ࡱ> '` bjbjLULU _3.?.?Id $@HHHPL@Flmoooooohro |oRmm 0s…$HR!L 0F)||ooF@@@DgnT@@@n@@@ AP Chemistry Name ________________________ Fall Semester Practice Multiple Choice Period _____ Multiple Choice: Briefly show/explain why the multiple choice answer is correct in the space provided (no calculator). 1. Copper has two naturally occurring isotopes, 63Cu and 65Cu. What is the abundance of 65Cu if the average atomic mass of copper is 63.5? (A) 90% (B) 70% (C) 50% (D) 25% 2. Which of the following particles is emitted by an atom of 39Ca when it decays to produce an atom of 39K? (A) 10n (B) 11H (C) b- (D) b+ 3. After 195 days, a 10.0 g sample of pure 95Zr has decayed to the extent that only 1.25 g of the original 95Zr remains. The half-life of 95Zr is closest to (A) 195 days (B) 98 days (C) 65 days (D) 49 days Questions 4-5 The diagram shows the energy levels (in eV) for hydrogen gas.  4. What is the energy, in eV, of a photon emitted by an electron as it moves from the n = 6 to the n = 2 energy level in a hydrogen atom. (A) 0.38 eV (B) 3.02 eV (C) 3.40 eV (D) 13.60 eV 5. A photon having energy of 9.4 eV strikes a hydrogen atom in the ground state. Why is the photon not absorbed by the hydrogen atom? (A) The atom's orbital electron is moving too fast (B) The photon striking the atom is moving too fast. (C) The photon's energy is too small. (D) The photon is being repelled by electrostatic force. Questions 6-8 (A) Heisenberg uncertainty principle (B) Pauli exclusion principle (C) Hund's rule (principle of maximum multiplicity) (D) Shielding effect 6. Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic. 7. Indicates that an atomic orbital can hold no more than two electrons. 8. Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron. 9. Which set of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (Z = 31)? (A) 4,0,0, (B) 4,0,1, (C) 4,1,1, (D) 4,1,2, Questions 10-12 refer to neutral atoms for which the atomic orbitals are represented below. (A) 1s() (B) 1s() 2s( ) 2p( )( )( ) (C) 1s() 2s() 2p( )( )( ) (D) [Ar] 4s() 3d()()()( )( ) 10. Is in an excited state 11. Has exactly five valence electrons 12. Has the highest first ionization energy 13. The first seven ionization energies of element X are shown in the table below. Ionization Energy (kJmol-1)1st2nd3rd4th5th6th7th7871,5803,2004,40016,00020,00024,000On the basis of these data, element X is most likely a member of which of the following groups of elements? (A) Alkaline earth metals (B) Boron group (C) Carbon group (D) Nitrogen group 14. In which of the following are the chemical species correctly ordered from smallest radius to largest radius? (A) B < C < N (B) At < Xe < Kr (C) CI < S < S2- (D) Na < Na+ < K 15. Of the following elements, which would be expected to have chemical properties most similar to those of sulfur, S? (A) Br (B) CI (C) P (D) Se 16. Which pair of ions should have the highest lattice energy? (A) Na+ and Br- (B) Li+ and F- (C) Cs+ and F- (D) Li+ and O2- 17. Which molecule has the weakest bond? (A) CO (B) O2 (C) Cl2 (D) N2 18. Which pair of atoms