Question

(a) Why is it impossible to measure the standard reduction potential of a single half-reaction? (b) Describe how the standard reduction potential of a half-reaction can be determined.

Short answer

(a) It is impossible to measure the standard reduction potential of a single half-reaction because a redox reaction requires both reduction and oxidation processes to occur simultaneously. Additionally, potential measurements involve comparing the half-reaction of interest to a reference half-reaction, such as the standard hydrogen electrode. (b) To determine the standard reduction potential of a half-reaction, set up an electrochemical cell that includes the half-reaction of interest and the standard hydrogen electrode. Connect them with a salt bridge and measure the cell potential using a voltmeter. Under standard conditions, the measured cell potential represents the standard reduction potential of the half-reaction of interest.

Step-by-step solution

(a) Impossibility of Measuring Single Half-Reaction

In electrochemistry, a half-reaction involves either reduction (gain of electrons) or oxidation (loss of electrons). Standard reduction potential is a measure of the tendency of a species participating in a half-reaction to gain electrons and undergo reduction. The main reason it is impossible to measure the standard reduction potential of a single half-reaction is that it's incomplete; a redox reaction needs both a reduction and an oxidation process to take place simultaneously. In other words, electrons cannot be gained without an accompanying loss of electrons, so single half-reactions cannot happen in isolation. Moreover, when measuring potential, we compare the potential of the half-reaction of interest to that of a reference half-reaction, such as the standard hydrogen electrode, which has an assigned potential of 0 volts. Due to these reasons, it is impossible to measure the standard reduction potential of a single half-reaction.

(b) Determining the Standard Reduction Potential of a Half-Reaction

To determine the standard reduction potential of a half-reaction, we need to set up an electrochemical cell that includes the half-reaction of interest along with a reference half-reaction. The most common reference half-reaction is the standard hydrogen electrode. The standard hydrogen electrode consists of a platinum electrode immersed in a solution of H⁺ ions (with an activity of 1) and exposed to hydrogen gas at a pressure of 1 atm. Here are the steps to determine the standard reduction potential of a half-reaction: 1. Set up an electrochemical cell that includes the half-reaction of interest and the standard hydrogen electrode. 2. Connect the two half-cells with a salt bridge, which maintains charge neutrality by allowing the flow of ions between the two half-cells. 3. Measure the voltage (cell potential) across the two electrodes using a voltmeter. Under standard conditions (1 M concentration of all species involved, temperature of 298 K, and pressure of 1 atm), this voltage represents the difference in standard reduction potential between the half-reaction of interest and the standard hydrogen electrode. 4. The standard reduction potential of the half-reaction of interest is equal to the measured cell potential of the electrochemical cell since the standard hydrogen electrode has a reduction potential of 0 volts.

Key concepts

Half-Reaction

A half-reaction is a crucial component in the study of electrochemical processes. Half-reactions focus on the behavior of electrons in a chemical reaction, highlighting either the gain or loss of electrons. Essentially, they break down a full redox (reduction-oxidation) reaction into two distinct parts: oxidation half-reaction and reduction half-reaction.

• Oxidation Half-Reaction: Involves the loss of electrons. An oxidizing agent is responsible for accepting these electrons.
• Reduction Half-Reaction: Involves the gain of electrons. A reducing agent is responsible for donating these electrons.

By investigating half-reactions, scientists can better understand how electrons are transferred in a redox reaction. This helps measure key properties like standard reduction potential, which is an important measurement indicating a chemical species' tendency to gain electrons.

Electrochemical Cell

An electrochemical cell is an essential apparatus for studying electrochemical reactions. It allows the separation of oxidation and reduction processes to harness the flow of electrons as electrical energy.

• Two Half-Cells: An electrochemical cell consists of two half-cells, each containing a different half-reaction. These are generally composed of a metal electrode immersed in a solution of its ions.
• Salt Bridge: The half-cells are connected by a salt bridge, a device that enables ions to move between solutions, thereby maintaining electrical neutrality.
• Cell Potential: The potential difference between the two electrodes when connected forms the cell potential. This voltage is the key measurement used to compare the standard reduction potentials of half-reactions.

Electrochemical cells not only provide a direct way to measure the potential difference of half-reactions but also have practical applications in batteries and electroplating.

Standard Hydrogen Electrode

The standard hydrogen electrode (SHE) is used as a reference in measuring electrode potentials. It serves as the baseline with a reduction potential defined as exactly 0 volts, against which other half-reactions are measured.

• Components: The SHE consists of a platinum electrode in contact with hydrogen gas at 1 atm pressure, immersed in a 1 mol/L solution of H⁺ ions.
• Reference Electrode Role: As a reference, it allows scientists to compare the reduction potential of various half-reactions under consistent conditions, typically 298 K and a pressure of 1 atm.
• Significance in Electrochemistry: The SHE's reproducibility and standardized conditions make it crucial for determining the standard reduction potentials of other substances.

In practice, the standard hydrogen electrode ensures that potential measurements are consistent and comparable across different experiments and conditions.

Redox Reaction

Redox reactions, short for reduction-oxidation reactions, are chemical processes where electrons are transferred between two substances. These reactions are the foundation of electrochemical cells and are crucial in a variety of natural and industrial processes.

• Reduction: Involves gaining electrons, decreasing oxidation state. The species that gains electrons is reduced.
• Oxidation: Involves losing electrons, increasing oxidation state. The species that loses electrons is oxidized.

Redox reactions maintain the balance of charge in an electrochemical cell. These processes enable the conversion of chemical energy into electrical energy, highlighting their importance not just in theory but in practical applications like energy storage and production. Through the understanding of redox reactions, scientists and engineers can design more efficient systems such as fuel cells and rechargeable batteries.