# Le Chatelier's Principle on the Haber Bosch process [closed]

Why would the forward reaction of $$\ce{N2(g) + 3H2(g) <=> 2NH3(g)}$$ be favored if bubbling the reaction mixture through $$\ce{HCl(aq)}$$ rather than $$\ce{NaOH(aq)}$$? Is it related to the concentration of $$\ce{H+}$$ ions in these two solutions?

## closed as unclear what you're asking by andselisk, A.K., Nuclear Chemist, Mithoron, TyberiusFeb 11 at 16:39

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• You should edit your question to add some more context and make it clearer. – porphyrin Feb 10 at 14:28
• Nothing was really said about that, we were just asked to explain why adding those would yield a greater concentration of ammonia – SuperMage1 Feb 10 at 14:36
• The equation does not describe an acid base reaction, and neither hydronium ions nor hydroxide ions appear in it. Nevertheless, the statement suggests that acid base chemistry plays a role. I always thought the Haber Bosch process takes place in the gas phase, not in aqueous solution, so the acid base chemistry is less clear (as is how you would add NaOH in a meaningful way). It would help if you could add the physical state (s, l, g, aq) to the equation to clarify. – Karsten Theis Feb 10 at 15:20
• Think about which components of your reaction would react with acid or base. If the reaction with acid or base causes the concentration of component to go down, it will pull the reaction in that direction. – Andrew Feb 11 at 13:21