An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (c) Give the shorthand notation for the cell.

Verified step by step guidance

1. Identify the anode and cathode reactions. The anode is the oxidation half-cell, and the cathode is the reduction half-cell.
2. Write the half-reaction for the anode: \( \text{H}_2(g) \rightarrow 2\text{H}^+(aq) + 2e^- \).
3. Write the half-reaction for the cathode: \( \text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s) \).
4. In the shorthand notation, the anode is written on the left and the cathode on the right, separated by a double vertical line representing the salt bridge.
5. Combine the half-reactions into the shorthand notation: \( \text{Pt} | \text{H}_2(g) | \text{H}^+(aq) || \text{Ag}^+(aq) | \text{Ag}(s) \).

Key Concepts

Electrochemical Cells

Electrochemical cells are devices that convert chemical energy into electrical energy through redox reactions. They consist of two half-cells: an anode where oxidation occurs and a cathode where reduction takes place. The flow of electrons from the anode to the cathode generates an electric current, which can be harnessed for various applications.

Half-Cell Notation

Half-cell notation is a standardized way to represent the components of an electrochemical cell. It typically includes the anode and cathode separated by a double vertical line, indicating the salt bridge. Each half-cell is written with the oxidized form on the left and the reduced form on the right, allowing for a clear understanding of the reactions occurring at each electrode.

Salt Bridge

A salt bridge is a crucial component of electrochemical cells that maintains electrical neutrality by allowing the flow of ions between the two half-cells. It typically contains a gel or solution of an inert electrolyte, which prevents the mixing of the different solutions while enabling the movement of ions. This movement is essential for completing the circuit and sustaining the redox reactions.