Question #9ecfb

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Ernest Z.
Mar 8, 2017

The balanced equation is #"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("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 #"Ag"^"+"# ion to #"Ag(s)"# and is in turn oxidized to #"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")#

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