# Question 9ecfb

Mar 8, 2017

The balanced equation is $\text{Cu(s)" + "2AgNO"_3"(aq)" → "Cu"("NO"_3)_2"(aq)" + "2Ag(s)}$

#### Explanation:

The reaction can be called a single displacement reaction.

Copper is above silver in the activity series of metals.

Thus, copper will displace silver from its salts.

The silver deposits as a finely-divided gray-black solid "mold" on the copper, and the greenish colour is caused by the aqueous solution of copper(II) nitrate.

$\underbrace{\text{Cu(s)")_color(red)("copper") + underbrace("2AgNO"_3"(aq)")_color(red)("silver nitrate") → underbrace("Cu"("NO"_3)_2"(aq)")_color(red)("blue-green solution") + underbrace("2Ag(s)")_color(red)("gray-black}}$

The reaction is also a reduction-oxidation reaction.

The copper reduces the $\text{Ag"^"+}$ ion to $\text{Ag(s)}$ and is in turn oxidized to $\text{Cu"^"2+}$ ion.

The net ionic equation is "Cu(s)" + "2Ag"^"+" → underbrace("Cu"^"2+""(aq)")_color(red)("blue-green") + underbrace("2Ag(s)")_color(red)("gray-black")#