A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper. The solution turned a blue color characteristic of copper(II) ions. Select the correct balanced chemical equation for this reaction. A) Cu(s) + AgNO₃(aq) $\rarr$Ag(s) + Cu(NO₃)₂(aq) B) Cu(s)₂ + AgNO₃(aq) $\rarr$ Ag(s) + Cu(NO₃)₂(aq) C) Cu(s) + 2AgNO₃(aq) $\rarr$ 2Ag(s) + Cu(NO₃)₂(aq) D) 2Cu(s) + 2AgNO₃(aq) $\rarr$2Ag(s) + 2Cu(NO₃)₂(aq) E) None of the above

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction should have the same number of atoms of each element on both sides of the equation. In this case, copper (Cu) is oxidized to Cu2+ and silver ions (Ag+) are reduced to silver metal (Ag). The correct balanced equation is:

Cu(s) + 2AgNO3(aq) → 2Ag(s) + Cu(NO3)2(aq)

The blue color of the solution is due to the formation of Cu2+ ions, which are blue in aqueous solution.

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