Dynamic Equilibrium occurs when the rates of forward and reverse reactions are equal. It's like a dance battle between two teams, where each side is bringing their best moves but no one is winning or losing!

Reactions can go both ways: from reactants to products and from products back to reactants! In chemical equations, we show this with the equilibrium sign (⇌). For instance - Liquid Bromine (Gaseous Bromine) Liquid Bromine - Br₂​(l) ⇌ Br₂​(g) (Gaseous Bromine) 

It's a state where everything seems calm and unchanging, but there's a ton of action happening microscopically! Imagine a game of musical chairs where everyone is swapping chairs but the number of people sitting and standing remains constant!

👉 Real-world Example

Place liquid bromine in a flask, and it will evaporate, increasing gaseous bromine concentration. But, some gaseous molecules will also condense back. When the rate of evaporation equals the rate of condensation, voilà, Dynamic Equilibrium!

• Heterogeneous Equilibrium: Different phases involved (e.g. Liquid ⇌ Gas, Solid ⇌ Aqueous).
• Chemical Equilibrium: Reaction involving the interconversion of reactants and products.