NCERT Class XII Chemistry
Chapter - Electrochemistry
Questions with Solutions

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Question : 4
Total: 32
Calculate the standard cell potentials of galvanic cell in which the following reactions take place:
(i)2Cr(s)+3Cd2+(aq)2Cr3+(aq)+3Cd(s)
(ii) Fe2+(aq)+Ag+(aq)Fe3+(aq)+Ag(s)
Calculate the ΔrG° and equilibrium constant of the reactions.
Given : E°Cr3+Cr=0.74V,E°Cd2+Cd=0.40V
E°Ag+Ag=0.80V,E°Fe3+Fe2+=0.77V
Solution:  
(i) E°cell=E°cathodeE°anode =0.40V(0.74V)=+0.34V
ΔG°=nFE°cell =6×96500×0.34=196860Jmol1 =196.86kJmol1
ΔG°=2.303RTlogK
196860=2.303×8.314×298×logK or logK=34.5014
K=Antilog34.5014 =3.172×1034
(ii) E°cell = +0.80 V – 0.77 V = +0.03 V
ΔG° = –nFE°cell = – 1 × 96500 × 0.03 = –2895 J mol1 = –2.895 kJ mol1
ΔG°= –2.303 RT log K
–2895 = –2.303 × 8.314 × 298 × log K
or log K = 0.5074
K = Antilog (0.5074) = 3.22
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