A catalyst increases the rate of reaction by:

Decreasing the activation energy with unchanged equilibrium state

The correct answer is Option (3) → Decreasing the activation energy with unchanged equilibrium state

A catalyst speeds up a chemical reaction by providing an alternative reaction pathway with lower activation energy.

Activation energy is the minimum energy required for reactant molecules to form the activated complex and proceed to products.

By lowering the activation energy, more molecules can successfully react, increasing the reaction rate.

However, a catalyst does not affect the thermodynamic properties of the reaction:

• It does not change Gibbs free energy (ΔG)

• It does not change the equilibrium constant

• It does not shift the equilibrium position

A catalyst only helps the system reach equilibrium faster.