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Predict the sign of the entropy change

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Reference no: EM131530174

Part -1:

Question:

1. Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds:

(a) PbCl2
(b) Ag2S
(c) Sr3(PO4)2
(d) SrSO4

2. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
(a) Ag2SO4
(b) PbBr2
(c) AgI
(d) CaC2O4·H2O

3. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:
(a) AgBr: [Ag+] = 5.7 × 10-7 M, [Br-] = 5.7 × 10-7 M
(b) CaCO3: [Ca2+] = 5.3 × 10-3 M, [CO32-] = 9.0 × 10-7 M
(c) PbF2: [Pb2+] = 2.1 × 10-3 M, [F-] = 4.2 × 10-3 M
(d) Ag2CrO4: [Ag+] = 5.3 × 10-5 M, 3.2 × 10-3 M
(e) InF3: [In3+] = 2.3 × 10-3 M, [F-] = 7.0 × 10-3 M

4. Calculate the molar solubility of AgBr in 0.035 M NaBr (Ksp = 5 × 10-13).

Part -2:

1. A helium-filled balloon spontaneously deflates overnight as He atoms diffuse through the wall of the balloon. Describe the redistribution of matter and/or energy that accompanies this process.

2. Arrange the following sets of systems in order of increasing entropy. Assume one mole of each substance and the same temperature for each member of a set.
(a) H2(g), HBrO4(g), HBr(g)
(b) H2O(l), H2O(g), H2O(s)
(c) He(g), Cl2(g), P4(g)

3. Predict the sign of the entropy change for the following processes.
(a) An ice cube is warmed to near its melting point.
(b) Exhaled breath forms fog on a cold morning.
(c) Snow melts.

4. "Thermite" reactions have been used for welding metal parts such as railway rails and in metal refining. One such thermite reaction is Fe2O3(s) + 2Al(s) ? Al2O3(s) + 2Fe(s). Is the reaction spontaneous at room temperature under standard conditions? During the reaction, the surroundings absorb 851.8 kJ/mol of heat. 25. Using the relevant S°298 values listed in Appendix G, calculate S°298 for the following changes:

(a) N2(g) + 3H2(g) ? 2NH3(g)
(b) N2(g) + 5/2O2(g) ? N2O5(g)

Verified Expert

In this assignment, ionic equation for dissolution and the solubility product (Ksp) expression was required to be calculated. Next was to calculate the molar solubility of the given compounds. Next were given some case based questions to determine the change in entropy and describing the redistribution of matter and/or energy that accompanies this process.

Reference no: EM131530174

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Reviews

inf1530174

7/29/2017 6:04:28 AM

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inf1530174

7/29/2017 6:03:39 AM

Fe(s) 0 0 27.3 Fe(g) 416.3 370.7 180.5 Fe2+(aq) –89.1 –78.90 –137.7 Fe3+(aq) –48.5 –4.7 –315.9 Fe2O3(s) –824.2 –742.2 87.40 Fe3O4(s) –1118.4 –1015.4 146.4 Fe(CO)5(l) –774.04 –705.42 338.07 Fe(CO)5(g) –733.87 –697.26 445.18 FeCl2(s) –341.79 –302.30 117.95 FeCl3(s) –399.49 –334.00 142.3 FeO(s) –272.0 –255.2 60.75 Fe(OH)2(s) –569.0 –486.5 88. Fe(OH)3(s) –823.0 –696.5 106.7 FeS(s) –100.0 –100.4 60.29 Fe3C(s) 25.10 20.08 104.60 lead Pb(s) 0 0 64.81 Pb(g) 195.2 162. 175.4 Pb2+(aq) –1.7 –24.43 10.5 PbO(s) (yellow) –217.32 –187.89 68.70 PbO(s) (red) –218.99 –188.93 66.5 Pb(OH)2(s) –515.9 — — PbS(s) –100.4 –98.7 91.2 Pb(NO3)2(s) –451.9 — — PbO2(s) –277.4 –217.3 68.6 PbCl2(s) –359.4 –314.1 136.0 lithium Li(s) 0 0 29.1 Li(g) 159.3 126.6 138.8 Li+(aq) –278.5 –293.3 13.4 LiH(s) –90.5 –68.3 20.0 Li(OH)(s) –487.5 –441.5 42.8 LiF(s) –616.0 –587.5 35.7 Li2CO3(s) –1216.04 –1132.19 90.17 magnesium Mg2+(aq) –466.9 –454.8 –138.1 manganese