should form the most polar bond? (A) F and B (B) C and O (C) F and O (D) N and F 19. Which species has a valid non-octet Lewis structure? (A) GeCl4 (B) SiF4 (C) NH4+ (D) SeCl4 20. For which molecule are resonance structures necessary to describe the bonding satisfactorily? (A) H2S (B) SO2 (C) CO2 (D) OF2 21. The Lewis structure for SeS2 with zero formal charge has a total of (A) 2 bonding pairs and 7 nonbonding pairs of electrons. (B) 2 bonding pairs and 6 nonbonding pairs of electrons. (C) 3 bonding pairs and 6 nonbonding pairs of electrons. (D) 4 bonding pairs and 5 nonbonding pairs of electrons. Questions 22-24 refer to the following molecules. (A) CO (B) CH4 (C) HF (D) PH3 22. Contains two p-bonds 23. Has the highest dipole moment (most polar) 24. Has a molecular geometry that is trigonal pyramidal 25. Which of the following molecules contains bonds that have a bond order of 1.5? (A) N2 (B) O3 (C) NH3 (D) CO2 26. CCl4, CO2, PCl3, PCl5, SF6 Which does NOT describe any of the molecules above? (A) Linear (B) Octahedral (C) Square planar (D) Tetrahedral 27. According to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3, and H2O is best accounted for by the (A) increasing strength of the bonds (B) decreasing size of the central atom (C) increasing electronegativity of the central atom (D) increasing number of unshared pairs of electrons 28. Which of the following is a formula for an acid? (A) CH3COCH3 (B) CH3CH2COOH (C) CH3CH2CH2OH (D) CH3CH2OCH3 29. Which is NOT a structural isomer of 2-methylpentane? (A) hexane (B) 3-methylpentane (C) 2,2-dimethylbutane (D) 4-methylpentane 30. Types of hybridization exhibited by carbon atoms in a molecule of propyne, CH3CCH, include which of the following? I. sp II. sp2 III. sp3 (A) I only (B) II only (C) III only (D) I and III only 31. Which of the following best explains why the normal boiling point of CCI4(I) (350 K) is higher than the normal boiling point of CF4(I) (145 K)? (A) The C-CI bonds in CCI4 are less polar than the C-F bonds in CF4. (B) The C-CI bonds in CCI4 are weaker than the C-F bonds in CF4. (C) The mass of the CCI4 molecule is greater than that of the CF4 molecule. (D) The electron cloud of the CCI4 molecule is more polarizable than that of the CF4 molecule. 32. Which of the following substances exhibits significant hydrogen bonding in the liquid state? (A) CH2F2 (B) N2H4 (C) CH3OCH3 (D) C2H4 Questions 33-34 refer to a various points in time during an experiment conducted at 1.0 atm. Heat is added at a constant rate to a sample of a pure substance that is solid at time to. The graph below shows the temperature of the sample as a function of time.  (A) t1 (B) t2 (C) t3 (D) t5 33. Time when the average distance between particles is greatest 34. Time when the temperature of the substance is between its melting point and its boiling point 35. Heat energy is added slowly to a pure solid covalent compound at its melting point. About half of the solid melts to become a liquid. Which of the following must be true about this process? (A) Covalent bonds are broken as the solid melts. (B) The temperature of the solid/liquid mixture remains the same while heat is being added. (C) The volume of the compound increases as the solid melts to become a liquid. (D) The average kinetic energy of the molecules becomes greater as the molecules leave the solid state and enter the liquid state. 