Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing tin and silver: sn(s)|sn2 (aq)||ag (aq)|ag(s)

The half reactions as they occur at each electrode

is as follows

at the anode Sn(s) =sn^2+(aq) + 2e -
at the cathode 2 ag^+(aq) + 2e - = 2Ag (s)

net cell reaction = Sn (s) + 2Ag^+(aq) = sn^2+ (aq) + 2 Ag (s)

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aliasger2709 aliasger2709 · Answer 2 · 2022-04-13T10:30:57+02:00

An electrochemical cell generates or uses electrical energy for chemical reactions. At the anode of the cell, tin forms a tin ion and releases two electrons.

What is a half-cell?

A half-cell in an Electrochemical cell is one of the electrodes and electrolytes of the cell which connect to another half by a salt bridge.

The anode of the half-cell is the electrode where the oxidation takes place and the electrons are lost. The half-reaction at the anode is shown as,

[tex]\rm Sn(s) \rightarrow Sn^{2+}(aq) + 2e^{-}[/tex]

The cathode of the half-cell is the electrode where the reduction takes place, and the electrons are gained. The half-reaction at the cathode is shown as,

[tex]\rm 2 Ag^{+}(aq) + 2e^{-} \rightarrow 2Ag (s)[/tex]

The overall net reaction of the electrochemical cell is shown as,

[tex]\rm Sn(s) + 2 Ag^{+}(aq) \rightarrow Sn^{2+}(aq) + 2Ag (s)[/tex]

Therefore, the half-reaction at the cathode results in the gaining of electrons.

Learn more about half-reactions here:

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