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C06 Enthalpy Table for Beginners


                      Standard Heats of Formation, ∆Hformation

             Hess’s Law, ∆Hrx = Σ∆Hformation products - Σ∆Hformation reactants


                                                           Standard Enthalpy of
                                                             Formation Table
                                   Rx of Formation               ∆Hformation
                                                              Substance     kJ/mol
                                                   Al(s) → Al(s)               0
                                      Al(s) + 3/2 O2(g) → Al2O3(s)          -1670
                                          C(s, graphite) → C(s, graphite)      0
                                        C(s) + ½ O2(g) → CO (g)              -111
                                           C(s) + O2(g) → CO2 (g)            -394
                                          C(s) + 2H2(g) → CH4 (g)             -75
                              C(s) + 2H2(g) + 1/2 O2(g) → CH3OH (l)          -239
                                          2C(s) + H2(g) → C2H2 (g)           227
                                         2C(s) + 2H2 g) → C2H4 (g)            52
                                        2C(s) + 3H2(g) → C2H6 (g)             -85
                              2C(s) + 3H2(g) + ½ O2(g) → C2H5OH (l)          -278
                                       Ca(s) + ½ O2(g) → CaO (s)             -636
                                 Ca(s) + O2(g) + H2(g) → Ca(OH)2 (s)         -987
                                  Ca(s) + S(s)+ 2O2(g) → CaSO4(s)           -1433
                                                  Cl2(g) → Cl2 (g)             0
                                     2Fe(s) + 3/2 O2(g) → Fe2O3 (s)          -822
                                                  H2(g) → H2 (g)               0
                                     ½ H2(g) + ½ Cl2(g) → HCl(g)              -92
                                       H2(g) + ½ O2(g) → H2O (g)             -242
                                       H2(g) + ½ O2(g) → H2O (l)             -286
                                          H2(g) + O2(g) → H2O2 (l)           -188
                                        ½ H2(g) + S(s) → H2S (g)             -20.
                                  H2(g) + S(s)+ 2O2(g) → H2SO4 (l)           -811
                                                  Hg(l) → Hg (l)               0
                                                  Hg(l) → Hg (g)              61
                                       Mg(s) + ½O2(g) → MgO(s)               -602
                                                  N2 (g) → N2 (g)              0
                                     ½N2(g) + 3/2H2(g) → NH3 (g)              -46
                              ½N2(g) + 2H2(g) ½Cl2(g) → NH4Cl(s)             -315
                                        N2(g) + ½O2(g) → N2O (g)              82
                                        N2(g) + 2O2(g) → N2O4 (g)             10
                                       Na(s) + ½Cl2(g) → NaCl (s)            -411
                              Na(s) + ½O2(g) + ½H2(g) → NaOH (s)             -427
                                                  O2 (g) → O2 (g)              0
                                        4P(s) + 5O2 (g) → P4O10(s)          -2980
                                                    S(s) → S(s)                0
                                           S(s) + O2 (g) → SO2 (g)           -297
                                       S(s) + 3/2O2 (g) → SO3 (g)            -395

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Heat of formation by reactions

  • 1. C06 Enthalpy Table for Beginners Standard Heats of Formation, ∆Hformation Hess’s Law, ∆Hrx = Σ∆Hformation products - Σ∆Hformation reactants Standard Enthalpy of Formation Table Rx of Formation ∆Hformation Substance kJ/mol Al(s) → Al(s) 0 Al(s) + 3/2 O2(g) → Al2O3(s) -1670 C(s, graphite) → C(s, graphite) 0 C(s) + ½ O2(g) → CO (g) -111 C(s) + O2(g) → CO2 (g) -394 C(s) + 2H2(g) → CH4 (g) -75 C(s) + 2H2(g) + 1/2 O2(g) → CH3OH (l) -239 2C(s) + H2(g) → C2H2 (g) 227 2C(s) + 2H2 g) → C2H4 (g) 52 2C(s) + 3H2(g) → C2H6 (g) -85 2C(s) + 3H2(g) + ½ O2(g) → C2H5OH (l) -278 Ca(s) + ½ O2(g) → CaO (s) -636 Ca(s) + O2(g) + H2(g) → Ca(OH)2 (s) -987 Ca(s) + S(s)+ 2O2(g) → CaSO4(s) -1433 Cl2(g) → Cl2 (g) 0 2Fe(s) + 3/2 O2(g) → Fe2O3 (s) -822 H2(g) → H2 (g) 0 ½ H2(g) + ½ Cl2(g) → HCl(g) -92 H2(g) + ½ O2(g) → H2O (g) -242 H2(g) + ½ O2(g) → H2O (l) -286 H2(g) + O2(g) → H2O2 (l) -188 ½ H2(g) + S(s) → H2S (g) -20. H2(g) + S(s)+ 2O2(g) → H2SO4 (l) -811 Hg(l) → Hg (l) 0 Hg(l) → Hg (g) 61 Mg(s) + ½O2(g) → MgO(s) -602 N2 (g) → N2 (g) 0 ½N2(g) + 3/2H2(g) → NH3 (g) -46 ½N2(g) + 2H2(g) ½Cl2(g) → NH4Cl(s) -315 N2(g) + ½O2(g) → N2O (g) 82 N2(g) + 2O2(g) → N2O4 (g) 10 Na(s) + ½Cl2(g) → NaCl (s) -411 Na(s) + ½O2(g) + ½H2(g) → NaOH (s) -427 O2 (g) → O2 (g) 0 4P(s) + 5O2 (g) → P4O10(s) -2980 S(s) → S(s) 0 S(s) + O2 (g) → SO2 (g) -297 S(s) + 3/2O2 (g) → SO3 (g) -395