Table 3: Standard Gibbs free energy change when using methanogens for metabolism of intermediates.

Reaction equation (pH = 7, = 298.15 K) (kJ/mol)

4CH3CH2COO + 3H2O 4CH3COO + + H+ + 3CH4−102.0 < 0>0
2CH3CH2CH2COO + + H2O 4CH3COO + H+ + CH4−39.4 < 0>0
CH3COOH CO2 + CH4−31.0 < 0>0
4HCOOH 3CO2 + 2H2O + CH4−130.1 < 0>0
4H2 + + H+ 3H2O + CH4−135.6 < 0>0
2CH3CH2OH + CO2 2CH2COOH + CH4−116.3 < 0>0
CH3OH + H2 H2O + CH4−112.5 < 0>0
4CH3OH CO2 + 2H2O + 3CH4−104.9 < 0>0
4CH3NH2 + 2H2O CO2 + 4NH3 + 3CH4−75.0 < 0>0
2(CH3)2NH + 2H2O CO2 + 2NH3 + 3CH4−73.2 < 0>0
4(CH3)3N + 6H2O 3CO2 + 4NH3 + 9CH4−74.3 < 0>0
2(CH3)2S + 2H2O CO2 + 2H2S + 3CH4−73.8 < 0>0