The standard oxidation potentials of Zn, Cu, Ag and Ni electrodes are +0.76,-0.34,-0.80 and +0.2

step 1 In this question we have been given the standard oxidation potentials for zinc, copper, silver a

The standard oxidation potentials of Zn, Cu, Ag and Ni...

The standard oxidation potentials of $\mathrm{Zn}, \mathrm{Cu}, \mathrm{Ag}$ and Ni electrodes are $+0.76,-0.34,-0.80$ and $+0.25 \mathrm{~V}$ respectively. Which of the following reaction will provide maximum voltage? a. $\mathrm{Zn}+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}$ b. $\mathrm{Cu}+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}$ c. $\mathrm{Zn}+2 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}$ d. $\mathrm{Zn}+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}$

The standard oxidation potentials of $\mathrm{Zn}, \mathrm{Cu}, \mathrm{Ag}$ and Ni electrodes are $+0.76,-0.34,-0.80$ and $+0.25 \mathrm{~V}$ respectively. Which of the following reaction will provide maximum voltage?
a. $\mathrm{Zn}+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}$
b. $\mathrm{Cu}+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}$
c. $\mathrm{Zn}+2 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}$
d. $\mathrm{Zn}+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}$

Key Concepts

Galvanic Cells

A galvanic cell is an electrochemical cell that converts the energy released from spontaneous redox reactions into electrical energy. The choice of electrodes, based on their standard potentials, directly affects the voltage output of the cell. Maximizing the cell potential involves pairing electrodes with the greatest difference in their tendency to be oxidized or reduced.

Half-Cell Reactions

Half-cell reactions separate the overall redox process into two parts: one for oxidation and one for reduction. Each half-cell has its own electrode potential, and these individual potentials are used to calculate the overall cell potential, which determines the maximum voltage available from the reaction.

Cell Potential Calculation

The overall cell potential of an electrochemical cell is determined by combining the electrode potentials of the two half-cells. Typically, it is calculated by taking the difference between the reduction potential at the cathode and the oxidation potential at the anode. A larger difference indicates a higher possible voltage output from the cell.

Standard Electrode Potentials

Standard electrode potentials are values that describe the intrinsic tendency of a chemical species to lose or gain electrons under standard conditions. They provide a baseline for comparing the relative strengths of oxidizing and reducing agents, and are essential for predicting the direction and feasibility of redox reactions.

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between chemical species. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding redox reactions is key to analyzing how and why electrons move in electrochemical cells.

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