A galvanic cell is constructed from a Zn/Zn2+ half-cell (anode) and a Cl2/Cl- half-cell (cathode). (c) Give the shorthand notation for the cell.

Verified step by step guidance

Identify the anode and cathode reactions. The anode reaction involves the oxidation of Zn to Zn^{2+}, and the cathode reaction involves the reduction of Cl_2 to Cl^-.

Write the half-reactions for the anode and cathode. The anode half-reaction is Zn \rightarrow Zn^{2+} + 2e^-, and the cathode half-reaction is Cl_2 + 2e^- \rightarrow 2Cl^-.

Determine the direction of electron flow. Electrons flow from the anode to the cathode in a galvanic cell.

Write the cell notation. The anode is written on the left and the cathode on the right, separated by a double vertical line representing the salt bridge.

Combine the components into the shorthand notation: Zn | Zn^{2+} || Cl_2 | Cl^-.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Galvanic Cell

A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells, each containing an electrode and an electrolyte, where oxidation occurs at the anode and reduction occurs at the cathode. The flow of electrons from the anode to the cathode generates an electric current.

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, which indicates the salt bridge or porous barrier. Each half-cell notation includes the metal or gas involved, its ion form, and their respective concentrations, allowing for a clear understanding of the cell's components and reactions.

Standard Electrode Potential

Standard electrode potential is a measure of the tendency of a chemical species to be reduced, measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It is expressed in volts and is crucial for determining the overall cell potential of a galvanic cell. The difference in standard electrode potentials between the anode and cathode indicates the direction of electron flow and the cell's voltage output.

Recommended video:

Guided course

01:27

Standard Cell Potential

Related Practice

Textbook Question

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.

Textbook Question

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (b) Write balanced equations for the electrode and overall cell reactions.

Textbook Question

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.

Textbook Question

Write balanced equations for the electrode and overall cell reactions in the following galvanic cells. Sketch each cell, labeling the anode and cathode and showing the direction of electron and ion flow.(a) .

Textbook Question

What conditions must be met for a cell potential E to qualify as a standard cell potential E°?

views

Textbook Question

Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: Br2(aq), MnO4+(aq), Sn4+(aq).