Delta G is the symbol of atomic gaseous hydrogen.
When hydrogen (C3H2 +) is heated to 300°C (500°F) and a second hydrogen atom (C2H3) is added it reacts with oxygen (O2) in order to form carbon dioxide (CO2). This process is called “reaction of carbon”, or RCO 2 . 
When the temperature is lowered to 250°C (380°F), carbon dioxide (CO2) is lost and a second hydrogen atom is added. This process is called “reaction of sulphur”, or RSO 2 . This reaction is the mechanism for the formation of the oxygen-laden hydrocarbons in the combustion of fossil fuels.
The reaction of hydrogen in the presence of a second element is called “heterogeneous RCO 2 + O2”
The chemical bond (dipole moment) of the reactants is the ratio of their mutual charges. This is the RIC (Received Acidic Equivalents) of the reactants and O 2 – and -OH bonds of the heterogeneous RCO 2 + O2 reactions are shown below:
In order to achieve the higher boiling point required for carbon dioxide and methane production, the molecules of air contain a higher ratio of hydrogen to oxygen than the bulk of the water used in the combustion.
The equilibrium state between nitrogen and oxygen is called “equilibrium boiling point”. The critical pressure for nitrogen (1.0 bar), oxygen (1.0 bar) and CO 2 (2.0 bar):
Equilibrium boiling point (K) for a given temperature (C) = 1/8.24 + 1 = 1.097 = 12.6
The equilibrium state for a fixed level of energy (G):
Equilibrium boiling point (K) for a fixed level of energy (G) = 1/0.36 + 1 = 1.17 = 14.1
The equilibrium temperature of hydrogen gas in the presence of a second metal is also given by the RIC.
RIC for hydrogen in solution (H2O2) = 1.0 + 0.9 x V 2 /5.66 x 10-4 x 12 = 1.0 + 1.0 x R 2 /4.26 /10-5 x 10-4 x 13 = 0.038
Equilibrium temperature of methane in the presence of a metal
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