APPENDIX 231 Appendix I d Definitions of the SI Base Units he Metre (m): The metre is the length of path travelled by light in vacuum during a time interval of 1/299 792 458 of a second (17th CGPM, 1983) Kilogram (kg): The kilogram is the unit of mass; it is equal to the mass of the international prototype of the kilogram (3rd CGPM, 1901) is Second (s): The second is the duration of 9192631770 periods of the radiation corresponding to the transition between the two hyperfine levels of the ground state of the caesium-133 atom (13th CGPM, 1967) © no N C tt E o R be T re pu bl Ampere (A): The ampere is that constant current which, if maintained in two straight parallel conductors of infinite length, of negligible circular cross-section, and placed metre apart in vacuum, would produce between these conductors a force equal to 10-7 Newton per metre of length (9th CGPM, 1948) Kelvin (K): The kelvin, unit of thermodynamic temperature, is the fraction 1/273.16 of the thermodynamic temperature of the triple point of water (13th CGPM, 1967) Mole (mol): The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon-12 When the mole is used, the elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specified groups of such particles (14th CGPM, 1971) Candela (cd): The candela is the luminous intensity, in a given direction, of a source that emits monochromatic radiation of frequency 540 1012 hertz and that has a radiant intensity in that direction of (1/683) watt per steradian (16th CGPM, 1979) (The symbols listed here are internationally agreed and should not be changed in other languages or scripts) 232 CHEMISTRY Appendix II Elements, their Atomic Number and Molar Mass Symbol Ac Al Am Sb Ar As At Ba Bk Be Bi Bh B Br Cd Cs Ca Cf C Ce Cl Cr Co Cu Cm Db Dy Es Er Eu Fm F Fr Gd Ga Ge Au Hf Hs He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Mt Md 89 13 95 51 18 33 85 56 97 83 107 35 48 55 20 98 58 17 24 27 29 96 105 66 99 68 63 100 87 64 31 32 79 72 108 67 49 53 77 26 36 57 103 82 71 12 25 109 101 227.03 26.98 (243) 121.75 39.95 74.92 210 137.34 (247) 9.01 208.98 (264) 10.81 79.91 112.40 132.91 40.08 251.08 12.01 140.12 35.45 52.00 58.93 63.54 247.07 (263) 162.50 (252) 167.26 151.96 (257.10) 19.00 (223) 157.25 69.72 72.61 196.97 178.49 (269) 4.00 164.93 1.0079 114.82 126.90 192.2 55.85 83.80 138.91 (262.1) 207.19 6.94 174.96 24.31 54.94 (268) 258.10 Mercury Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praseodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Rutherfordium Samarium Scandium Seaborgium Selenium Silicon Silver Sodium Strontium Sulphur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten Ununbium Ununnilium