# Would a reaction occur if solid tin was placed in a solution of copper (II) nitrate?

## If so, what is the balanced net ionic equation for the reaction?

Jun 25, 2018

No because....

#### Explanation:

Tin is less reactive and can not displace copper..

Jun 25, 2018

Of course a reaction would occur

#### Explanation:

As the standard reduction potential of copper is higher than tin, it will get reduced.

Net reaction is:

$C u {\left(N {O}_{3}\right)}_{2} + S n \rightarrow S n {\left(N {O}_{3}\right)}_{2} + C u$

Jun 25, 2018

The single replacement reaction will occur.

The net ionic equation is:

$\text{Sn(s) + Cu"^(2+)("aq")}$$\rightarrow$$\text{Cu(s) + Sn"^(2+)("aq")}$

#### Explanation:

In order to determine whether a reaction will occur we need to consult a reactivity series of metals like the one below. In a single replacement reaction can occur only if the metal reactant, in this case tin (Sn) is more reactive than the metal in the reactant that is a compound, in this case copper (Cu). As you can see, tin is above copper in the reactivity series, so this reaction will occur. Balanced molecular equation

$\text{Sn(s) + Cu(NO"_3)_2("aq")}$$\rightarrow$$\text{Cu(s) + Sn(NO"_3)_2("aq")}$

Complete ionic equation

$\text{Sn(s) + Cu"^(2+)("aq") + "2NO"_3("aq")}$$\rightarrow$$\text{Cu(s) + Sn"^(2+)("aq") + "2NO"_3("aq")}$

Net ionic equation

Remove the ions that occur on both sides of the equation.

$\text{Sn(s) + Cu"^(2+)("aq")}$$\rightarrow$$\text{Cu(s) + Sn"^(2+)("aq")}$