Why equilibrium is dynamic in nature

The reaction is still going on in the forward and backward direction but the rate of forwarding reaction is equal to the rate of backward reaction. Hence, chemical equilibrium is dynamic in nature and not static. Report Error Is there an error in this question or solution?

Chapter Chemical Equilibrium - Exercises [Page ]. A Page Share 0. Select a course. My Profile. The equilibrium can be made to shift in either direction by changing the concentration, Pressure, or Volume. Hence it is dynamic in nature. Stoichiometric Representation Of Equilibrium Constant. National education day: e-learning transforming educational landscape. Understanding the importance of education with e-learning transforming. JEE Main may commence the registration in the first week of Dec tentatively.

CBSE has released the term-1 admit card SBI PO prelims admit card released. Share This Video. Apne doubts clear karein ab Whatsapp par bhi. Try it now. This is the case because at different temperatures, more products or reactants may exist in solution. If there is a very large concentration of either a product or reactant, it will shift the equilibrium one way or the other. This is because the addition of reactants or products will always yield a reaction one way or the other, unless the reaction can no longer dissolve any more of it.

In that case, it becomes a precipitate which does not effect equilibrium. This affects gaseous products and reactants. The side where there is more gas is the side in which the equilibrium will shift to if the pressure is decreased, because more can fit now.

Vice versa as well. There are many factors that shift equilibrium Kc so we must always be wary of these factors before we jump to a conclusion about what the equilibrium is, because it is very dynamic! Good question Now, by definition, the chemical condition of equilibrium is defined when the forward and reverse rates are equal:. However, a chemist or engineer can certainly manipulate the equilibrium.

For instance, if we remove somehow the products of the reaction, C and D , the equilibrium will have to re-establish itself, and it does this by moving to the right as written to satisfy the equilibrium equation, and to re-establish equilibrium concentrations of C and D. On the other hand, if we pump more reactant into the equilibrium, the equilibrium will move in a forward direction to cope with increased [A] and [B].