Chemical Equilibrium Explained: Identifying Correct Statements

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Chemical equilibrium is a state in a chemical reaction where the concentration of the reactants and products no longer changes with time. This does not mean the reaction has stopped, but rather, the rates of the forward and reverse reactions have become equal. Let's delve into each of the given options to understand them better.

Statement A says that in equilibrium, the concentrations of products and reactants are equal. This is a common misconception. In reality, equilibrium doesn't mean that products and reactants are equal in concentration, but that their concentrations do not change because the rate of formation of products equals the rate of formation of reactants.

Statement B suggests that an equilibrium reaction is irreversible. But that's not true. Equilibrium reactions are, in fact, reversible. When a reaction is at equilibrium, the forward and reverse reactions continue to occur - they don't stop