Given the unbalanced equation Ca(s) + Ag+(aq) → Ca2+(aq) + Ag(s), for a reaction, what is being reduced?

Ag^+ is reduced to Ag^0

Explanation:

Based on the equation

Ca+Ag^+=Ca^2+ + Ag

Ca^0 is increased to Ca^2+

And Ag^+ is reduced to Ag^0

Ag is reduced in the reaction.

Explanation: From the balanced equation: Ca + Ag+ => Ca2+ + Ag

For an element to be reduced there must be a decrease in oxidation number. For Ca in the reactant it is an independent atom so its oxidation number is 0. The on the product the oxidation number of Ca increases to 2+. So Ca is oxidized.

Ag in the reactant has an oxidation of +1 and decreases on the product side where its oxidation is 0. So Ag is reduced in the reaction since there is a decrease in oxidation number.

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