Exothermic reaction moves forward with increase in Temp?

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An exothermic reaction, such as the syngas reaction CH4 + 0.5O2 → 2H2 + CO, can proceed to completion at high temperatures, contrary to the expectation that increased temperature would drive it backward. This behavior is influenced by the number of moles of products being greater than that of the reactants, suggesting a role for entropy. The equilibrium position can remain significantly shifted to the right even at elevated temperatures. The discussion highlights that the shift to the left in exothermic reactions may be minimal. Understanding these dynamics is crucial for predicting reaction behavior under varying conditions.
leumas614
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I did an equilibrium calculation with some chem software that I have and it told me that a syngas reaction

CH4+0.5O2\rightarrow 2H_{2}+CO

which is an exothermic reaction will proceed to completion at high temperature. If you increase temperature, that should drive the reaction backwards not forwards. I think it has something to do with the fact that there are more moles of products than reactants. Does it have something to do with entropy?

Thanks
 
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Just because reaction is exothermic doesn't mean its equilibrium can't lie far to the right, even in high temperatures. Shift to the left can be very small.

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