The value of E^$\circ$_cell for an aluminum-nickel electrochemical cell is +1.41 V at 25^$\circ$C. The value of K^$\circ$ for this cell under standard conditions is

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The Nernst equation relates the cell potential to the standard cell potential and the reaction quotient. For a cell under standard conditions, the reaction quotient Q = 1, and the cell potential equals the standard cell potential. The equation that relates the standard cell potential ($E^\circ$) to the equilibrium constant ($K$) is given by $E^\circ = \frac{RT}{nF} \ln K$, where $R$ is the gas constant, $T$ is the temperature in Kelvin, $n$ is the number of moles of electrons transferred in the reaction, and $F$ is Faraday's constant. A positive value of $E^\circ$ indicates a spontaneous reaction, which corresponds to a large equilibrium constant ($K$). Since the given $E^\circ$ is +1.41 V, which is significantly positive, it implies that $K$ is much greater than 1, suggesting that the equilibrium lies far to the right, favoring the products. Therefore, the value of $K$ is >>100.

The Value of E ∘\circ∘ cell for an Aluminum-Nickel Electrochemical Cell Is +1

The Value of E^$\circ$_cell for an Aluminum-Nickel Electrochemical Cell Is +1