Respuesta :
The half-reactions are as follows
At anode: [tex]Zn (s) \longrightarrow Zn^{2+}(aq) + 2e^-[/tex]
At cathode:[tex]Sn^{2+}(aq) + 2e^- \longrightarrow Sn (s)[/tex]
The overall reaction of the cell is
[tex]Zn (s) + Sn^{2+}(aq) \longrightarrow Zn^{2+}(aq) + Sn (s)[/tex]
What is a voltaic cell?
The device in which electrons are transferred through an external source is known as a voltaic cell.
The electron flow of a voltaic cell allows redox reactions to produce energy in the form of electricity.
An anode, a cathode, and a salt bridge are all parts of a voltaic cell's setup. The salt bridge serves to neutralize the system.
To write the balanced half-cell reactions. Identify which metal is oxidized and which is reduced.
As the Zinc electrode is negative. Hence, zinc metal is being oxidized
At the anode, oxidation occurs
[tex]Zn (s) \longrightarrow Zn^{2+}(aq) + 2e^-[/tex]
At the cathode, reduction occurs
[tex]Sn^{2+}(aq) + 2e^- \longrightarrow Sn (s)[/tex]
Both reactions are already balanced.
Write the overall cell reaction
[tex]Zn (s) + Sn^{2+}(aq) \longrightarrow Zn^{2+}(aq) + Sn (s)[/tex]
Learn more about Voltaic cells:
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