Which risk increases when a chemical reactor operates significantly off ideal equilibrium constant conditions?

💡 Explanation

When reactants are far from the concentrations predicted by the equilibrium constant, the reaction shifts to restore equilibrium, causing the faster kinetics and heat generation, driving a positive feedback loop and increasing risk of a runaway reaction. Therefore, a runaway reaction is more likely, rather than catalyst poisoning, reduced yield or increased energy solely which require different mechanisms.

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