For a cell given below [2002] Ag |Ag^+ Cu^2+ iCu - + Ag^++e^- ⟶ Cu^

step 1 Here in this question, an oxide is electrolyzed at 1000 degrees Celsius to furnish aluminum meta

For a cell given below [2002] Ag |Ag^+ Cu^2+ iCu ...

For a cell given below [2002] $$ \begin{aligned} & \mathrm{Ag} \mid \mathrm{Ag}^{+} \| \mathrm{Cu}^{2+} \mathrm{iCu} \\ & - \\ & + \\ & \mathrm{Ag}^{+}+\mathrm{e}^{-} \longrightarrow \\ & \mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Ag}, E^{\circ}=\mathrm{x} \\ & \mathrm{Cu}, E^{\circ}=\mathrm{y} \end{aligned} $$ $E_{\text {cell }}^0$ is (a) $x+2 y$ (b) $2 x+y$ (c) $y-x$ (d) $y-2 x$

For a cell given below
[2002]

$$
\begin{aligned}
& \mathrm{Ag} \mid \mathrm{Ag}^{+} \| \mathrm{Cu}^{2+} \mathrm{iCu} \\
& - \\
& + \\
& \mathrm{Ag}^{+}+\mathrm{e}^{-} \longrightarrow \\
& \mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Ag}, E^{\circ}=\mathrm{x} \\
& \mathrm{Cu}, E^{\circ}=\mathrm{y}
\end{aligned}
$$

$E_{\text {cell }}^0$ is
(a) $x+2 y$
(b) $2 x+y$
(c) $y-x$
(d) $y-2 x$

Key Concepts

Cell Potential Calculation

The overall cell potential (E°cell) is calculated by taking the difference between the reduction potential of the cathode (site of reduction) and the oxidation potential of the anode (site of oxidation). This calculation may involve multiplying the electrode potentials by stoichiometric coefficients from the balanced half-reactions, ensuring that electron transfer is balanced before determining the net voltage.

Cell Notation

Cell notation is a shorthand method to represent the components of an electrochemical cell, showing the two half-cells separated by a double vertical line. The notation lists the substances in order of decreasing chemical potential, with phase boundaries indicated by vertical lines and the salt bridge represented by the double line.

Half-Reactions

Half-reactions are the separate oxidation and reduction processes that occur at the anode and cathode of an electrochemical cell. Each half-reaction is written to show either the loss of electrons (oxidation) or the gain of electrons (reduction), and their individual electrode potentials are used to determine the cell's overall voltage.

Electrochemical Cells

Electrochemical cells are systems that convert chemical energy into electrical energy (or vice versa) through redox reactions occurring in spatially separated regions. They consist of two electrodes – one where oxidation occurs and one where reduction occurs – connected by an external circuit and usually a salt bridge or porous partition to maintain charge neutrality.

Standard Electrode Potentials

Standard electrode potentials are measures of the intrinsic tendency of a chemical species to be reduced under standard conditions (1 M concentration, 1 atm pressure, and 25°C). These values, typically given in volts, serve as a basis for predicting the direction of redox reactions and for calculating the overall cell potential.

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