36. Of the following gases, which has the greatest average molecular speed at 298 K? (A) Cl2 (B) NO (C) H2S (D) HCN 37. At approximately what temperature will 40. g of argon gas at 2.0 atm occupy a volume of 22.4 L? (A) 600 K (B) 550 K (C) 270 K (D) 140 K 38. Three gases in the amounts shown in the table are added to a previously evacuated rigid tank. GasArCH4N2Amount0.35 mol0.90 mol0.25 mol If the total pressure in the tank is 3.0 atm at 25oC, the partial pressure of N2(g) in the tank is closest to (A) 0.75 atm (B) 0.50 atm (C) 0.33 atm (D) 0.25 atm 39. At which of the following temperatures and pressures would a real gas be most likely to deviate from ideal behavior? Temperature (K) Pressure (atm) (A) 100 50 (B) 200 5 (C) 300 0.01 (D) 500 0.01 40. In which process are covalent bonds broken? (A) Solid silver melts. (B) Solid potassium chloride melts. (C) Solid carbon (graphite) sublimes. (D) Solid iodine sublimes. 41. A closed rigid container contains distilled water and N2(g) at equilibrium. Actions that would increase the concentration of N2(g) in water include which of the following? I. Shaking the container vigorously II. Raising the temperature of the water III. Injecting more N2(g) into the container (A) I only (B) II only (C) III only (D) I and II only 42. What is the mole fraction of ethanol in a 6 molal aqueous solution? (A) 0.006 (B) 0.1 (C) 0.08 (D) 0.2 43. What additional information is needed to determine the molality of a 1.0-M glucose (C6H12O6) solution? (A) Volume of the solution (B) Temperature of the solution (C) Solubility of glucose in water (D) Density of the solution 44. A solution of toluene (MM = 90 g) in benzene (MM = 80 g) is prepared. The mole fraction of toluene in the solution is 0.2. What is the molality of the solution? (A) 0.2 (B) 0.5 (C) 2 (D) 3 45. Which of the following aqueous solutions has the highest boiling point at 1.0 atm? (A) 0.20 M CaCl2 (B) 0.25 M Na2SO4 (C) 0.30 M NaCl (D) 0.40 M C6H12O6 46. _CH3OCH3(g) + _O2(g) _CO2(g) + _ H2O(g) When the equation above is balanced using the lowest whole-number coefficients, the coefficient for O2(g) is (A) 6 (B) 4 (C) 3 (D) 2 47. What mass of KBr (MM = 119 g" mol-1) is required to make 250. mL of a 0.400 M KBr solution? (A) 0.595 g (B) 1.19 g (C) 2.50 g (D) 11.9 g 48. Na2CO3(s) + 2 HCl(aq) 2 NaCl(aq) + CO2(g) + H2O(l) In a laboratory, a student wants to quantitatively collect the CO2(g) generated by adding Na2CO3(s) to 2.5 M HCI(aq). The student sets up the apparatus to collect the CO2 gas over water. The volume of collected gas is much less than the expected volume because CO2 gas (A) is soluble in water (B) is produced at a low pressure (C) is more dense than water vapor (D) has a larger molar mass than