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For the given cell Fe2+(aq) + Ag+(aq) → Fe3+(aq) and Ag(s) The standard cell potential of the above reaction is Given : Ag+ + e− → Ag E° = x V Fe2+ + 2e− → Fe E° = y V Fe3+ + 3e− → Fe E° = z V

1. x + y − z
2. x + 2y − 3z
3. y − 2x
4. x + 2y

Correct answer: x + 2y − 3z

Solution

The standard cell potential is calculated using the reduction potentials of the half-reactions involved. In this case, Ag+ is reduced to Ag (gaining one electron) and Fe2+ is oxidized to Fe3+ (losing two electrons), which leads to the equation x + 2y - 3z, accounting for the stoichiometry of the electrons transferred.

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