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Suppose we are doing heterogeneous catalysis, for example, between nitrogen and hydrogen to create ammonia in the presence of a solid catalyst, like rhuthenium. It's obvious that the gas molecules don't "collide" directly and, therefore, the Arrhenius equation does not completely apply. Does a modified version of the equation exist that takes this into account?

My guess would be that since catalysts generally decrease the activation energy of a reaction, the activation energy value would possibly have a fractional component to it. Furthermore, because the reaction is occurring on a surface, the decreased direct collisions may affect the rate. I would greatly appreciate it if someone could point me in the right direction.

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    $\begingroup$ Being catalyzed is not the major modification factor. The major factor is becoming a reaction on solid surface, instead in free volume. $\endgroup$
    – Poutnik
    Oct 29 '21 at 6:02
  • $\begingroup$ I would start with the 2D model of the multistep reaction mechanism, each step having its own activation energy. ( so does not catalyzed reaction if free space ) $\endgroup$
    – Poutnik
    Oct 29 '21 at 9:41

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