that of N2 gas, the major component of air 49. Which of the following would produce the LEAST mass of CO2 if completely burned in excess oxygen gas? (A) 10.0 g CH4 (B) 10.0 g CH3OH (C) 10.0 g C2H4 (D) 10.0 g C2H6 50. A solution of RbCl (MM = 121 gmol-1) contains 11.0 % RbCl by mass. From the following list, what is needed to determine the molarity of RbCl in the solution? I. Mass of the sample II. Volume of the sample III. Temperature of the sample (A) I only (B) II only (C) III only (D) I and II only 51. CS2(l) + 3 O2(g) CO2(g) + 2 SO2(g) When 0.60 mol of CS2(l) reacts as completely as possible with 1.5 mol of O2(g) according to the equation above, the total number of moles of reaction products is (A) 2.4 mol (B) 2.1 mol (C) 1.8 mol (D) 1.5 mol 52. What is the empirical formula of a hydrocarbon that is 10 % hydrogen by mass? (A) CH3 (B) C2H5 (C) C3H4 (D) C4H9 53. By mixing only 0.15 M HCl and 0.25 M HCl, it is possible to create all of the following solutions EXCEPT (A) 0.21 M (B) 0.18 M (C) 0.16 M (D) 0.14 M 54. 8 H2(g) + S8(s) 8 H2S(g) When 25.6 g of S8(s) (MM = 256 g" mol-1) reacts completely with an excess of H2(g) according to the equation above, the volume of H2S(g), measured at 0oC and 1.00 atm, produced is closest to (A) 30 L (B) 20 L (C) 10 L (D) 5 L 55. 2 N2H4 + N2O4 3 N2 + 4 H2O What mass of N2 can be produced when 8.0 g of N2H4 (MM = 32 g) and 9.2 g of N2O4 (MM = 92 g) react? (A) 8.4 g (B) 12.6 g (C) 7.8 g (D) 10.5 g 56. A student weighs out 0.0154 mol of pure, dry NaCI in order to prepare a 0.154 M NaCI solution. Of the following pieces of laboratory equipment, which would be most essential for preparing the solution? (A) 50 mL volumetric pipet (B) 100 mL Erlenmeyer flask (C) 100 mL graduated beaker (D) 100 mL volumetric flask Questions 57-60 The figures show portions of a buret used in a titration 0.0464 moles of monoprotic acid with a solution of Ba(OH)2. Figures I and 2 show the level of the Ba(OH)2 solution at the start and at the endpoint of the titration, respectively. Phenolphthalein was used as the indicator for the titration. Figure 1 Figure 2 57. What is the evidence that the endpoint of the titration has been reached? (A) The color of the solution in the buret changes from pink to colorless. (B) The color of the solution in the buret changes from blue to red. (C) The color of the contents of the flask changes from colorless to pink. (D) The color of the contents of the flask changes from blue to red 58. The volume of Ba(OH), used to neutralize the acid was closest to (A) 22.80 mL (B) 23.02 mL (C) 23.20 mL (D) 29.80 mL 59. The concentration of the Ba(OH)2 solution is closest to (A) 1 M (B) 2 M (C) 3 M (D) 4 M 60. What could explain why the student calculated a concentration of Ba(OH)2 that was too large? (A) An extra drop of phenolphthalein was added. (B) A small amount of the acid was not transferred to the titration flask. (C) A drop of Ba(OH)2 remained attached to the buret tip. (D) Rinsing the buret with distilled water just before filling it with the Ba(OH)2 to be titrated. 