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A galvanic (voltaic) cell contains a copper cathode immersed in a copper(ii) chloride solution and a nickel anode immersed in a nickel(ii) chloride solution. the two solutions are connected with a salt bridge. write the balanced equation for the galvanic cell. phases are optional.

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We can write the balanced equation for the galvanic cell by using the oxidation and reduction half-reactions. In the anode, Ni(s) is oxidized and produces aqueous Ni2+:
     Ni(s) → Ni2+
while in the cathode, Cu2+ is reduced and deposits copper:
      Cu2+ → Cu(s)
We now balance the charge of each reaction by adding electrons to the side of the equation with the greater charge:
     Ni(s) → Ni2+ + 2 e-
     Cu2+ + 2 e- → Cu(s)
Finally, we add the half-reactions to obtain the overall balanced equation for the galvanic cell:
     Cu2+(aq) + Ni(s) → Ni2+(aq) + Cu(s)

The overall reaction for the galvanic cell has been [tex]\rm Cu^2^+\;+\;Ni\;\rightarrow\;Ni^2^+\;+\;Cu[/tex].

The galvanic cell has been given as the electrochemical cell that converts chemical energy of the reaction into electrical energy.

Balanced equation for the Galvanic cell

The galvanic cell has anode as the oxidizing electrode, whee the loss of electrons takes place, and cathode as the reducing electrode where the gain of electrons takes place.

The cathodic reaction in the cell has been:

[tex]\rm Cu^2^+\;\rightarrow\;Cu\;(s)[/tex]

The anodic reaction in the cell has been:

[tex]\rm Ni\;(s)\;\rightarrow\;Ni^2^+[/tex]

The overall reaction for the galvanic cell has been:

[tex]\rm Cu^2^+\;+\;Ni\;\rightarrow\;Ni^2^+\;+\;Cu[/tex]

Learn more about galvanic cell, here:

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