A voltaic cell that uses the reaction PdCl₄^2-(aq) + Cd(s) → Pd(s) + 4 Cl^-(aq) + Cd²⁺(aq) has a measured standard cell potential of +1.03 V. (a) Write the two half-cell reactions.

검증된 단계별 안내

Identify the oxidation and reduction components of the overall reaction. In this case, PdCl4^2- is reduced to Pd, and Cd is oxidized to Cd^2+.

Write the reduction half-reaction. Since PdCl4^2- is reduced to Pd, the palladium ion gains electrons. The equation will show the reduction of PdCl4^2- to Pd with the release of Cl^- ions.

Balance the reduction half-reaction for atoms other than hydrogen and oxygen. Ensure that the number of Pd and Cl atoms are equal on both sides of the equation.

Write the oxidation half-reaction. Since Cd is oxidized to Cd^2+, the cadmium metal loses electrons. The equation will show Cd transforming into Cd^2+.

Balance the oxidation half-reaction for atoms and charge. Ensure that the number of Cd atoms and the overall charge are equal on both sides of the equation.

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주요 개념

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Half-Cell Reactions

Half-cell reactions represent the oxidation and reduction processes occurring in a voltaic cell. Each half-cell reaction shows the transfer of electrons, with one species being oxidized (losing electrons) and another being reduced (gaining electrons). In the given reaction, identifying the species that undergo oxidation and reduction is essential for writing the half-cell reactions.

Standard Cell Potential

The standard cell potential (E°) is the measure of the voltage produced by a voltaic cell under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It indicates the driving force behind the electrochemical reaction, with positive values suggesting a spontaneous reaction. Understanding how to interpret and calculate standard cell potentials is crucial for analyzing the overall cell reaction.

Electrochemical Series

The electrochemical series is a list of standard electrode potentials for various half-reactions, arranged from the most positive to the most negative. This series helps predict the direction of electron flow in a voltaic cell and the feasibility of reactions. By comparing the standard potentials of the half-reactions involved, one can determine which species will be oxidized and which will be reduced in the cell.

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (a) Write the two half-cell reactions.