61. CaCl2(s) Ca2+ + 2 Cl- For the process of solid calcium chloride dissolving in water, represented above, the entropy change might be expected to be positive. However, DS for the process is actually negative. Which best helps to account for the net loss of entropy? (A) Cl- ions are much larger in size than Ca2+ ions. (B) The particles in solid calcium chloride are more ordered than are particles in amorphous solids. (C) Water molecules in the hydrated Ca2+ and Cl- ions are more ordered than they are in the pure water. (D) The Ca2+ and Cl- ions are more free to move around in solution than they are in CaCl2(s) 62. For which of the processes does entropy decrease (DS < 0)? (A) H2O(s) H2O(l) (B) Br2(l) Br2(g) (C) Crystallization of I2(s) from an ethanol solution (D) Thermal expansion of a balloon filled with CO2(g) 63. What mass of Cu(s) would be produced if 0.40 mol of Cu2O(s) was reduced completely with excess H2(g)? (A) 13 g (B) 25 g (C) 38 g (D) 51 g 64. A certain reaction is spontaneous at temperatures below 400 K but is not spontaneous at temperatures above 400 K. If DHo for the reaction is -20 kJ" mol-1 and it is assumed that DHo and DSo do not change appreciably with temperature, then the value of DSo for the reaction is (A) -50 J" mol-1" K-1 (B) -20.0 J" mol-1" K-1 (C) -0.05 J" mol-1" K-1 (D) -20 J" mol-1" K-1 65. Z X + Y A pure substance Z decomposes into two products, X and Y, as shown by the equation. Which of the following graphs of the concentration of Z versus time is consistent with the rate of the reaction being first order with respect to Z? (A) (B) (C) (D) Questions 66-67 refer to an experiment to determine the heat of solution of an ionic solid. A student used a calorimeter consisting of a polystyrene cup and a thermometer. The cup was weighed, then filled halfway with water, then weighed again. The temperature of the water was measured, and some of the ionic solid was added to the cup. The mixture was gently stirred until all of the solute dissolved and the lowest temperature reached by the water in the cup was recorded. The cup and its contents were weighed again. 66. The purpose of weighing the cup and its contents again at the end of the experiment was to (A) determine the mass of solute that was added. (B) determine the mass of the thermometer. (C) determine the mass of water that evaporated. (D) verify the mass of water that was cooled. 67. Suppose that during the experiment, a significant amount of solution spilled from the polystyrene cup before all of the solute dissolved. How does this affect the calculated value for the heat of solution of the ionic compound? (A) The calculated value is too large because less water was cooled as the remaining solute dissolved. (B) The calculated value is too large because some solute was lost with the spilled solution. (C) The calculated value is too small because less solute was dissolved than the student assumed. (D) The calculated value is too small because the total mass of the calorimeter contents was too small. 