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Question

(a) The cell in which the following reaction occurs:
2Fe3+(aq)+2I(aq)2Fe2+(aq)+I2(s) has Ecell=0.236V at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C mol1)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C mol1)

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Solution

(a) The two half cell reactions for the cell are:
2Fe3+(aq)+2e2Fe2+ (Reduction)
2II2+2e (Oxidation)
No. of electrons transferred = 2
ΔG=n F Ecell
=2×96500×0.236
=45.55 kJ

(b) Q=I×t=0.5×2×60×60=3600C
No. of electrons flowing through wire on passing charge of 1F=6.023×1023
No. of electrons flowing through wire on passing charge of 3600 C=6.022×1023×360096500
=2.246×1022

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