Unununium Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Sc Sg Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W Uub Uun Uuu U V Xe Yb Y Zn Zr Atomic Number Molar mass/ (g mol–1) d Element he Molar mass/ (g mol–1) 80 42 60 10 93 28 41 102 76 46 15 78 94 84 19 59 61 91 88 86 75 45 37 44 104 62 21 106 34 14 47 11 38 16 73 43 52 65 81 90 69 50 22 74 112 110 111 92 23 54 70 39 30 40 200.59 95.94 144.24 20.18 (237.05) 58.71 92.91 14.0067 (259) 190.2 16.00 106.4 30.97 195.09 (244) 210 39.10 140.91 (145) 231.04 (226) (222) 186.2 102.91 85.47 101.07 (261) 150.35 44.96 (266) 78.96 28.08 107.87 22.99 87.62 32.06 180.95 (98.91) 127.60 158.92 204.37 232.04 168.93 118.69 47.88 183.85 (277) (269) (272) 238.03 50.94 131.30 173.04 88.91 65.37 91.22 is Atomic Number © no N C tt E o R be T re pu Actinium Aluminium Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Bohrium Boron Bromine Cadmium Caesium Calcium Californium Carbon Cerium Chlorine Chromium Cobalt Copper Curium Dubnium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Hassium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Meitneium Mendelevium Symbol bl Element The value given in parenthesis is the molar mass of the isotope of largest known half-life APPENDIX 233 Appendix III A Specific and Molar Heat Capacities for Some Substances at 298 K and one Atmospheric Pressure Molar Heat Capacity (J/mol) 0.720 4.184 2.06 0.797 0.360 4.70 2.46 2.42 2.06 0.861 0.5980 0.817 1.03 0.477 0.473 0.460 0.385 0.902 0.128 0.720 20.8 75.4 35.1 29.1 29.1 79.9 113.16 152.52 37.08 132.59 72.35 39.2 20.7 33.8 75.6 25.1 24.7 24.35 25.2 8.65 he is © no N C tt E o R be T re pu air water (liquid) ammonia (gas) hydrogen chloride hydrogen bromide ammonia (liquid) ethyl alcohol (liquid) ethylene glycol (liquid) water (solid) carbon tetrachloride (liquid) chlorofluorocarbon (CCl F ) 2 ozone neon chlorine bromine iron copper aluminium gold graphite B d Specific Heat Capacity (J/g) bl Substance Molar Heat Capacities for Some Gases (J/mol) Gas Monatomic* helium argon iodine mercury Diatomic† hydrogen oxygen nitrogen hydrogen chloride carbon monoxide Triatomic† nitrous oxide carbon dioxide Polyatomic† ethane Cp Cv Cp - C v Cp / Cv 20.9 20.8 20.9 20.8 12.8 12.5 12.6 12.5 8.28 8.33 8.37 8.33 1.63 1.66 1.66 1.66 28.6 29.1 29.0 29.6 29.0 20.2 20.8 20.7 21.0 21.0 8.33 8.33 8.30 8.60 8.00 1.41 1.39 1.40 1.39 1.41 39.0 37.5 30.5 29.0 8.50 8.50 1.28 1.29 53.2 44.6 8.60 1.19 *Translational kinetic energy only †Translational, vibrational and rotational energy 234 CHEMISTRY Appendix IV Symbol Traditional Units ao Bohr radius k e/m e 9.806 m/s 1.6606 × 10-27 kg 6.022 ×1023 particles/mol 0.52918 C 5.2918 × 10-9 cm 1.3807 × 10-16 erg/K 1.7588 ×l08 coulomb/g 