If E^∘(Fe^2+ / Fe)=-0.441 V and E^0(Fe^2+ / Fe^2+)=0.771 V, the standard emf of the reaction F

Step 1:u000AFirst, letu0027s identify the halfu002Dreactions from the given standard reduction potentials:u000Au002D

If E^∘(Fe^2+ / Fe)=-0.441 V and E^0(Fe^2+ / Fe^2+)=0.771...

If $E^{\circ}\left(\mathrm{Fe}^{2+} / \mathrm{Fe}\right)=-0.441 \mathrm{~V}$ and $E^0\left(\mathrm{Fe}^{2+} / \mathrm{Fe}^{2+}\right)=0.771 \mathrm{~V}$, the standard emf of the reaction $\mathrm{Fe}+2 \mathrm{Fe}^{3+} \longrightarrow 3 \mathrm{Fe}^{3+}$ will be (a) 1.212 V (b) 0.111 V (c) 0.330 V (d) 1.653 V

If $E^{\circ}\left(\mathrm{Fe}^{2+} / \mathrm{Fe}\right)=-0.441 \mathrm{~V}$ and $E^0\left(\mathrm{Fe}^{2+} / \mathrm{Fe}^{2+}\right)=0.771 \mathrm{~V}$, the standard emf of the reaction
$\mathrm{Fe}+2 \mathrm{Fe}^{3+} \longrightarrow 3 \mathrm{Fe}^{3+}$ will be
(a) 1.212 V
(b) 0.111 V
(c) 0.330 V
(d) 1.653 V

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Key Concepts

Standard Electrode Potentials

Standard electrode potentials are measures of the intrinsic tendency of a chemical species to be reduced, measured under standard conditions relative to the standard hydrogen electrode. These potentials are fundamental in predicting the direction of redox reactions and determining the feasibility of electrochemical processes.

Half-Cell Reactions

Half-cell reactions represent the individual oxidation and reduction processes that occur during a redox reaction. Each half-reaction is associated with a standard electrode potential, and by analyzing these, one can deduce which species undergoes oxidation and which reduction.

Electrochemical Cell EMF Calculation

The electromotive force (EMF) of an electrochemical cell is calculated by taking the difference between the cathode and anode potentials. This difference indicates the driving force for the redox reaction, and a positive EMF signifies a spontaneous process under standard conditions.

Balancing Redox Reactions

Balancing redox reactions involves ensuring that the total number of electrons lost in the oxidation half-reaction equals the total number of electrons gained in the reduction half-reaction. This is crucial for correctly combining the half-reactions and accurately predicting the overall cell potential.

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