- #1
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
[tex]CH4+0.5O2\rightarrow 2H_{2}+CO[/tex]
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
[tex]CH4+0.5O2\rightarrow 2H_{2}+CO[/tex]
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