6.022 × 1023 particles/mol 5.2918 × 10-11 m 1.60219 × 10-19 coulomb 4.8033 × 10-19 esu 9.10952 ×10-28 g 0.00054859 u 96,487 coulombs/eq 23.06 kcal/volt eq 1.60219 × 10-19 C 1.3807 × 10-23 J/K 1.7588 × 1011 C/kg © no N C tt E o R be T re pu Boltzmann constant Charge-to-mass ratio of electron Electronic charge 980.6 cm/s 1.6606 × 10-24 g he g amu or u NA is Acceleration of gravity Atomic mass unit (1/12 the mass of 12C atom) Avogadro constant SI Units bl Quantity Electron rest mass me Faraday constant F Gas constant R mol K cal mol K Molar volume (STP) Vm 22.710981 L/mol Neutron rest mass mn Planck constant Proton rest mass h mp Rydberg constant R∞ 1.67495 × 10-24 g 1.008665 u 6.6262 × 10-27 ergs 1.6726 ×10-24 g 1.007277 u 3.289 × 1015 cycles/s 2.1799 × 10-11 erg 2.9979 ×1010 cm/s (186,281 miles/second) c 9.10952 ×10-31 kg 96,487 C/mol e96,487 J/V.mol e- kPa dm L atm 0.8206 1.987 Speed of light (in a vacuum) 8.3145 mol K 8.3145 J/mol.K 22.710981 × 10-3 m3/mol 22.710981 dm3/mol 1.67495 × 10-27 kg 6.6262 × 10-34 J s 1.6726 ×10-27 kg 1.0974 × 107 m-1 2.1799 × 10-18 J 2.9979 × 108 m/s π = 3.1416 2.303 R = 4.576 cal/mol K = 19.15 J/mol K e = 2.71828 2.303 RT (at 25°C) = 1364 cal/mol = 5709 J/mol ln X = 2.303 log X d Physical Constants APPENDIX 235 Appendix V Some Useful Conversion Factors Common Units of Length inch = 2.54 centimetres (exactly) pound = 453.59 grams = 0.45359 kilogram kilogram = 1000 grams = 2.205 pounds gram = 10 decigrams = 100 centigrams = 1000 milligrams gram = 6.022 × 1023 atomic mass units or u atomic mass unit = 1.6606 × 10–24 gram metric tonne = 1000 kilograms = 2205 pounds mile = 5280 feet = 1.609 kilometres yard = 36 inches = 0.9144 metre metre = 100 centimetres = 39.37 inches = 3.281 feet = 1.094 yards kilometre = 1000 metres = 1094 yards = 0.6215 mile Angstrom = 1.0 × 10–8 centimetre = 0.10 nanometre = 1.0 × 10–10 metre = 3.937 × 10–9 inch he is Common Units of Force* and Pressure atmosphere = 760 millimetres of mercury = 1.013 × 105 pascals = 14.70 pounds per square inch bar = 105 pascals torr = millimetre of mercury pascal = kg/ms2 = N/m2 © no N C tt E o R be T re pu litre = cubic decimetre = 1000 cubic centimetres = 0.001 cubic metre millilitre = cubic centimetre = 0.001 litre = 1.056 × 10-3 quart cubic foot = 28.316 litres = 29.902 quarts = 7.475 gallons bl Common Unit of Volume quart = 0.9463 litre litre = 1.056 quarts Common Units of Energy joule = × 107 ergs thermochemical calorie** = 4.184 joules = 4.184 × 107 ergs = 4.129 × 10–2 litre-atmospheres = 2.612 × 1019 electron volts ergs = × 10–7 joule = 2.3901 × 10–8 calorie electron volt = 1.6022 × 10–19 joule = 1.6022 × 10–12 erg = 96.487 kJ/mol† litre-atmosphere = 