Answer:
See Explanation
Explanation:
From the data given an argument for either reactant as limiting can be presented. The Limiting Reactant is that reactant which when consumed the reaction stops as the remaining reactant does not have any reagent to react with.
Based on this definition, if one adds a small quantity of AgNO₃ solution to a large quantity of copper wire the interaction will spontaneously react with copper metal undergoing oxidation forming CuNO₃ followed by formation of the reduced form of silver precipitate until all of the AgNO₃ is consumed and the reaction stops. In this case, the AgNO₃ is the limiting reactant and the copper will remain in excess.
On the other hand and based on this definition of limiting reactant, one can add a small amount of copper wire to a concentrated solution of AgNO₃ and the same reaction will spontaneously occur. However, in this reaction system the reaction would proceed until all of the copper wire is consumed (dissolved) and the reaction stops leaving an excess of unreacted AgNO₃ in solution with CuNO₃ and reduced Ag.
Problems dealing with limiting reactants require specifying the quantities of each reactant from which identification for the limiting reactant can be specified. One simple way to ID the limiting reactant is to convert all given reactant quantities to moles followed by dividing each by its respective coefficient from the balanced rxn equation. The smaller value will be the limiting reactant.
