Q.Salt bridge can be prepared with a laminated long strip of good quality filter paper. Cut the two ends of a laminated strip. Dip the two ends in a saturated solution of KCl for 24 hours. This strip can be used as salt bridge by dipping the two ends in two solutions.

Reduction is the gain of electrons; in the Daniell cell it is the $Cu^{2+}$ ion that gains electrons and deposits as copper metal.

Identifying the half-reactions

The overall cell reaction is: $Zn(s) + Cu^{2+}(aq) \rightarrow Zn^{2+}(aq) + Cu(s)$.

Splitting it: zinc metal is losing electrons to become $Zn^{2+}$ (oxidation), while $Cu^{2+}$ ions are gaining electrons to become copper metal (reduction).

Reduction half-reaction

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Oxidation is the loss of electrons; in the Daniell cell the zinc electrode loses electrons and dissolves into solution as $Zn^{2+}$.

Identifying the half-reaction

From the overall reaction $Zn(s)+Cu^{2+}(aq)\rightarrow Zn^{2+}(aq)+Cu(s)$, zinc metal is converted to $Zn^{2+}$ ions, which requires the loss of two electrons per Zn atom — this is oxidation.

Oxidation half-reaction

$Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$

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The anode is, by definition, the electrode at which oxidation takes place — in the Daniell cell this is the zinc electrode.

Why zinc is the anode

In any galvanic cell, the anode is defined as the electrode where oxidation occurs. Since zinc metal loses electrons and goes into solution as $Zn^{2+}$ (as shown by the overall reaction $Zn(s)+Cu^{2+}(aq)\rightarrow Zn^{2+}(aq)+Cu(s)$), the zinc electrode is the site of oxidation.

Half-cell reaction at the anode

$Zn(s) \rightarrow Zn^{2+}(aq) + 2e^-$

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The cathode is, by definition, the electrode at which reduction takes place — in the Daniell cell this is the copper electrode.

Why copper is the cathode

In any galvanic cell, the cathode is defined as the electrode where reduction occurs. Since $Cu^{2+}$ ions gain electrons and are deposited as copper metal (from the overall reaction $Zn(s)+Cu^{2+}(aq)\rightarrow Zn^{2+}(aq)+Cu(s)$), the copper electrode is the site of reduction.

Half-cell reaction at the cathode

$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$

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A galvanic cell is an electrochemical device that generates electricity directly from a spontaneous chemical (redox) reaction by keeping oxidation and reduction physically apart.

Definition

A galvanic cell (also called a voltaic cell) is an electrochemical device in which the chemical energy released by a spontaneous ($\Delta G < 0$) redox reaction is converted directly into electrical energy. This is achieved by physically separating the oxidation half-reaction and the reduction half-reaction into two different half-cells (each containing an electrode dipped in an electrolyte), connected externally by a wire (through which electrons — and hence current — flow) and internally by a salt bridge (which completes the circuit and maintains electrical neutrality by allowing ion flow).

Example

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