Answer:
Increasing the reactants in the reaction.
Explanation:
By Le Chatelier's principle, any additional reactant added to the system (silver or chlorine reactant) would shift the reaction equilibrium to the right, favouring the product formation. That is more product is formed when the equilibrium is disturbed by adding more reactant.
I hope this explanation is clear.
The addition of solid silver chloride has resulted in the disturbed equilibrium, and the equilibrium has been shifted towards the left.
The equilibrium principle states that the addition of the reactants shifts the equilibrium to the right, while the addition of the product shifts the equilibrium to the left.
The equilibrium has been the state when the concentration of the products and reactants in the solution has been equal. The addition of the reactant and products will disturb the equilibrium and shift it towards the other species in the reaction.
The AgCl has been the product in the reaction. The addition of solid silver chloride in the solution results in the early reaching of the equilibrium as soon the concentration of reactants and products become equal.
Thus, the addition of solid silver chloride has resulted in the disturbed equilibrium, and the equilibrium has been shifted towards the left.
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