Why reversible reaction never complete
Hey Bob Make It Simple.R.R Attain Equiblirium.Thats The Reason Mothers Boy.Muhaa
The reason a reversible reaction never fully completes is due to something called equilibrium. In a reversible reaction, reactants can react to form products, and products can also react to reform reactants. At the beginning of the reaction, the concentration of reactants is typically higher than that of the products. As the reaction proceeds, the concentrations of products increase while the concentrations of reactants decrease.
However, as the concentrations of products increase, a point is eventually reached where the reverse reaction becomes favorable as well. This means that while the forward reaction is still occurring, the reverse reaction is also happening simultaneously. At equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain relatively constant over time.
The position of equilibrium is determined by various factors, including temperature, pressure, and the concentrations of reactants and products. In some cases, the equilibrium position may favor the formation of more reactants, resulting in a lower yield of products. In other cases, the equilibrium position may favor the formation of more products, resulting in a higher yield.
So, in a reversible reaction, the reaction never fully completes because it continually reaches a point of equilibrium where both the forward and reverse reactions are occurring simultaneously.