I keep getting “Activation energy” questions wrong in Chemical Kinetics. What's the trap?
thinking a catalyst changes ΔH or the position of equilibrium.
The usual trap: thinking a catalyst changes ΔH or the position of equilibrium. How to avoid it: a catalyst speeds BOTH directions equally — it never shifts equilibrium. Go back to the definition — the minimum energy barrier reactants must cross; a catalyst lowers it.
Key point
Activation energy
Common mistake
thinking a catalyst changes ΔH or the position of equilibrium.
Memory tip
a catalyst speeds BOTH directions equally — it never shifts equilibrium.
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