A small value of the equilibrium constant (K) indicates that, at equilibrium, the concentration of reactants is much higher than that of the products. This means the reaction favors the reactants and does not proceed significantly in the forward direction to form products

. In other words, when K is very small (much less than 1), the equilibrium position lies to the left, meaning the reaction hardly converts reactants into products and mostly remains with the reactants present

. This also implies that equilibrium is achieved at low product concentration

. To summarize:

• A small equilibrium constant means the reaction favors reactants.
• The reaction proceeds very little towards product formation.
• The concentration of reactants at equilibrium is large relative to products.
• Equilibrium is established with low product concentration.

This understanding helps predict the direction and extent of a chemical reaction under equilibrium conditions