Give the symbolic representation of the galvanic cell obtained by using the following standard reduction potentials at $298 \ K$ and calculate its standard cell potential $(E^o_{cell})$.
$(i)$ $E^o_{Ag^{+}|Ag} = 0.80 \ V$
$(ii)$ $E^o_{Zn^{2+}|Zn} = -0.76 \ V$

(N/A) In a galvanic cell,the electrode with the lower reduction potential acts as the anode (oxidation) and the electrode with the higher reduction potential acts as the cathode (reduction).
Here,$E^o_{Zn^{2+}|Zn} = -0.76 \ V$ (lower) and $E^o_{Ag^{+}|Ag} = 0.80 \ V$ (higher).
Therefore,$Zn$ acts as the anode and $Ag$ acts as the cathode.
The symbolic representation of the cell is: $Zn(s) | Zn^{2+}(aq) || Ag^{+}(aq) | Ag(s)$.
The standard cell potential is calculated as:
$E^o_{cell} = E^o_{cathode} - E^o_{anode}$
$E^o_{cell} = E^o_{Ag^{+}|Ag} - E^o_{Zn^{2+}|Zn}$
$E^o_{cell} = 0.80 \ V - (-0.76 \ V)$
$E^o_{cell} = 0.80 \ V + 0.76 \ V = 1.56 \ V$.