68. Pb(s) D Pb(l) Which of the following is true for the process represented above at 327oC and 1 atm? (The normal melting point for Pb(s) is 327o(C)) (A) DH = 0 (B) TDS = 0 (C) DS < 0 (D) DH = TDS 69. C(diamond) C(graphite) For the reaction represented above, the standard Gibbs free energy change, DGo298, has a value of -2.90 kJ" mol-1. Which of the following best accounts for the observation that the reaction does NOT occur (i.e. diamond is stable) at 298 K and 1.00 atm? (A) DSo for the reaction is positive. (B) The activation energy, Ea, for the reaction is very large. (C) The reaction is slightly exothermic (DHo < 0). (D) Diamond has a density greater than that of graphite. 70. When a solution is formed by adding some methanol, CH3OH, to water, processes that are endothermic include which of the following? I. Methanol molecules move water molecules apart as the methanol goes into solution. II. Water molecules move methanol molecules apart as the methanol goes into solution. III. Intermolecular attractions form between molecules of water and methanol as the methanol goes into solution. (A) I only (B) II only (C) III only (D) I and II only Answers #PExplanation1dAverage = (Mass1 x Abundance1) + (Mass2 x Abundance2) 63.5 = (63)(1  x) + (65)(x) = 63  63x + 65 x \ x = 0.25 (25 %)2d3920Ca 3919K + 01b3cIt takes 3 half-lives to reduce the radioactivity to 1/8 (1.25/10.0). 195 days/3 = 65 days4bFrom the diagram: E6 = -0.38 eV and E2 = -3.40 eV DE = E2  E6 = -3.40 eV  (-0.38 eV) = -3.02 eV5cThe electron can only absorb energy that will move it to a higher energy level. 9.4 eV is not enough energy (the minimum needed is -3.40 eV  (-13.60 eV) = 10.2 eV).6cThe orbital diagram for C,1s() 2s() 2p( )( )( ), has two unpaired electrons (Hund's rule) = paramagnetic.7bPauli states that no orbital can contain electrons with the same spin. Since two spins, this limits the number to two electrons.8aHeisenberg states that the wave nature of matter (DeBroglie) limits what we can know about position and velocity.9cElectron # 31 is located in the 4th row (n = 4), 13th column (p section, l = 1), which limits ml = 1, 0 or -1 and ms = + or - \ (4, 1, 1, ) fits requirement10b1s() 2s( ) 2p( )( )( ): The 2p electron is in an excited state, otherwise it would go into the 2s sublevel.11c1s() 2s() 2p( )( )( ): The 2 2s electrons and 3 2p electrons are in the valence shell (highest energy level) \ five.12a1s(): The first ionized electron is from the 1s sublevel. It takes the most energy to remove electrons that are close to nucleus.13cThe biggest jump in ionization energy occurs between 4 and 5, which means 4 valence electrons \ Carbon group.14cAtomic radius increases going left and down in periodic table. 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layt{TTTTTUU%U&U/U0UIUJU]U^UUUUUUUUUUUU./0235ШѨڨۨ!"$'./0ʼްްhFho|2>*CJH*aJhFho|2>*CJaJUhHho|2>*CJaJho|2CJaJhFho|2CJH*aJhFho|2CJaJhaA+ho|2;CJaJh=ho|2CJaJ@UUUUUUlNN33$If]^gd{l_$$If]^a$gd{l_kd;$$IflF@ t06    44 layt{90 g C x 1 mol/12 g = 7.5 mol/7.5 = 1 x 3 = 353dThe resulting solution must have a concentration between the two solutions added together. 