Molecules of A and B (blue/red) wander the reaction vessel and convert to product C (green) when they collide with enough energy — a toy A + B ⇌ 2C equilibrium.
k = A₀·exp(−Eₐ / R·T) (Arrhenius equation)
Equilibrium: rate_forward = rate_reverse
- Temperature — higher T exponentially increases both forward and reverse rates, reaching equilibrium faster (and shifting it, since the reverse step has a higher effective barrier).
- Activation energy — the energy barrier collisions must clear to react; raising it slows the whole system down.
- Catalyst — lowers the barrier for both directions equally, speeding up the approach to equilibrium without shifting where it settles.
Real-world relevance: this is exactly why industrial reactors use catalysts and precise temperature control — to hit a target conversion rate without waiting for (or overshooting) the reaction's natural equilibrium.