. The K<\/em>a<\/sub> for acetic acid, CH3<\/sub>COOH, is 1.75 x 10-5<\/sup> at 25\u2070C.<\/p>\n

a)\u00a0\u00a0Using the K<\/em>a<\/sub> value, determine the \u0394G<\/em>\u2070 for the dissociation of acetic acid in aqueous solution.<\/p>\n

b)\u00a0\u00a0What is the value of \u0394G <\/em>when [H+<\/sup>] is 7.5 x 10-2<\/sup> M, [CH3<\/sub>COO–<\/sup>] is 2.5 x 10-2<\/sup> M, and [CH3<\/sub>COOH] is 0.10 M?<\/p>\n

13. Calculate the equilibrium constant for the reaction H+<\/sup>(aq)\u00a0+ OH–<\/sup>(aq)\u00a0\u2192\u00a0H2<\/sub>O(\u2113<\/span>)\u00a0from the following data:<\/p>\n\n\n\n\n\n
<\/td>\nH+<\/sup>(aq)<\/strong><\/td>\nOH–<\/sup>(aq)<\/strong><\/td>\nH2<\/sub>(\u2113<\/span><\/em>)<\/strong><\/td>\n<\/tr>\n
\u0394H\u00b0<\/strong><\/span>f<\/sub><\/em>, kJ mol\u20131<\/strong><\/td>\n0<\/td>\n\u2013230.0<\/td>\n\u2013285.8<\/td>\n<\/tr>\n
S<\/em><\/strong>\u00b0, J K\u20131\u00a0mol\u20131<\/strong><\/td>\n0*<\/td>\n\u201310.9<\/td>\n70.0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

* Note that the standard entropy of the hydrogen ion is zero by definition. This reflects the fact that it is impossible to carry out thermodynamic studies on a single-charged species. All ionic entropies are relative to that of H+<\/sup>(aq), which explains why some values (as for the aqueous hydroxide ion) are negative.[2]<\/sup><\/a><\/p>\n

14. Using data from the appendix, calculate the equilibrium constants at 298 K for all the reactions in question 5.<\/p>\n<\/div>\n

\n

Answers<\/h3>\n

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

a)\u00a0\u00a0spontaneous<\/p>\n

b)\u00a0nonspontaneous<\/p>\n

c)\u00a0\u00a0nonspontaneous<\/p>\n

d)\u00a0\u00a0spontaneous<\/p>\n

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

a)\u00a0\u00a0\u0394S =\u00a0–<\/p>\n

b)\u00a0\u00a0\u0394S = +<\/p>\n

c)\u00a0\u00a0\u0394S = +<\/p>\n

d)\u00a0\u00a0\u0394S = +<\/p>\n

e)\u00a0\u00a0\u0394S =\u00a0–<\/p>\n

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

a)<\/p>\n

\u0394S<\/em>\u2070 = \u2211nS<\/em>\u2070(products) – \u2211mS<\/em>\u2070(reactants)<\/p>\n

\u0394S<\/em>\u2070 = (6 S<\/em>\u2070 H2<\/sub>O(g) \u00a0+ 4 S<\/em>\u2070 NO(g)) – (4 S<\/em>\u2070 NH3<\/sub>(g) \u00a0+ 5 S<\/em>\u2070 O2<\/sub>(g))<\/p>\n

\u0394S<\/em>\u2070 = [(6 x 188.8 J\/mol K) + (4 x 210.8 J\/mol K)] – [(4 x 192.8 J\/mol K) + (5 x 205.2 J\/mol K)]<\/p>\n

\u0394S<\/em>\u2070 = 178.8 J\/mol K<\/p>\n

b)<\/p>\n

\u0394S<\/em>\u2070 = \u2211nS<\/em>\u2070(products) – \u2211mS<\/em>\u2070(reactants)<\/p>\n

\u0394S<\/em>\u2070 = (2 S<\/em>\u2070 Hg(\u2113<\/span>) + S<\/em>\u2070 O2<\/sub>(g)) – (2 S<\/em>\u2070 HgO)<\/p>\n

\u0394S<\/em>\u2070 = [(2 x 75.9 J\/mol K) + (205.2 J\/mol K)] – (2 x 70.3 J\/mol K)<\/p>\n

\u0394S<\/em>\u2070 = 216.4 J\/mol K<\/p>\n

c)<\/p>\n

\u0394S<\/em>\u2070 = \u2211nS<\/em>\u2070(products) – \u2211mS<\/em>\u2070(reactants)<\/p>\n

