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E^@ values of N^(2+), Ni and Cl(2), Cl^(...

`E^@` values of `N^(2+), Ni and Cl_(2), Cl^(-)` are respectively `-0.25 V and +1.37 V`. Calculate the EMF of the cell, `Ni , Ni^(2+) (0.01M)"//"Cl^(-)(0.1M), Cl_(2),Pt`.

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To calculate the EMF of the cell given the standard electrode potentials and the concentrations of the solutions, we can follow these steps: ### Step 1: Identify the half-reactions and their standard electrode potentials (E°) The half-reactions and their standard electrode potentials are: - For Nickel (Ni): \[ \text{Ni}^{2+} + 2e^- \rightarrow \text{Ni} \quad E^\circ = -0.25 \, \text{V} \] ...
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