Two electrochemical cell Zn|Zn^2+ Cu^2+| Cu and Fe|Fe^2+ Cu^2+| Cu are connected in series. Wh

step 1 In this question we have been given two different cells and these cells are ZN to ZN plus 2 and

Two electrochemical cell Zn|Zn^2+ Cu^2+| Cu and Fe|Fe^2+ ...

Two electrochemical cell $\mathrm{Zn}\left|\mathrm{Zn}^{2+} \| \mathrm{Cu}^{2+}\right| \mathrm{Cu}$ and $\mathrm{Fe}\left|\mathrm{Fe}^{2+} \| \mathrm{Cu}^{2+}\right| \mathrm{Cu}$ are connected in series. What will be the net e.m.f. of the cell at $25^{\circ} \mathrm{C}$ ? Given: $\mathrm{Zn}^{2+} \mid \mathrm{Zn}=-0.73 \mathrm{~V}$ $\mathrm{Cu}^{2+} \mid \mathrm{Cu}=+0.34 \mathrm{~V}$ $\mathrm{Fe}^{2+} \mid \mathrm{Fe}=-0.41 \mathrm{~V}$ a. $+1.85$ b. $-1.85 \mathrm{~V}$ c. $+0.83 \mathrm{~V}$ d. $-0.83 \mathrm{~V}$

Two electrochemical cell
$\mathrm{Zn}\left|\mathrm{Zn}^{2+} \| \mathrm{Cu}^{2+}\right| \mathrm{Cu}$ and $\mathrm{Fe}\left|\mathrm{Fe}^{2+} \| \mathrm{Cu}^{2+}\right| \mathrm{Cu}$ are
connected in series. What will be the net e.m.f. of the cell at $25^{\circ} \mathrm{C}$ ?
Given: $\mathrm{Zn}^{2+} \mid \mathrm{Zn}=-0.73 \mathrm{~V}$
$\mathrm{Cu}^{2+} \mid \mathrm{Cu}=+0.34 \mathrm{~V}$
$\mathrm{Fe}^{2+} \mid \mathrm{Fe}=-0.41 \mathrm{~V}$
a. $+1.85$
b. $-1.85 \mathrm{~V}$
c. $+0.83 \mathrm{~V}$
d. $-0.83 \mathrm{~V}$

Key Concepts

Electrochemical Cell

An electrochemical cell is a device in which a spontaneous redox reaction produces an electric current. In these cells, chemical energy is converted into electrical energy through a series of oxidation and reduction reactions occurring in separate compartments, typically involving two electrodes and an electrolyte. The overall reaction is split into two half-reactions that take place at the anode (oxidation) and cathode (reduction).

Standard Electrode Potential

Standard electrode potentials are the voltages associated with specific redox half-reactions measured under standard conditions (25°C, 1 M concentrations, and 1 atm pressure). These potentials are referenced against the standard hydrogen electrode and indicate the tendency of a chemical species to be reduced. They are essential for predicting the direction of electron flow and the spontaneity of redox reactions.

Half-Reactions

Half-reactions describe the individual oxidation and reduction processes in an electrochemical cell. Each half-reaction includes electrons either as products or reactants, which clearly shows how electrons are transferred during the redox process. Understanding half-reactions is crucial in balancing redox equations and calculating the overall cell potential.

Series Connection of Cells

When multiple electrochemical cells are connected in series, the net electromotive force (emf) of the system is obtained by algebraically adding the individual cell potentials. This principle is similar to adding the voltages of batteries in series, taking into account the correct sign (positive for reduction potential at the cathode and negative for oxidation at the anode).

Net EMF Calculation

The net EMF of a combined electrochemical system is determined by the difference between the reduction and oxidation potentials of the individual cell reactions. This involves identifying which electrode undergoes oxidation and which undergoes reduction and then summing the potentials accordingly. The calculated net EMF indicates the overall driving force available for an electric current in the circuit.

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