What is the reduction potential of Cl⁻(aq)?
Final answer: The reduction potential of Cl⁻(aq) is -1.36 V.
Explanation:
The reduction potential of Cl⁻(aq) is -1.36 V, which represents the potential change when chloride ions are oxidized to chlorine gas under standard conditions. The standard reduction potential of an ion is the potential difference that makes the ion undergo reduction at the standard conditions. In the case of chloride ions (Cl⁻), the reduction potential usually found in standard reduction potential tables is for its reverse reaction, 'Cl2 + 2e- -> 2Cl-', where chlorine gas is reduced to chloride ion. Its potential is +1.36 V. However, we are looking at the reverse reaction where Cl⁻ is going to Cl2, which would actually be an oxidation process. Thus, we need to change the sign of the potential, so the reduction potential of Cl⁻(aq) is -1.36 V.
Understanding Reduction Potential
Reduction potential (E°) is a measure of how easily a species gains electrons in a redox reaction. It is a fundamental concept in electrochemistry and is used to predict the direction in which redox reactions will occur. The more positive the reduction potential of a species, the greater its tendency to gain electrons and be reduced.
Standard Conditions: The reduction potential values are always given under standard conditions, which typically include a concentration of 1 M, a pressure of 1 atm, and a temperature of 25°C.
Specific Example: In the case of Cl⁻(aq), the reduction potential of -1.36 V indicates that chloride ions have a strong tendency to be oxidized to chlorine gas in a redox reaction. This means that in a system where Cl⁻(aq) is present, it is likely to undergo oxidation and lose electrons to become Cl2.
Sign Convention: When looking at a standard reduction potential table, it's important to identify the direction of the reaction you are interested in. In the case of Cl⁻(aq), the relevant reaction is its oxidation to form Cl2, which requires changing the sign of the potential from the standard reduction potential value.
By understanding reduction potential, we can predict the behavior of species in redox reactions and design electrochemical systems for various applications.