Question #bf3a3
1 Answer
Explanation:
When you add a strip of zinc metal to a solution of copper(II) nitrate, a single replacement reaction takes place.
Zinc will displace copper from the solution. This will result in the formation of aqueous zinc nitrate,
"Zn"_ ((s)) + "Cu"("NO"_ 3)_ (2(aq)) -> "Zn"("NO"_ 3) _ (2(aq)) + "Cu"_ ((s))
The nitrate anions,
"Zn"_ ((s)) + "Cu"_ ((aq))^(2+) -> "Zn"_ ((aq))^(2+) + "Cu"_ ((s))
Another way to think about this reaction involves recognizing the fact that electrons are being transferred here, which implies that this is also a redox reaction.
Zinc metal reduces copper cations,
You have
"Zn"_ ((s)) -> "Zn"_ ((aq))^(2+) + color(red)(cancel(color(black)(2"e"^(-))))
"Cu"_ ((aq))^(2+) + color(red)(cancel(color(black)(2"e"^(-)))) -> "Cu"_ ((s))
color(white)(aaaaaaaaaaaaaaaaaaaaa)/color(white)(a)
"Zn"_ ((s)) + "Cu"_ ((aq))^(2+) -> "Zn"_ ((aq))^(2+) + "Cu"_ ((s))