24.217 calories = 101.32 joules = 1.0132 ×109 ergs British thermal unit = 1055.06 joules = 1.05506 ×1010 ergs = 252.2 calories d Common Unit of Mass and Weight pound = 453.59 grams Temperature SI Base Unit: Kelvin (K) K = -273.15°C K = °C + 273.15 °F = 1.8(°C) + 32 °C = °F − 32 1.8 * Force: newton (N) = kg m/s2, i.e.,the force that, when applied for second, gives a 1-kilogram mass a velocity of metre per second ** The amount of heat required to raise the temperature of one gram of water from 14.50C to 15.50C † Note that the other units are per particle and must be multiplied by 6.022 ×1023 to be strictly comparable 236 CHEMISTRY Appendix VI Thermodynamic Data at 298 K INORGANIC SUBSTANCES Enthalpy of formation, ΔfHJ / (kJ mol–1) Gibbs Energy of formation, ΔfGJ / (kJ mol–1) – 524.7 –1675.7 –1276 –704.2 –481.2 –1582.3 — –628.8 Antimony 147.75 –301.2 –334.29 232.78 337.80 401.94 bl 145.11 –313.8 –394.34 © no N C tt E o R be T re pu SbH3(g) SbCl3(g) SbCl5(g) 28.33 –321.7 50.92 — 110.67 is Al(s) Al3+(aq) Al2O3(s) Al(OH)3(s) AlCl3(s) he Aluminium Entropy,* SJ /(J K–1 mol–1) d Substance Arsenic As(s), gray As2S3(s) AsO43–(aq) –169.0 –888.14 –168.6 –648.41 35.1 163.6 –162.8 –537.64 –553.5 –1216.3 –1214.78 –560.77 –525.1 –1137.6 –1088.59 62.8 9.6 70.42 112.1 –47.3 –1272.8 –1137.0 –1193.7 –1120.3 5.86 53.97 254.12 Barium Ba(s) Ba2+(aq) BaO(s) BaCO3(s) BaCO3(aq) Boron B(s) B2O3(s) BF3(g) Bromine Br2(l) Br2(g) Br(g) Br–(aq) HBr(g) BrF3(g) 30.91 111.88 –121.55 –36.40 –255.60 3.11 82.40 –103.96 –53.45 –229.43 152.23 245.46 175.02 82.4 198.70 292.53 178.2 –542.83 144.3 –553.58 41.42 154.88 –53.1 Calcium Ca(s) Ca(g) Ca2+(aq) (continued) APPENDIX Substance 237 Enthalpy of formation, ΔfHJ / (kJ mol–1) Gibbs Energy of formation, ΔfGJ / (kJ mol–1) Entropy,* SJ /(J K–1 mol–1) Calcium (continued) Carbon** 1.895 716.68 –110.53 –393.51 –677.14 –135.44 89.70 135.1 108.87 d 39.75 83.39 –74.5 92.9 88.7 –110.0 68.87 –80.8 104.6 59.8 130 69.96 56.5 106.7 –33.1 he 2.900 671.26 –137.17 –394.36 –527.81 –65.21 65.27 124.7 124.97 © no N C tt E o R be T re pu C(s), graphite C(s), diamond C(g) CO(g) CO2(g) CO32–(aq) CCl4(l) CS2(l) HCN(g) HCN(l) –604.03 –898.49 –868.07 –1128.8 –1127.8 –1081.39 –1167.3 –1111.15 –748.1 –816.0 –663.6 –64.9 –477.4 –1321.79 –1298.10 is –635.09 –986.09 –1002.82 –1206.92 –1207.1 –1219.97 –1219.6 –1208.09 –795.8 –877.1 –682.8 –59.8 –482.4 –1434.11 –1452.10 bl CaO(s) Ca(OH)2(s) Ca(OH)2(aq) CaCO3(s), calcite CaCO3(s), aragonite CaCO3(aq) CaF2(s) CaF2(aq) CaCl2(s) CaCl2(aq) CaBr2(s) CaC2(s) CaS(s) CaSO4(s) CaSO4(aq) 5.740 2.377 158.10 197.67 213.74 –56.9 216.40 151.34 201.78 112.84 Cerium Ce(s) Ce3+(aq) Ce4+(aq) –696.2 –537.2 –672.0 –503.8 72.0 –205 –301 121.68 –167.16 –92.31 –167.16 105.68 –131.23 –95.30 –131.23 223.07 165.20 56.5 186.91 56.5 71.67 64.77 –168.6 –157.3 –771.36 –2279.7 49.98 65.49 –146.0 –129.7 –661.8 –1879.7 33.15 40.6 –99.6 93.14 42.63 109 300.4 Chlorine Cl2(g) Cl(g) Cl–(aq) HCl(g) HCl(aq) Copper Cu(s) Cu+(aq) Cu2+(aq) Cu2O(aq) CuO(s) CuSO4(s) CuSO4.5H2O(s) ** For organic compounds, a separate table is provided in continuation (continued) 238 Substance CHEMISTRY Enthalpy of formation, ΔfHJ / (kJ mol–1) Gibbs Energy of formation, ΔfGJ / (kJ mol–1) Entropy,* SJ /(J K–1 mol–1) –249.20 –294.60 –234.54 –243.44 144.96 198.34 75.94 Fluorine F2(g) F–(aq) HF(g) HF(aq) –332.63 –271.1 –332.63 –278.79 –273.2 –278.79 202.78 –13.8 173.78 –13.8 Hydrogen (see also Deuterium) H2(g) H(g) 217.97 H+(aq) H 2O(l) –285.83 H2O(g) –241.82 –187.78 H 2O 2(l) H2O2(aq) –191.17 203.25 –237.13 –228.57 –120.35 –134.03 he d Deuterium D2(g) D2O(g) D 2O(l) is bl © no N C tt E o R be T re pu Iodine I2(s) I2(g) I–(aq) HI(g) Iron Fe(s) Fe2+(aq) Fe3+(aq) Fe3O4(s), magnetite Fe2O3(s), haematite FeS(s,α) FeS(aq) FeS2(s) 62.44 –55.19 26.48 130.68 114.71 69.91 188.83 109.6 143.9 19.33 –51.57 1.70 116.14 260.69 111.3 206.59 –78.90 –4.7 –1015.4 –742.2 –100.4 6.9 –166.9 27.28 –137.7 –315.9 146.4 87.40 60.29 — 52.93 –1.7 –277.4 –919.94 –278.7 –244.8 –24.43 –217.33 –813.14 –261.92 –232.34 64.81 10.5 68.6 148.57 161.5 175.3 147.70 –466.85 –601.70 –1095.8 –524.3 113.10 –454.8 –569.43 –1012.1 –503.8 32.68 148.65 –138.1 26.94 65.7 117.2 –89.1 –48.5 –1118.4 –824.2 –100.0 — –178.2 Lead Pb(s) Pb2+(aq) PbO2(s) PbSO4(s) PbBr2(s) PbBr2(aq) Magnesium Mg(s) Mg(g) Mg2+(aq) MgO(s) MgCO3(s) MgBr2(s) (continued) APPENDIX Substance 239 Enthalpy of formation, ΔfHJ / (kJ mol–1) Gibbs Energy of formation, ΔfGJ / (kJ mol–1) Entropy,* SJ /(J K–1 mol–1) Mercury 61.32 –90.83 –265.22 31.82 –58.54 –210.75 76.02 174.96 70.29 192.5 90.25 82.05 33.18 9.16 –174.10 –207.36 –205.0 –46.11 –80.29 –132.51 –114.2 294.1 50.63 –365.56 –314.43 –295.31 86.55 104.20 51.31 97.89 –80.71 –111.25 –108.74 –16.45 –26.50 –79.31 — 328.1 149.34 –183.87 –202.87 –88.75 191.61 210.76 219.85 240.06 304.29 155.60 146.4 146.4 192.45 111.3 113.4 — 238.97 121.21 151.08 94.6 186.2 d Hg(1) Hg(g) HgO(s) Hg2Cl2(s) is bl © no N C tt E o R be T re pu N2(g) NO(g) N2O(g) NO2(g) N2O4(g) HNO3(1) HNO3(aq) NO3– (aq) NH3(g) NH3(aq) NH+4 (aq) NH2OH(s) HN3(g) N2H4(1) NH4NO3(s) NH4Cl(s) NH4ClO4(s) he Nitrogen Oxygen O2(g) O3(g) OH–(aq) 142.7 –229.99 163.2 –157.24 205.14 238.93 –10.75 58.91 5.4 –2984.0 –964.8 –1266.9 –1277.4 –319.7 –287.0 –374.9 24.44 13.4 –2697.0 — — –1018.7 –272.3 –267.8 –305.0 41.09 279.98 210.23 228.86 — — — 217.18 311.78 364.6 89.24 –252.38 –424.76 –482.37 –567.27 60.59 –283.27 –379.08 –440.50 –537.75 64.18 160.34 102.5 78.9 91.6 66.57 Phosphorus P(s), white P4(g) PH3(g) P4O10(s) H3PO3(aq) H3PO4(1) H3PO4(aq) PCl3(1) PCl3(g) PCl5(g) Potassium K(s) K(g) K+(aq) KOH(s) KOH(aq) KF(s) (continued) 240 Substance CHEMISTRY Enthalpy of formation, ΔfHJ / (kJ mol–1) Gibbs Energy of formation, ΔfGJ / (kJ mol–1) Entropy,* SJ /(J K–1 mol–1) Potassium (continued) –409.14 –380.66 –324.89 –296.25 –303.09 –364.0 –480.7 Si(s) SiO2(s,α) –910.94 –856.64 Silver Ag(s) Ag+(aq) Ag2O(s) AgBr(s) AgBr(aq) AgCl(s) AgCl(aq) AgI(s) AgI(aq) AgNO3(s) 105.58 –31.05 –100.37 –15.98 –127.07 –61.58 –61.84 50.38 –124.39 77.11 –11.20 –96.90 –26.86 –109.79 –54.12 –66.19 25.52 –33.41 82.59 95.90 106.32 143.1 151.0 105 190.4 d –436.75 –393.80 –327.90 –397.73 –432.75 –380.7 –471.5 he KCl(s) KBr(s) KI(s) KClO3(s) KClO4(s) K2S(s) K2S(aq) Silicon is 18.83 41.84 bl © no N C tt E o R be T re pu Sodium Na(s) Na(g) Na+(aq) NaOH(s) NaOH(aq) NaCl(s) NaCl(aq) NaBr(s) NaI(s) NaHCO3(s) Na2CO3(s) 42.55 72.68 121.3 107.1 155.2 96.2 129.3 115.5 184.1 140.92 107.32 –240.12 –425.61 –470.11 –411.15 –407.3 –361.06 –287.78 –947.7 –1130.9 76.76 –261.91 –379.49 –419.15 –384.14 –393.1 –348.98 –286.06 –851.9 –1047.7 51.21 153.71 59.0 64.46 48.1 72.13 115.5 86.82 98.53 102.1 136.0 0.33 33.1 –296.83 –395.72 –813.99 –909.27 –909.27 –20.63 –39.7 –1209 0.1 85.8 –300.19 –371.06 –690.00 –744.53 –744.53 –33.56 –27.83 –1105.3 31.80 32.6 –14.6 248.22 256.76 156.90 20.1 20.1 205.79 121 291.82 Sulphur S(s), rhombic S(s), monoclinic S2–(aq) SO2(g) SO3(g) H 2SO 4(l) H2SO4(aq) SO42–(aq) H2S(g) H2S(aq) SF6(g) (continued) APPENDIX Substance 241 Enthalpy of formation, ΔfHJ / (kJ mol–1) Gibbs Energy of formation, ΔfGJ / (kJ mol–1) Entropy,* SJ /(J K–1 mol–1) Tin –2.09 –285.8 –580.7 0.13 –256.9 –519.6 51.55 44.14 56.5 52.3 –153.89 –348.28 +130.73 –147.06 –318.30 +95.14 41.63 –112.1 43.64 160.93 d Sn(s), white Sn(s), gray SnO(s) SnO2(s) Zn(s) Zn2+(aq) ZnO(s) Zn(g) he Zinc bl is *The entropies of individual ions in solution are determined by setting the entropy of H+ in water equal to and then defining the entropies of all other ions relative to this value; hence a negative entropy is one that is lower than the entropy of H+ in water © no N C tt E o R be T re pu ORGANIC COMPOUNDS Substance Enthalpy of Enthalpy of Gibbs Energy of combustion, formation, formation, Entropy, ΔcHJ / (kJ mol–1) ΔfHJ / (kJ mol–1) ΔfGJ / (kJ mol–1) SJ /(J K–1 mol–1) Hydrocarbons CH4(g), methane C2H2(g), ethyne (acetylene) C2H4(g), ethene(ethylene) C2H6(g), ethane C3H6(g), propene (propylene) C3H6(g), cyclopropane C3H8(g), propane C4H10(g), butane C5H12(g), pentane C6H6(l), benzene C6H6(g) C7H8(l), toluene C7H8(g) C6H12(l), cyclohexane