Question

Consider the chemical equilibrium of the reaction. AgCl(s) <---> Ag+(aq) + Cl–(aq) What will happen to the chemical equilibrium if AgNO3 is added? There is no shift in the chemical equilibrium of the system. The chemical equilibrium of the system shifts to the right. The chemical equilibrium of the system shifts to the left. The chemical equilibrium of the system is destroyed.

Answer 1

The chemical equilibrium shifts to the left.

In a chemical equilibrium, the products and reactants are balanced, and there is no net production or consumption. When silver nitrate will be added, it will disturb the equilibrium by creating more silver ions. The system will produce a change in order to counter this, according to Le Chatelier's principle, and less silver ions will be released from the silver chloride, decreasing the solubility of silver chloride. This effect is also termed the common ion effect.<span />

Answer 2

Answer:

The correct answer is "The chemical equilibrium of the system shifts to the left."

Explanation:

In most chemical reactions the reagents are not consumed completely to obtain the desired products. On the contrary, there comes a time when it seems that the reaction is over. This is observed in that the concentration of the reagents consumed and products formed remain constant. This does not mean that a reaction has ended, but that the reagents are continually becoming in products and products become reagents.

The chemical equilibrium is a state of a reactant system in which they are not observed changes as time goes by, even though the reaction continues. In other words, the chemical equilibrium is established when there are two opposite reactions which take place simultaneously at the same speed.

The variation in the concentration of any of the species involved in the equilibrium varies the value of the concentrations of the remaining species in the equilibrium.   AgNO3 silver nitrate is a salt that contributes Ag + and NO3- ions to the reaction medium. In other words, it contributes Ag + ions, one of the products of the reaction:

AgCl(s) ⇔ Ag+(aq) + Cl- (aq)

This varies the concentration of one of the reaction products (Ag+), increasing it since there is a greater amount of Ag + ions. This causes the equilibrium to shift to the reagents to compensate for the reaction. Then the balance goes to the left.

So, the correct answer is "The chemical equilibrium of the system shifts to the left."