How is equilibrium established in reversible reactions?

Equilibrium in a reversible reaction is established when the rate of the forward reaction becomes equal to the rate of the backward reaction.

Here’s how it happens in simple terms:

1. Initially:
   • Reactants start converting into products, so the forward reaction is faster.
   • The backward reaction is slower because there are few products at the beginning.
2. As the reaction proceeds:
   • Products build up, so the backward reaction starts speeding up.
   • The forward reaction slows down slightly as reactants are used up.
3. At equilibrium:
   • Both forward and backward reactions occur at the same rate.
   • The concentrations of reactants and products remain constant over time.
   • The system becomes a dynamic balance — reactions continue, but there’s no net change.

In short: Equilibrium is a dynamic state where the forward and backward reactions balance each other.