Question 16.2: Calculate ΔS° for ⓐ dissolving one mole of calcium hydroxide...
Calculate ΔS° for
ⓐ dissolving one mole of calcium hydroxide in water.
ⓑ the combustion of one gram of methane to form carbon dioxide and liquid water.
ⓐ
STRATEGY
1. Write a balanced equation for dissolving Ca(OH)_{2}.
2. Find ΔS° by substituting S° values found in Table 16.1 into Equation 16.1.
Table 16.1 Standard Entropies at 25°C (J/mol·K) of Elements and Compounds at 1 atm, Aqueous Ions at 1 M
Elements |
Ag(s) 42.6 Cl_{2}(g) 223.0 I_{2}(s) 116.1 O_{2}(g) 205.0 Al(s) 28.3 Cr(s) 23.8 K(s) 64.2 Pb(s) 64.8 Ba(s) 62.8 Cu(s) 33.2 Mg(s) 32.7 P_{4}(s) 164.4 Br_{2}(l) 152.2 F_{2}(g) 202.7 Mn(s) 32.0 S(s) 31.8 C(s) 5.7 Fe(s) 27.3 N_{2}(g) 191.5 Si(s) 18.8 Ca(s) 41.4 H_{2}(g) 130.6 Na(s) 51.2 Sn(s) 51.6 Cd(s) 51.8 Hg(l) 76.0 Ni(s) 29.9 Zn(s) 41.6 |
Compounds |
AgBr(s) 107.1 CaCl_{2}(s) 104.6 H_{2}O(g) 188.7 NH_{4}NO_{3}(s) 151.1 AgCl(s) 96.2 CaCO_{3}(s) 92.9 H_{2}O(l) 69.9 NO(g) 210.7 AgI(s) 115.5 CaO(s) 39.8 H_{2}O_{2}(l) 109.6 NO_{2}(g) 240.0 AgNO_{3}(s) 140.9 Ca(OH)_{2}(s) 83.4 H_{2}S(g) 205.7 N_{2}O_{4}(g) 304.2 Ag_{2}O(s) 121.3 CaSO_{4}(s) 106.7 H_{2}SO_{4}(l) 156.9 NaCl(s) 72.1 Al_{2}O_{3}(s) 50.9 CdCl_{2}(s) 115.3 HgO(s) 70.3 NaF(s) 51.5 BaCl_{2}(s) 123.7 CdO(s) 54.8 KBr(s) 95.9 NaOH(s) 64.5 BaCO_{3}(s) 112.1 Cr_{2}O_{3}(s) 81.2 KCl(s) 82.6 NiO(s) 38.0 BaO(s) 70.4 CuO(s) 42.6 KClO_{3}(s) 143.1 PbBr_{2}(s) 136.0 BaSO_{4}(s) 132.2 Cu_{2}O(s) 93.1 KClO_{4}(s) 151.0 PbCl_{2}(s) 136.0 CCl_{4}(l) 216.4 CuS(s) 66.5 KNO_{3}(s) 133.0 PbO(s) 66.5 CHCl_{3}(l) 201.7 Cu_{2}S(s) 120.9 MgCl_{2}(s) 89.6 PbO_{2}(s) 68.6 CH_{4}(g) 186.2 CuSO_{4}(s) 107.6 MgCO_{3}(s) 65.7 PCl_{3}(g) 311.7 C_{2}H_{2}(g) 200.8 Fe(OH)_{3}(s) 106.7 MgO(s) 26.9 PCl_{5}(g) 364.5 C_{2}H_{4}(g) 219.5 Fe_{2}O_{3}(s) 87.4 Mg(OH)_{2}(s) 63.2 SiO_{2}(s) 41.8 C_{2}H_{6}(g) 229.5 Fe_{3}O_{4}(s) 146.4 MgSO_{4}(s) 91.6 SnO_{2}(s) 52.3 C_{3}H_{8}(g) 269.9 HBr(g) 198.6 MnO(s) 59.7 SO_{2}(g) 248.1 CH_{3}OH(l) 126.8 HCl(g) 186.8 MnO_{2}(s) 53.0 SO_{3}(g) 256.7 C_{2}H_{5}OH(l) 160.7 HF(g) 173.7 NH_{3}(g) 192.3 ZnI_{2}(s) 161.1 CO(g) 197.6 HI(g) 206.5 N_{2}H_{4}(l) 121.2 ZnO(s) 43.6 CO_{2}(g) 213.6 HNO_{3}(l) 155.6 NH_{4}Cl(s) 94.6 ZnS(s) 57.7 |
Cations Anions |
Ag^{+}(aq) 72.7 Hg^{2+}(aq) -32.2 Br^{-}(aq) 82.4 HPO_{4}^{2-}(aq) -33.5 Al^{3+}(aq) -321.7 K^{+}(aq) 102.5 CO_{3}^{2-}(aq) -56.9 HSO_{4}^{-}(aq) 131.8 Ba^{2+}(aq) 9.6 Mg^{2+}(aq) -138.1 Cl^{-}(aq) 56.9 I^{-}(aq) 111.3 Ca^{2+}(aq) -53.1 Mn^{2+}(aq) -73.6 ClO_{3}^{-}(aq) 162.3 MnO_{4}^{-}(aq) 191.2 Cd^{2+}(aq) -73.2 Na^{+}(aq) 59.0 ClO_{4}^{-}(aq) 182.0 NO_{2}^{-}(aq) 123.0 Cu^{+}(aq) 40.6 NH_{4}^{+}(aq) 113.4 CrO_{4}^{2-}(aq) 50.2 NO_{3} ^{-}(aq) 146.4 Cu^{2+}(aq) -99.6 Ni^{2+}(aq) -128.9 Cr_{2}O_{7}^{2-}(aq) 261.9 OH^{-}(aq) -10.8 Fe^{2+}(aq) -137.7 Pb^{2+}(aq) 10.5 F^{-}(aq) -13.8 PO_{4}^{3-}(aq) -222 Fe^{3+}(aq) -315.9 Sn^{2+}(aq) -17.4 HCO_{3}^{-}(aq) 91.2 S^{2-}(aq) -14.6 H^{+}(aq) 0.0 Zn^{2+}(aq) -112.1 H_{2}PO_{4}^{-}(aq) 90.4 SO_{4}^{2-}(aq) 20.1 |
ΔS° = ΣS°_{products} – ΣS°_{reactants} (16.1)
ⓑ
STRATEGY
1. Write a balanced equation for the reaction.
2. Find ΔS° by substituting S° values from Table 16.1 into Equation 16.1.
Note that the value you obtained is for the difference in entropy for one mole.
3. Use ΔS° for one mole as a conversion factor to obtain ΔS° for one gram of CH_{4}.
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