\u0394S<\/em>\u2070 = (3 S<\/em>\u2070 FeCl3<\/sub>(s) + S<\/em>\u2070 KCl(s) + S<\/em>\u2070 NO(g) + 2 S<\/em>\u2070 H2<\/sub>O(\u2113<\/span>))- (3 S<\/em>\u2070 FeCl2<\/sub>(s) + S<\/em>\u2070 KNO3<\/sub>(s) + 4 S<\/em>\u2070 HCl (aq))<\/p>\n

\u0394S<\/em>\u2070 = [(3 x 142.3 J\/mol K) + (82.6 J\/mol K) + (210.8 J\/mol K) + (2 x 70.0 J\/mol K)] – [(3 x 118.0 J\/mol K) + (133.1 J\/mol K) + (4 x 56.5 J\/mol K)]<\/p>\n

\u0394S<\/em>\u2070 = 147.2 J\/mol K<\/p>\n

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

\u0394G<\/em>\u2070 = \u0394H<\/em>\u2070 – T<\/em>\u0394S<\/em>\u2070<\/p>\n

\u0394G<\/em>\u2070 = -43.5 kJ \u2013 [(298 K)(-65.8 J\/K)]<\/p>\n

\u0394G<\/em>\u2070 = -23.9 kJ<\/p>\n

\u0394G<\/em>\u2070 is negative therefore this is a spontaneous process.<\/p>\n

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

\u0394G\u00b0<\/em>\u00a0= (\u2013603.5 \u2013137.2) \u2013 (\u20131128)\u00a0kJ\/mol =\u00a0+130.9\u00a0kJ\/mol,\u00a0<\/strong>indicating that the process is not spontaneous under standard conditions (i.e., solid calcium carbonate will not form solid calcium oxide and CO2<\/sub>\u00a0at 1 atm partial pressure at 25\u00b0C.)<\/p>\n

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

a) \u00a0spontaneous at all temperatures<\/p>\n

b)\u00a0\u00a0spontaneous at low temperatures, nonspontaneous at high temperatures<\/p>\n

c)\u00a0\u00a0nonspontaneous at all temperatures<\/p>\n

d)\u00a0\u00a0spontaneous at high temperatures, nonspontaneous at low temperatures<\/p>\n

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

\u0394H<\/em>\u00b0 = (\u2211\u0394H<\/em>\u00b0f<\/sub><\/em>,\u00a0products<\/em>) \u2013 (\u2211\u0394H<\/em>\u00b0f<\/sub><\/em>,\u00a0reactants<\/em>) = (\u2013285.8) \u2013 (\u2013230) = \u201355.8 kJ\/mol<\/p>\n

\u0394S<\/em>\u00b0 = (\u2211\u0394S<\/em>\u00b0,\u00a0products<\/em>) \u2013 (\u2211\u0394S<\/em>\u00b0,\u00a0reactants<\/em>) = (70.0) \u2013 (\u201310.9) = +80.8\u00a0J\/mol K<\/p>\n

The value of \u0394G<\/em>\u00b0 at 298 K is \u0394H<\/em>\u00b0 \u2013 T<\/em>\u0394S<\/em>\u00b0 = (\u201355,800)\u00a0\u2013 (298)(80.8) = \u201379,900\u00a0J\/mol<\/p>\n

K<\/em>\u00a0= exp(\u201379,900\/(8.314\u00a0\u00d7\u00a0298) = e<\/em>-32.2<\/sup>\u00a0=\u00a01.01\u00a0\u00d7\u00a010-14<\/sup><\/p>\n<\/div>\n

  1. Question and solution from Chem1 Virtual Textbook, Stephen Lower\/CC-BY-SA-3.0 ↵<\/a><\/li>
  2. Question and solution from Chem1 Virtual Textbook, Stephen Lower\/CC-BY-SA-3.0 ↵<\/a><\/li><\/ol><\/div>","protected":false},"author":124,"menu_order":7,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":["jessie-a-key"],"pb_section_license":"cc-by"},"chapter-type":[],"contributor":[61],"license":[52],"class_list":["post-1092","chapter","type-chapter","status-publish","hentry","contributor-jessie-a-key","license-cc-by"],"part":1071,"_links":{"self":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/1092","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":2,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/1092\/revisions"}],"predecessor-version":[{"id":1462,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/1092\/revisions\/1462"}],"part":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/parts\/1071"}],"metadata":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapters\/1092\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/media?parent=1092"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/pressbooks\/v2\/chapter-type?post=1092"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/contributor?post=1092"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistryclone\/wp-json\/wp\/v2\/license?post=1092"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}