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NCERT Class XII Chemistry
Chapter - Electrochemistry
Questions with Solutions

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Question : 24
Total: 32
The cell in which the following reaction occurs:
2Fe3+(aq)+2I–(aq) –––––▶2Fe2+(aq)+I2(s)‌has‌E°cell=0.236V‌at‌298‌K.Calculate the standard Gibb’s energy and the equilibrium constant of the cell reaction.
Solution:  
2 Fe3++2e−→2 Fe2+
2 I−→I2+2e−
–––––––––––––––––––––––––––––––––––––––
2Fe3++2I−→I2+2Fe2+;E°cell=0.236V
–––––––––––––––––––––––––––––––––––––––
ΔG0=−nE0F
=−2×0.236×96500
=−45548 Jmol−1
=−45.54 kJ mol−1
ΔG0=−2.303RT‌log‌K
log‌K=−
ΔG0
2.303RT

=
−(−45548)
2.303×8.314×298
=7.98
⇒K=9.61×107
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