inf1530174

7/29/2017 6:03:12 AM

fluorine F2(g) 0 0 202.8 F(g) 79.4 62.3 158.8 F–(aq) –332.6 –278.8 –13.8 F2O(g) 24.7 41.9 247.43 HF(g) –273.3 –275.4 173.8 hydrogen H2(g) 0 0 130.7 H(g) 217.97 203.26 114.7 H+(aq) 0 0 0 OH–(aq) –230.0 –157.2 –10.75 H3O+(aq) –285.8 69.91 H2O(l) –285.83 –237.1 70.0 H2O(g) –241.82 –228.59 188.8 H2O2(l) –187.78 –120.35 109.6 H2O2(g) –136.3 –105.6 232.7 HF(g) –273.3 –275.4 173.8 HCl(g) –92.307 –95.299 186.9 HBr(g) –36.3 –53.43 198.7 HI(g) 26.48 1.70 206.59 H2S(g) –20.6 –33.4 205.8 H2Se(g) 29.7 15.9 219.0 iodine I2(s) 0 0 116.14 I2(g) 62.438 19.3 260.7 I(g) 106.84 70.2 180.8 I–(aq) –55.19 –51.57 11.13 IF(g) 95.65 –118.49 236.06 ICl(g) 17.78 –5.44 247.44 IBr(g) 40.84 3.72 258.66 IF7(g) –943.91 –818.39 346.44 HI(g) 26.48 1.70 206.59 iron

inf1530174

7/29/2017 6:02:36 AM

Cl(g) 121.3 105.70 165.2 Cl–(aq) –167.2 –131.2 56.5 ClF(g) –54.48 –55.94 217.78 ClF3(g) –158.99 –118.83 281.50 Cl2O(g) 80.3 97.9 266.2 Cl2O7(l) 238.1 — — Cl2O7(g) 272.0 — — HCl(g) –92.307 –95.299 186.9 HClO4(l) –40.58 — — chromium Cr(s) 0 0 23.77 Cr(g) 396.6 351.8 174.50 CrO42–(aq) –881.2 –727.8 50.21 Cr2O72–(aq) –1490.3 –1301.1 261.9 Cr2O3(s) –1139.7 –1058.1 81.2 CrO3(s) –589.5 — — (NH4)2Cr2O7(s) –1806.7 — — cobalt Co(s) 0 0 30.0 Co2+(aq) –67.4 –51.5 –155 Co3+(aq) 92 134 –305.0 CoO(s) –237.9 –214.2 52.97 Co3O4(s) –910.02 –794.98 114.22 Co(NO3)2(s) –420.5 — — copper Cu(s) 0 0 33.15 Cu(g) 338.32 298.58 166.38 Cu+(aq) 51.9 50.2 –26 Cu2+(aq) 64.77 65.49 –99.6 CuO(s) –157.3 –129.7 42.63 Cu2O(s) –168.6 –146.0 93.14 CuS(s) –53.1 –53.6 66.5 Cu2S(s) –79.5 –86.2 120.9 CuSO4(s) –771.36 –662.2 109.2 Cu(NO3)2(s) –302.9 — —

inf1530174

7/29/2017 6:02:19 AM

CCl4(g) –95.7 –58.2 309.7 CHCl3(l) –134.1 –73.7 201.7 CHCl3(g) –103.14 –70.34 295.71 CS2(l) 89.70 65.27 151.34 CS2(g) 116.9 66.8 238.0 C2H2(g) 227.4 209.2 200.9 C2H4(g) 52.4 68.4 219.3 C2H6(g) –84.0 –32.0 229.2 CH3CO2H(l) –484.3 –389.9 159.8 CH3CO2H(g) –434.84 –376.69 282.50 C2H5OH(l) –277.6 –174.8 160.7 C2H5OH(g) –234.8 –167.9 281.6 HCO3–(aq) –691.11 –587.06 95 C3H8(g) –103.8 –23.4 270.3 C6H6(g) 82.927 129.66 269.2 C6H6(l) 49.1 124.50 173.4 CH2Cl2(l) –124.2 –63.2 177.8 CH2Cl2(g) –95.4 –65.90 270.2 CH3Cl(g) –81.9 –60.2 234.6 C2H5Cl(l) –136.52 –59.31 190.79 C2H5Cl(g) –112.17 –60.39 276.00 C2N2(g) 308.98 297.36 241.90 HCN(l) 108.9 125.0 112.8 HCN(g) 135.5 124.7 201.8 cesium Cs+(aq) –248 –282.0 133 chlorine Cl2(g) 0 0 223.1