C6H12(g), C8H18(l), octane –890 –1300 –1411 –1560 –2058 –2091 –2220 –2878 –3537 –3268 –3302 –3910 –3953 –3920 –3953 –5471 –74.81 226.73 52.26 –84.68 20.42 53.30 –103.85 –126.15 –146.44 49.0 — 12.0 — –156.4 — –249.9 –50.72 209.20 68.15 –32.82 62.78 104.45 –23.49 –17.03 –8.20 124.3 — 113.8 — 26.7 — 6.4 186.26 200.94 219.56 229.60 266.6 237.4 270.2 310.1 349 173.3 — 221.0 — 204.4 — 358 –726 –764 –1368 –1409 –3054 –238.86 –200.66 –277.69 –235.10 –164.6 –166.27 –161.96 –174.78 –168.49 –50.42 126.8 239.81 160.7 282.70 144.0 Alcohols and phenols CH3OH(l), methanol CH3OH(g) C2H5OH(l), ethanol C2H5OH(g) C6H5OH(s), phenol (continued) 242 Substance CHEMISTRY Enthalpy of Enthalpy of Gibbs Energy of combustion, formation, formation, Entropy, ΔcHJ / (kJ mol–1) ΔfHJ / (kJ mol–1) ΔfGJ / (kJ mol–1) SJ /(J K–1 mol–1) Carboxylic acid –424.72 –484.5 –485.76 –827.2 –385.1 –361.35 –389.9 –396.64 –697.9 –245.3 –571 –108.57 –102.53 –1166 –192.30 –128.12 –1192 –1790 –166.19 –248.1 –128.86 –155.4 Sugars –2808 — –2810 –5645 –1268 — –1266 –2222 –910 –917 — –1545 © no N C tt E o R be T re pu C6H12O6(s), glucose C6H12O6(aq) C6H12O6(s), fructose C12H22O11(s), sucrose 218.77 160.2 250.3 200 bl HCHO(g), methanal (formaldehyde) CH3CHO(l), ethanal (acetaldehyde) CH3CHO(g) CH3COCH3(l), propanone (acetone) is Aldehydes and ketones 128.95 159.8 86.6 120 167.6 d –255 –875 — –254 –3227 he HCOOH(l), formic acid CH3COOH(l), acetic acid CH3COOH (aq) (COOH)2(s), oxalic acid C6H5COOH(s), benzoic acid 212 — — 360 Nitrogen compounds CO(NH2)2(s), urea C6H5NH2(l), aniline –632 –333.51 –197.33 104.60 –3393 31.6 149.1 191.3 NH2CH2COOH(s), glycine –969 –532.9 –373.4 103.51 CH3NH2(g), methylamine –1085 –22.97 32.16 243.41 APPENDIX 243 Appendix VII Standard potentials at 298 K in electrochemical order Reduction half-reaction E J /V Reduction half-reaction H4XeO6 + 2H+ + 2e– ⎯→ XeO3 + 3H2O F2 + 2e– ⎯→ 2F– O3 + 2H+ + 2e– ⎯→ O2 + H2O 2– 2– S2O8 + 2e– ⎯→ 2SO4 + – + Ag + e ⎯→ Ag Co3+ + e– ⎯→ Co2+ H2O2 + 2H+ + 2e– ⎯→ 2H2O Au+ + e– ⎯→ Au Pb4+ + 2e– ⎯→ Pb2+ 2HClO + 2H+ + 2e– ⎯→ Cl2 + 2H2O Ce4+ + e– ⎯→ Ce3+ 2HBrO + 2H+ + 2e– ⎯→ Br2 + 2H2O – MnO4 + 8H+ + 5e– ⎯→ Mn2+ + 4H2O Mn3+ + e– ⎯→ Mn2+ Au3+ + 3e– ⎯→ Au Cl2 + 2e– ⎯→ 2Cl– 2– Cr2O + 14H+ + 6e– ⎯→ 2Cr3+ + 7H2O O3 + H2O + 2e– ⎯→ O2 + 2OH– O2 + 4H+ + 4e– ⎯→ 2H2O ClO–4 + 2H+ +2e– ⎯→ ClO–3 + 2H2O MnO2 + 4H+ + 2e– ⎯→ Mn2+ + 2H2O Pt2+ + 2e– ⎯→ Pt Br2 + 2e– ⎯→ 2Br– Pu4+ + e– ⎯→ Pu3+ NO–3 + 4H+ + 3e– ⎯→ NO + 2H2O 2Hg2+ + 2e– ⎯→ Hg 2+ ClO– + H2O + 2e– ⎯→ Cl– + 2OH– Hg2+ + 2e– ⎯→ Hg NO–3 + 2H+ + e– ⎯→ NO2 + H2O Ag+ + e– ⎯→ Ag – Hg 2+ +2e ⎯→ 2Hg 3+ – Fe + e ⎯→ Fe2+ BrO– + H2O + 2e– ⎯→ Br– + 2OH– Hg2SO4 +2e– ⎯→ 2Hg + SO42– MnO42– + 2H2O + 2e– ⎯→ MnO2 + 4OH– MnO–4 + e– ⎯→ MnO42– I2 + 2e– ⎯→ 2I– – I3 + 2e– ⎯→ 3I– +3.0 +2.87 +2.07 +2.05 +1.98 +1.81 +1.78 +1.69 +1.67 +1.63 +1.61 +1.60 +1.51 +1.51 +1.40 +1.36 +1.33 +1.24 +1.23 +1.23 +1.23 +1.20 +1.09 +0.97 +0.96 +0.92 +0.89 +0.86 +0.80 +0.80 +0.79 +0.77 +0.76 +0.62 +0.60 +0.56 +0.54 +0.53 Cu+ + e– ⎯→ Cu NiOOH + H2O + e– ⎯→ Ni(OH)2 + OH– Ag2CrO4 + 2e– ⎯→ 2Ag + CrO42– O2 + 2H2O + 4e– ⎯→ 4OH– ClO–4 + H2O + 2e– ⎯→ ClO–3 + 2OH– [Fe(CN)6]3– + e– ⎯→ [Fe(CN)6]4– Cu2+ + 2e– ⎯→ Cu Hg2Cl2 + 2e– ⎯→ 2Hg + 2Cl– AgCl + e– ⎯→ Ag + Cl– Bi3+ + 3e– ⎯→ Bi – SO42 + 4H+ + 2e– ⎯→ H2SO3 + H2O 2+ Cu + e– ⎯→ Cu+ Sn4+ + 2e– ⎯→ Sn2+ AgBr + e– ⎯→ Ag + Br– Ti4+ + e– ⎯→ Ti3+ 2H+ + 2e– ⎯→ H2 d E J /V © no N C tt E o R be T re pu bl is he +0.52 +0.49 +0.45 +0.40 +0.36 +0.36 +0.34 +0.27 +0.27 +0.20 +0.17 +0.16 +0.15 +0.07 0.00 0.0 by definition –0.04 –0.08 –0.13 –0.14 –0.14 –0.15 –0.23 –0.26 –0.28 –0.34 –0.34 –0.36 –0.37 –0.40 –0.40 –0.41 –0.44 –0.44 –0.48 –0.49 –0.61 –0.74 –0.76 Fe3+ + 3e– ⎯→ Fe O2 + H2O + 2e– ⎯→ HO–2 + OH– Pb2+ + 2e– ⎯→ Pb In+ + e– ⎯→ In Sn2+ + 2e– ⎯→ Sn AgI + e– ⎯→ Ag + I– Ni2+ + 2e– ⎯→ Ni V3+ + e– ⎯→ V2+ Co2+ + 2e– ⎯→ Co In3+ + 3e– ⎯→ In Tl+ + e– ⎯→ Tl PbSO4 + 2e– ⎯→ Pb + SO2– Ti3+ + e– ⎯→ Ti2+ Cd2+ + 2e– ⎯→ Cd In2+ + e– ⎯→ In+ Cr3+ + e– ⎯→ Cr2+ Fe2+ + 2e– ⎯→ Fe In3+ + 2e– ⎯→ In+ S + 2e– ⎯→ S2– In3+ + e– ⎯→ In2+ U4+ + e– ⎯→ U3+ Cr3+ + 3e– ⎯→ Cr Zn2+ + 2e– ⎯→ Zn (continued) 244 CHEMISTRY Appendix continued EJ /V Reduction half-reaction EJ /V Cd(OH)2 + 2e– ⎯→ Cd + 2OH– 2H2O + 2e– ⎯→ H2 + 2OH– Cr2+ + 2e– ⎯→ Cr Mn2+ + 2e– ⎯→ Mn V2+ + 2e– ⎯→ V Ti2+ + 2e– ⎯→ Ti Al3+ + 3e– ⎯→ Al U3+ + 3e– ⎯→ U Sc3+ + 3e– ⎯→ Sc Mg2+ + 2e– ⎯→ Mg Ce3+ + 3e– ⎯→ Ce –0.81 –0.83 –0.91 –1.18 –1.19 –1.63 –1.66 –1.79 –2.09 –2.36 –2.48 La3+ + 3e– ⎯→ La Na+ + e– ⎯→ Na Ca2+ + 2e– ⎯→ Ca Sr2+ + 2e– ⎯→ Sr Ba2+ + 2e– ⎯→ Ba Ra2+ + 2e– ⎯→ Ra Cs+ + e– ⎯→ Cs Rb+ + e– ⎯→ Rb K+ +e– ⎯→ K Li+ + e– ⎯→ Li –2.52 –2.71 –2.87 –2.89 –2.91 –2.92 –2.92 –2.93 –2.93 –3.05 © no N C tt E o R be T re pu bl is he d Reduction half-reaction ... 10 4.20 51. 31 97.89 –80. 71 ? ?11 1.25 ? ?10 8.74 ? ?16 .45 –26.50 –79. 31 — 328 .1 149.34 ? ?18 3.87 –202.87 –88.75 19 1. 61 210 .76 219 .85 240.06 304.29 15 5.60 14 6.4 14 6.4 19 2.45 11 1.3 11 3.4 — 238.97 12 1. 21 1 51. 08... 72.68 12 1.3 10 7 .1 155.2 96.2 12 9.3 11 5.5 18 4 .1 140.92 10 7.32 –240 .12 –425. 61 –470 .11 – 411 .15 –407.3 –3 61. 06 –287.78 –947.7 ? ?11 30.9 76.76 –2 61. 91 –379.49 – 419 .15 –384 .14 –393 .1 –348.98 –286.06 –8 51. 9... –868.07 ? ?11 28.8 ? ?11 27.8 ? ?10 81. 39 ? ?11 67.3 ? ?11 11. 15 –748 .1 – 816 .0 –663.6 –64.9 –477.4 ? ?13 21. 79 ? ?12 98 .10 is –635.09 –986.09 ? ?10 02.82 ? ?12 06.92 ? ?12 07 .1 ? ?12 19.97 ? ?12 19.6 ? ?12 08.09 –795.8 –877 .1 –682.8 –59.8