Question

A piece of solid Zn metal is put into an aqueous solution of SnSO4. Write the net ionic equation for any single-replacement redox reaction that may be predicted.

Answer 1

Not complete the sure, but I think it’s

Zn(s) + SnSO4(aq) —> ZnSO4(aq) + Sn(s)

Answer 2

`Zn (s) + SnSO_4 (aq)\longrightarrow ZnSO_4 (aq) + Sn (s)`

Step-by-step explanation:

Hi, when adding Zn to the solution because of its high reactivity it will displace the Sn. This process is a redox reaction.

First step is to identify the compound that oxidates and the compound that reduces. The Zn has a high oxidation potencial so it will oxidate:

Oxidation hemireaction:
`Zn (s) \longrightarrow Zn^+^2 (aq) + 2e^-`

The reduction reaction will be performed by the Sn:

Reduction hemireaction:
`Sn^+^2 (aq) + 2e^- \longrightarrow Sn (s)`

Writting the net redox equation:

`Zn (s) + Sn^+^2 (aq) + 2e^-\longrightarrow Zn^+^2 (aq) + 2e^- + Sn (s)`

`Zn (s) + SnSO_4 (aq)\longrightarrow ZnSO_4 (aq) + Sn (s)`