Question

Depict the galvanic cell in which the reaction: $Zn(s)+2Ag^{+}(aq) \longrightarrow Zn^{2+}(aq)+2Ag(s)$ takes place. Further show:
(i) which of the electrode is negatively charged.
(ii) the carriers of current in the cell.
(iii) individual reaction at each electrode.

Answer 1

Galvanic cell converts chemical energy into electrical energy and it consists of two half cells, they are anode and cathode.  

The given Galvanic cell representation is as follows.

$Z{ n }_{ (s) }|\quad Z{ n }_{ (aq) }^{ 2+ }\parallel A{ g }_{ (aq) }^{ + }|A{ g }_{ (s) }$

i) Zn electrode is anode because it is negatively charged.

ii) In the cell, current carried by ions, the flow of current from silver to zinc.

iii) The reaction taking place at the anode

$Z{ n }_{ (s) }\quad \rightarrow \quad { Zn }_{ (aq) }^{ 2+ }+\quad 2{ e }^{ - }$

The reaction taking place at the cathode

${ Ag }_{ (aq) }^{ + }+\quad { e }^{ - }\quad \rightarrow \quad { Ag }_{ (s) }$