For the reaction: CH₄(g)+ 2 H₂O(g)⇌ CO₂(g)+ 4 H₂(g),Δ_rH° = +190 kJ,when the temperature is raised to 1200 K:

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According to Le Chatelier's principle, when the temperature is increased, the equilibrium will shift to consume some of the added heat. Since this is an endothermic reaction (ΔH° is positive), the forward reaction is favored by an increase in temperature. Therefore, the equilibrium will shift to the right, producing more products (COS and HS) and reducing the amount of reactants (CH and H2S).

For the Reaction: CH4(g)+ 2 H2O(g)⇌ CO2(g)+ 4 H2(g),ΔrH° =

For the Reaction: CH₄(g)+ 2 H₂O(g)⇌ CO₂(g)+ 4 H₂(g),Δ_rH° =