0.14 M is less then both.54b25.6 g S8 x 256 g/mol x 8 mol H2S/1 mol S8 = 0.8 mol 0.8 mol x 22.4 L/mol = 20 L55a0.25 mol N2H4 x 3 mol N2 x 28 g N2 = 10.5 g 2 mol N2H4 1 mol N2 0.1 mol N2O4 x 3 mol N2/1 mol N2O4 x 28 g N2 = 8.4 g56d0.0154 mol NaCl x 1 L/0.154 mol = 0.1 L (100 mL) The most accurate way to measure 0.1 L of solution is to use a volumetric flask.57cPhenolphthalein changes from clear (acid) to pink (base)58cFinal volume Initial volume = Change in volume 35.75 mL 12.55 mL = 23.20 mL59a0.0464 mol H+ x 1 mol OH- x 1 mol B(A).. = 0.0232 mol B(A).. 1 mol H+ 2 mol OH- 0.0232 mol B(A)../0.0232 L = 1 M60bMBa(OH)2 = ( mol H+)/VBa(OH)2 \ too large MBa(OH)2 = too small VBa(OH)2 Titrating less acid would result in smaller VNaOH61cDissolving involves two process; (1) separation into ions, which increases disorder (+DS) and (2) ions combining with water (solvation), which decreases disorder (-DS).62cDisorder decreases when I2(aq) I2(s). Disorder increases when s l g (A) and (B). Disorder also increases when gas molecules spread out (D).63dCu2O + H2 2 Cu + H2O (balancing wasn't necessary because mole Cu in reactants and products are equal) 0.80 mol Cu x 63.5 g/mol = 51 g64aTthreshold = DH/DS DS = DH/Tthreshold = -20 kJ" mol-1/400 = -0.05 kJ" mol-1" K-1 -0.05 kJ" mol-1" K-1 x 1000 J/1 kJ = -50 J" mol-1" K-165dFor a first order reaction, the straight line graph is ln[Z] vs.U/035Q33$$If]^a$gd{l_kdŖ$$IflF@ t06    44 layt{$If]^gd{l_lNN33$If]^gd{l_$$If]^a$gd{l_kdO$$IflF@ t06    44 layt{:klNN33$If]^gd{l_$$If]^a$gd{l_kdٗ$$IflF@ t06    44 layt{09:\]^_ijktuvw֩ש'()+,.fghjkmzêϪѪӪ͵͵͵͵h3aho|2CJH*aJh/CJaJh3aho|2CJaJhaA+ho|2;CJaJhHho|2>*CJaJh=ho|2CJaJho|2CJH*aJhFho|2CJH*aJho|2CJaJhFho|2CJaJ8kשQ33$$If]^a$gd{l_kdc$$IflF@ t06    44 layt{$If]^gd{l_ש(),.gQ33$$If]^a$gd{l_kd$$IflF@ t06    44 layt{$If]^gd{l_ghkmlNN33$If]^gd{l_$$If]^a$gd{l_kdw$$IflF@ t06    44 layt{ê3lNN33$If]^gd{l_$$If]^a$gd{l_kd$$IflF@ t06    44 layt{Ӫ۪ܪߪ#$123?BSTUWXZ[bmnqx(DRTڵڵڡ}ڵ}te}}t}h3aho|2CJOJQJaJho|2CJH*aJh3aho|2CJH*aJhaA+ho|2;CJaJhHho|2>*CJaJh=ho|2CJaJho|2CJH*aJh3aho|2CJH*aJho|2CJaJhaA+CJaJhaA+>*CJaJh3aho|2CJaJh3aho|2>*CJH*aJh3aho|2>*CJaJ'3TUXZyQ33$$If]^a$gd{l_kd$$IflF@ t06    44 layt{$If]^gd{l_yTĬQ33$$If]^a$gd{l_kd$$IflF@ t06    44 layt{$If]^gd{l_Ĭprt "RTVX\`bdfhjlʮ̮BDJLPRVZ\fhjl~fhlnrho&CJaJh=ho|26CJaJh=ho|2CJH*aJ hZyho|2CJOJQJ^JaJhHho|2>*CJaJho&ho|26CJaJhZyho|2CJOJQJaJhaA+ho|2;CJaJh=ho|2CJaJh/CJaJ6Ĭ"JS55$$If]^a$gd{l_kd$$IflF@ t06    44 layt{$If]^gd{l_JLRV&nPP1 $If]^gd{l_$$If]^a$gd{l_kd%$$IflF@ t06    44 layt{&fhnrS55$$If]^a$gd{l_kd$$IflF@ t06    44 layt{$If]^gd{l_rt &*.2fjnrtvz|?@BCEJܰܜܚ܎ܜ܎ܜhHho|2>*CJaJUhaA+ho|2;CJaJh/CJaJ hh5fho|2CJOJQJ^JaJh=ho|2CJH*aJhZyho|2CJOJQJaJh=ho|2CJaJh=ho|2CJH*aJho&ho|26CJaJ2rtv4kd1$$IflF@ t06    44 layt{$If]^gd{l_ $If]^gd{l_v|?