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I am trying to model some industrial processes and having a hard time finding information about the Sabatier reaction. The Sabatier reaction combines $\ce{CO2}$ (and possibly $\ce{CO}$) with $\ce{H2}$ to produce $\ce{H2O}$ and $\ce{CH4}$.

On the one hand, this reaction is exothermic. On the other hand, it requires high heat and pressure. Does the reactor need initial heating and pressurizing of the gases, and then is it self-sustaining (or rather requiring cooling)?

What is clear is that some energy is be needed to compress gases and flow them over the catalysts.

Are there any estimates of how much energy a reactor would use? I understand that scale would also be an important parameter, but any preliminary estimates are useful to me.

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  • $\begingroup$ It is a chemical kinetics issue. Raising the temperature increases the rate of the reaction. $\endgroup$
    – Chet Miller
    Mar 14, 2021 at 20:25
  • $\begingroup$ Useful paper on this topic regarding the need to initially heat and then remove heat from reactor. pubs.rsc.org/en/content/articlelanding/2018/se/… $\endgroup$
    – dlight
    Mar 15, 2021 at 18:28
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    $\begingroup$ It is rather chemical engineering question, comparing rate of heat production and rate of heat sink at given operational temperature. $\endgroup$
    – Poutnik
    Jul 30, 2022 at 16:23
  • $\begingroup$ I'm a chemical engineer. What is the heat of reaction for this reaction? I mean the place I work at is doing an even stupider reaction so this one deserves a bit more looking into $\endgroup$
    – Pulkit Sharma
    Jul 30, 2022 at 17:15
  • $\begingroup$ @Maurice your answer has zero value. Do you know what "modeling" means. Maybe you should climb down from your high horse so you can read the question better? $\endgroup$
    – dlight
    Aug 15, 2022 at 17:53

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