The chemical reaction, 2AgCl(s) H2(g) 2HCl(aq) 2Ag(s) taking pla galvanic cell is represented by the notation [AIIMS-2005 A. Pt(s) H2(g). 1bar | 1MKCl(aq) | AgCl(s) | Ag(s) Pt(s)|H₂(g). 1bar | 1MKC(aq) | 1M Ag(s) | Ag(s) C. D. Pt(s) H2(g). 1bar | 1MHCl(aq) | AgCl(s) | Ag(s) Pt(s) H2(g). 1bar | 1MHCl(aq) | Ag(s) | AgCl(s Explain with proper notation and how to represent cell?

Question

Answer

To represent the given chemical reaction in a galvanic cell, we need to write the notation using the standard notation format. The standard notation format consists of two half-cells, separated by a double vertical line. The anode (oxidation half-reaction) is written on the left side of the double vertical line, and the cathode (reduction half-reaction) is written on the right side. Each half-cell is represented by its respective electrode and the species involved.

The given chemical reaction is:
2AgCl(s) + H2(g) → 2HCl(aq) + 2Ag(s)

The anode half-reaction is the oxidation half-reaction, where AgCl is being oxidized to Ag. The cathode half-reaction is the reduction half-reaction, where H2 is being reduced to form HCl. The overall cell notation is as follows:

[AIIMS-2005]
Anode: Pt(s) | H2(g), 1 bar | 1M KCl(aq) | AgCl(s) | Ag(s)
Cathode: Pt(s) | H2(g), 1 bar | 1M HCl(aq) | Ag(s) | AgCl(s)

Explanation of the notation:

1. Anode:
- The anode consists of a platinum (Pt) electrode.
- The reactant species in the anode half-cell is H2(g), which is at a pressure of 1 bar.
- The electrolyte solution in the anode half-cell is 1M KCl(aq).
- The anode half-cell also contains the solid AgCl(s) and Ag(s) as reactants and products, respectively.

2. Cathode:
- The cathode also consists of a platinum (Pt) electrode.
- The reactant species in the cathode half-cell is H2(g), which is at a pressure of 1 bar.
- The electrolyte solution in the cathode half-cell is 1M HCl(aq).
- The cathode half-cell also contains the solid Ag(s) and AgCl(s) as reactants and products, respectively.

Overall, the galvanic cell consists of two half-cells, the anode and the cathode, connected by a salt bridge or a porous barrier. The anode half-cell undergoes oxidation, releasing electrons into the external circuit, while the cathode half-cell undergoes reduction, accepting the electrons from the external circuit. This flow of electrons generates an electric current.

Note: The given options (A, B, C, and D) are not correct as they do not represent the correct cell notation for the given chemical reaction. The correct notation is the one mentioned above.

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