inf1530174

7/29/2017 6:02:05 AM

Cd(s) 0 0 51.76 Cd(g) 112.01 77.41 167.75 Cd2+(aq) –75.90 –77.61 –73.2 CdO(s) –258.2 –228.4 54.8 CdCl2(s) –391.5 –343.9 115.3 CdSO4(s) –933.3 –822.7 123.0 CdS(s) –161.9 –156.5 64.9 calcium Ca(s) 0 0 41.6 Ca(g) 178.2 144.3 154.88 Ca2+(aq) –542.96 –553.04 –55.2 CaO(s) –634.9 –603.3 38.1 Ca(OH)2(s) –985.2 –897.5 83.4 CaSO4(s) –1434.5 –1322.0 106.5 CaSO4•2H2O(s) –2022.63 –1797.45 194.14 CaCO3(s) (calcite) –1220.0 –1081.4 110.0 CaSO3•H2O(s) –1752.68 –1555.19 184.10 carbon C(s) (graphite) 0 0 5.740 C(s) (diamond) 1.89 2.90 2.38 C(g) 716.681 671.2 158.1 CO(g) –110.52 –137.15 197.7 CO2(g) –393.51 –394.36 213.8 CO32–(aq) –677.1 –527.8 –56.9 CH4(g) –74.6 –50.5 186.3 CH3OH(l) –239.2 –166.6 126.8 CH3OH(g) –201.0 –162.3 239.9 CCl4(l) –128.2 –62.5 214.4

inf1530174

7/29/2017 6:01:48 AM

Bi(s) 0 0 56.74 Bi(g) 207.1 168.2 187.00 Bi2O3(s) –573.88 –493.7 151.5 BiCl3(s) –379.07 –315.06 176.98 Bi2S3(s) –143.1 –140.6 200.4 boron B(s) 0 0 5.86 B(g) 565.0 521.0 153.4 B2O3(s) –1273.5 –1194.3 53.97 B2H6(g) 36.4 87.6 232.1 H3BO3(s) –1094.33 –968.92 88.83 BF3(g) –1136.0 –1119.4 254.4 BCl3(g) –403.8 –388.7 290.1 B3N3H6(l) –540.99 –392.79 199.58 HBO2(s) –794.25 –723.41 37.66 bromine Br2(l) 0 0 152.23 Br2(g) 30.91 3.142 245.5 Br(g) 111.88 82.429 175.0 Br–(aq) –120.9 –102.82 80.71 BrF3(g) –255.60 –229.45 292.42 HBr(g) –36.3 –53.43 198.7 cadmium

inf1530174

7/29/2017 6:01:27 AM

arsenic As(s) 0 0 35.1 As(g) 302.5 261.0 174.21 As4(g) 143.9 92.4 314 As4O6(s) –1313.94 –1152.52 214.22 As2O5(s) –924.87 –782.41 105.44 AsCl3(g) –261.50 –248.95 327.06 As2S3(s) –169.03 –168.62 163.59 AsH3(g) 66.44 68.93 222.78 H3AsO4(s) –906.3 — — barium Ba(s) 0 0 62.5 Ba(g) 180 146 170.24 Ba2+(aq) –537.6 –560.8 9.6 BaO(s) –548.0 –520.3 72.1 BaCl2(s) –855.0 –806.7 123.7 BaSO4(s) –1473.2 –1362.3 132.2 beryllium Be(s) 0 0 9.50 Be(g) 324.3 286.6 136.27 BeO(s) –609.4 –580.1 13.8 bismuth

inf1530174

7/29/2017 6:01:10 AM

Appendix G: Standard Thermodynamic Properties for Selected Substances Standard Thermodynamic Properties for Selected Substances Substance (kJ mol–) (kJ mol–1) (J K–1mol–1) aluminum Al(s) 0 0 28.3 Al(g) 324.4 285.7 164.54 Al3+(aq) –531 –485 –321.7 Al2O3(s) –1676 –1582 50.92 lF3(s) –1510.4 –1425 66.5 AlCl3(s) –704.2 –628.8 110.67 AlCl3•6H2O(s) –2691.57 –2269.40 376.56 Al2S3(s) –724.0 –492.4 116.9 Al2(SO4)3(s) –3445.06 –3506.61 239.32 antimony Sb(s) 0 0 45.69 Sb(g) 262.34 222.17 180.16 Sb4O6(s) –1440.55 –1268.17 220.92 SbCl3(g) –313.8 –301.2 337.80 SbCl5(g) –394.34 –334.29 401.94 Sb2S3(s) –174.89 –173.64 182.00 SbCl3(s) –382.17 –323.72 184.10 SbOCl(s) –374.0 — —

inf1530174

7/24/2017 5:29:47 AM

The last question "Thermite” reactions have been used for welding metal parts such as railway rails and in metal refining. One such thermite reaction is Fe2O3(s) + 2Al(s) ? Al2O3(s) + 2Fe(s). Is the reaction spontaneous at room temperature under standard conditions? During the reaction, the surroundings absorb 851.8 kJ/mol of heat. 25. Using the relevant S°298 values listed in Appendix G, calculate S°298 for the following changes:" Requires Appendix G for solving this question. Sorry about the inconvenience, I have attached Appendix G. Thanks! 24045486_1Appendix G.docx

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