Question

What does it mean when equilibrium shifts to the left?

Answer 1

Hint: We have to remember that the transformation of reactant to product is known as chemical reaction. There are some factors that will affect the chemical reactions and that is, temperature, presence of catalyst, concentration of reactant, physical state of the reactant and surface area. The catalyst is the substance which is used to increase the rate of a chemical reaction. And it will not consume itself. And the catalyst is the substance which increases the speed and rate of the reaction.

Complete answer:
According to Le Chatelier’s principle, when equilibrium shifts to the left, there is a formation of more reactants by adding additional products to the chemical reaction. And the equilibrium can be shifted also by taking out some reactant from the system. The Le Chatelier’s principle explains the chemical equilibrium of the reactions. This principle explains that, the changes in the volume, pressure, concentration of and temperature the system may lead to achieve the new equilibrium state of a reaction. The equilibrium position of the changes in the system reduces the effect of any forced changes in the reaction condition. Which means, the rising of temperature will help in the case of endothermic reaction. The presence of a catalyst will not affect the position of the equilibrium reaction.

Note:
We must have to remember that the position of equilibrium reaction can be explained on the basis of Le Chatelier’s principle. When the concentration of the product is reduced, then the equilibrium will shift towards the right. And if we put more product to the system, then the reaction will shift towards the left and form more reactant. Hence, the formation of more product and take out the reactants may lead to shift the equilibrium to the left.