A voltaic cell whose cell reaction is
`2Fe^(3+)(aq) + Zn(s) = 2Fe^(2+)(aq) + Zn^(2+) (aq)`
has an e.m.f. of 0.72 V. What is the maximum electrical work that can be obtained from the cell per mole of Fe (II) ion?

Explanation

To determine the maximum electrical work that can be obtained from the voltaic cell per mole of Fe(II) ion, we can use the relationship between the electromotive force (e.m.f.) of the cell and the work done. The maximum work (W) done by the cell can be calculated using the equation:

\[ W = n \cdot F \cdot E_{cell} \]

Where:
- \( W \) = maximum work (in joules)
- \( n \) = number of moles of electrons transferred in the reaction
- \( F \) = Faraday's constant (approximately \( 96485 \, C/mol \))
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