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For the following cell, Calculate the em...

For the following cell, Calculate the emf:
Al/`Al^(3+)` (0.01M)//`Fe^(2+)`(0.02M)/Fe Given:`E^(@)Al^(+3)`/Al=−1.86V,`E^(@)Fe^(2+)`/Fe =−0.54V.

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AI Generated Solution

To calculate the emf (electromotive force) for the given cell reaction, we can follow these steps: ### Step 1: Identify the Components The cell is given as: \[ \text{Al} | \text{Al}^{3+} (0.01 \, M) || \text{Fe}^{2+} (0.02 \, M) | \text{Fe} \] The standard reduction potentials are: - \( E^\circ_{\text{Al}^{3+}/\text{Al}} = -1.86 \, \text{V} \) ...
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