Concept:A catalyst provides an alternative reaction pathway with a lower activation energy, accelerating both forward and backward rates equally.
Formula:$$ \text{Rate} = k[\text{Reactants}]^x \quad (k \text{ increases via lower } E_a) $$
Solution:- Because the activation energy barrier is lowered from both sides, particles require less kinetic energy to react successfully.
- Both the forward and reverse reaction rates spike proportionally.
- As a result, the time required to balance these two rates (attain equilibrium) is significantly reduced.
Why other options are incorrect:While temperature increases rate, it also shifts the equilibrium position. A catalyst uniquely accelerates the attainment of equilibrium without shifting its final position.
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