Here's why:
* Reversible reactions proceed in both directions, meaning reactants can form products, and products can also react to form reactants.
* The rate of each direction (forward and reverse) is influenced by the concentrations of the involved species.
* Equilibrium is reached when the rates of the forward and reverse reactions become equal, meaning the net change in concentration of reactants and products is zero.
Examples of reversible reactions:
* The Haber-Bosch process: N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
* The reaction of hydrogen and iodine: H₂(g) + I₂(g) ⇌ 2HI(g)
* The dissolution of a salt in water: NaCl(s) ⇌ Na⁺(aq) + Cl⁻(aq)
In contrast, irreversible reactions proceed in one direction only, and their rate is not significantly influenced by the concentration of products.
