Concept:A catalyst provides an alternative reaction pathway with a lower activation energy, which accelerates both the forward and reverse reaction rates proportionally.
Formula:$$ \text{Rate} \propto e^{-E_a / RT} $$
Solution:- When activation energy (\( E_a \)) is lowered by a Catalyst, a much larger fraction of molecules possess enough kinetic energy to react.
- Both the forward and backward rates spike simultaneously.
- Because both opposing rates are faster, they intersect and balance each other out in a fraction of the time.
- Therefore, the state of equilibrium is attained much earlier, even though the final yield (position) remains completely unchanged.
Why other options are incorrect:While temperature and concentration changes can affect rates, they also shift the position of the equilibrium. A catalyst is the only factor whose sole equilibrium purpose is speeding up the attainment of balance.
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