@5kd$$IflF@ t06    44 layt{$If]^gd{l_$$If]^a$gd{l_ t. (zero order is [Z] vs. t and second order is 1/[Z] vs. t)66aAt the end of the experiment, the cup contained solute and water. If this value is subtracted from the mass of the cup and water, then the difference is the mass of the solute.67aThe heat needed to dissolve the remaining solute had to come from less water, which would make DT greater than it should have been (DH = -mcDT) \ DH would be too large.68dAt the normal melting point: DG = 0 = DH  TDS \ DH = TDS69bThe reaction is spontaneous, but it must not occur at a fast rate. This could be because the activation energy @CE5kd=$$IflF@ t06    44 layt{$If]^gd{le$$If]^a$gd{leJLZ\^bhj @ACDFؽةءؽةؓؽة؋ؽ{{h5*jh5*Uh4yho&CJaJUho&hZy6CJaJhZyCJaJhaA+ho|2;CJaJh/CJaJhHho|2>*CJaJhZyho|2CJOJQJaJh=ho|2CJaJho&ho|26CJaJho&ho|26CJOJQJaJ0S55$$If]^a$gd{lekdÞ$$IflF@ t06    44 layt{$If]^gd{le O11$$If]^a$gd{lekdI$$IflF@ t06    44 layt{ $If]^gdZyleis so high, that it takes too much energy to start the process.70dBreaking solute-solute bonds in methanol and water is endothermic, but forming solute-solute bonds between methanol and water is exothermic.     @ADFS55$$If]^a$gd{lkdϟ$$IflF@ t06    44 layt{$If]^gd{leFSNLLLLLgdo|2kdU$$IflF@ t06    44 layt{$If]^gd{lh4yh5*jh5*Ugdo|2800P:pT/ =!8"#$% = 01hP:pKB/ =!8"#$% P `!U8*6Ju 2 Vxڅ tW}߻,FeTh)iQcڊH"bB"jJbiQRK J)JſMR#D99|γ>>ups7{3~׬c@\_s?,͚hy^^bKxRd#e!;#O9 žtq't0'w릿Sa:妧SfC _Wĺ ;5jw_-%Y`J|em%"l/޾L7&5A+&Wn ~D*oD[ΓlH|6 (~D f/3/AE>`=,a n)BNh6C.#W@=lY2@6E6`ͷ2;,̇>g$;v4&XpôLh!-lk#V#G I@I&51ນk~6hΛ z$|l"dg'!<^F}Nu-׉Lǀ*?9/G`d)?3m?zNӠ^z_C|d˹6GfLcg֐mg 'S49 ˦IqR޽I\#;,ޭ0f,h#X;č})Iw}gۻ#m;6sP v{YٺnW7fhh+D]pw9#Ef59bIL2 Ⲏ4X1ZNj:Q4iW5GT6D,U"IUC#QD:*B)aⶼ(.J-K/A+eGw.r#GٲΖaA:ڶ )1n{J*.W@EJLUEɆ̄"lJC @+mo+Z7e"d9rad=;>%S$ .+'?x8"jx)v5ë0yr% ^<M7/Pifu-7Vv.H 7\3}?[3柷:;j'ģ=)oE'Mϝab{4[.Ҭ֬?] ޲-[7q3_pɻ ȝ'YN]-"t*]TQ*SĩY"K%"5 s) G5Nƈ`=R#D~Y /)s`ÿEZO&Rc+f3Y",fa&Qnvj=v?A_g:JQTy)"6 ^lCJ`)%\)\5 ɢf6d4jS)&QA-|q} 'ל#l'UPS)OB2J*WOj8Pqj:Q;Ֆ:VjAOf} MU(Vu'pJELVoj(žHTJSq=U:Qʦ`³P/KϪ"bRs'XwjPR[ߓjĊtڬ^hu\ORhuVT3gCUnJwVWu'~Hm?tkuHWgY)w qDBLG$=U;vKWSn~DM֏AjH5MUzJԑX#Z87>jUMA̘J4']]3U+F~MQ{I131__oc^ Yo8՞Fv4P=L%$ꡦ×D=qA?U1^Q47Az0uk7cCyC7iYu}Y^֗Y}^?/YyP1Rru,-}K.з<˙%32M!2Vz}NFk2^AUsQoՠv-1w>mZ3uA{7O݁_RҘ Қd9yT*s@#i[#,)-^,+/+`Hq"P4C1g(ӼL).A1K)RYI{GJ~tA\Јt0} cy]H@oس#Goe ݾ r쥬%?C}5ƾv8'ܞQ79*[}nu߀=w;6}VS7{w7k\μ^ϛx]xs{?F̻{?1ǻxًOlwMbQg3,>`KM+eF-AZ\|6ZPZAE*4*T]Z;l3B|j9q|͹ ;2nȺx% goLWr#sA#P|CﱗXŏcVB=åלWx;N'~]]E5n[Fy{no&8|W} g|s>uCns甹8W8;Akrp =U%4r)]PJt) awsi⣑7D XA߈%:#K@!?HM'ަO[@/]Q7Q@\А:!ԆAR䀥uVQ P1EA.OKN2 aSȣYI">࿓ھ]Q5ׅуxt?0'eOgL=qE@HTKtG[/u?5aӺx9 >,df&2^!lޝ24wA#Qm%_VX hr >v _>Yۙt9찾ٺd}C*ÜCxnي<]7L4Xe!6wj27c*]}o_ڞmsctu#]amv+jO8PN!W1W &VZש_Nz1A`!+㉇u_ (ٺ3$xڕxUŶg9g!\Jh{FDEj轅jE"@ $( &*CC{y{~ΚUf>'bs>?c^[>^"2 +;xAY$z)[k~UL]1Sz#\n3F0iFj7RwFMcQ٘a1ō`#i0@3./bʗH[?sH>n]A ̿h-xs_k<ͮSǼ| Gw(ސMޒ g`%Ç%Aڠh97ԕoȿByxh18Տ1N<Zu\5AЉ癞x ăΞi i<y_g|2?Xosy?>c2I"R.b)b)"Z GXD2X&bHClF|+*"^qF<^F3c32xK3dh 3JFШ&#QK`Q5Lל3<' xNso̣yRza).$40[zL0Q1VAsܤΚ9sggCfa6#h;g)v4#7>kN/skfz-ssCh+ gL8c4gd} "gr69)`k}霵vd.@OR_e>5ҿ^zw{wa> 5#鼠S:<XqO7oJz`s s:ws;ONti]vP;k̡N"=qsXзDAs9/ͩ=Xl]'N9K"fN@tqrҬާ:tg}DT ZҜ?Ŏ/sJOw[ |S4[&|`ΓJ|jzHr3yOK#kn¸47__uHt~ыt3H&`frW8 ׋x;YjocQ?cQ?Ymr~G`b?E/r<5[t-[4jM 祹c:yjN2Ӝ$3ݙfnpcOw f )f[smQx`3 z _oĺE/r_Cs7I.wy:%pM#vɛ]D{?wPӻ  F,="OȳYY\w`߃b= _yjFn {V;%3W)v)9+*|]w7D>O|qv(,b_Yoa`)sK`F ` 'nCͩv9jq ,B`/E7_%r&'KT{f`?b7Gn}OX9*G2. 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