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.

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dangerousmattoycs4v dangerousmattoycs4v · Answer 1 · 2017-12-05T04:04:37+01:00

Not complete the sure, but I think it’s

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

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Giangiglia Giangiglia · Answer 2 · 2019-10-15T17:10:37+02:00

Answer:

[tex]Zn (s) + SnSO_4 (aq)\longrightarrow ZnSO_4 (aq) + Sn (s)[/tex]

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: [tex]Zn (s) \longrightarrow Zn^+^2 (aq) + 2e^-[/tex]

The reduction reaction will be performed by the Sn:

Reduction hemireaction: [tex]Sn^+^2 (aq) + 2e^- \longrightarrow Sn (s) [/tex]

Writting the net redox equation:

[tex]Zn (s) + Sn^+^2 (aq) + 2e^-\longrightarrow Zn^+^2 (aq) + 2e^- + Sn (s)[/tex]

[tex]Zn (s) + SnSO_4 (aq)\longrightarrow ZnSO_4 (aq) + Sn (s)[/tex]