The conventional notation for representing galvanic cells is the cell diagram. For the Daniell cell, using `KCl` as the electrolyte in the salt bridge and assuming `1 M` concentration, the cell diagram is

Options

A. `Cu(s)|Cu^(2+)(aq., 1 M)|KCl(sat'd)|Zn^(2+)(aq., 1 M)|Zn(s)`
B. `Zn^(2+)(aq., 1 M)|Z(s)|KCl(sat'd)|Cu^(2+)(aq., 1 M)|Cu(s)`
C. `Zn(s)|Zn^(2+)(aq., 1 M)|KCl(sat'd)|Cu^(2+)(aq., 1 M)|Cu(s)`
D. `Cu^(2+)(aq., 1 M)|Cu(s)|KCl(sat'd)|Zn(s)|Zn^(2+)(aq., 1 M)`

Answer

B

Explanation

To identify the anode half-cell and cathode half-cell we split the cell reaction into half-reactions:
Anode : `(1)/(2) H_(2)(g) hArr H^(+)(aq.) + e^(-)`
Cathode : `AgCl(s) + e^(-) hArr Ag(s)+ Cl^(-) (aq.)`
Overall : `(1)/(2)H_(2)(g)+AgCl(s)hArr H^(+)(aq.)+Ag(s)+Cl^(-)(aq.)`
This implies that anode is the hydrogen has electrode and cathode is the silver-silver chloride-chloride electrode. Both the electrodes are immersed in the same electrolyte, `HCl(aq.)` which provides `H^(+)(aq.)` for the hydrogen gas electrode and `Cl^(-)(aq.)` for the silver-silver chloride-chloride electrode.
In the conventional notation for galvanic cells, the single vertical bars indicate boundaries between phases. The double vertical bar indicates a barrier (salt bridge) that allows the movement of ions but not the mixing of solutions.
By convention, the anode half-cell, wherre oxidation takes place, is on the left, the cathode, where reduction takes place is on the right. Here, we have not used the double vertical bar because both the electrodes have the common electrolyte.