Calculate the standard cell potentials of galvanic cell in whiCHM the following reactions take place `:` `a. Cr(s) +3Cd^(2+)(aq) rarr 2Cr^(3+)(aq)+3Cd

Question

Calculate the standard cell potentials of galvanic cell in whiCHM the following reactions take place : a.Cr(s)+3Cd2+(aq)→2Cr3+(aq)+3Cd b.Fe2+(aq)+Ag⊕(aq)→Fe3+(aq)+Ag(s) Calculate the ΔrGc- and equilibrium constant of the reactions . Select the correct answer from above options

Answer 1

Correct Answer - a.ΔrGc-=-196.86kJmol-1,Kc=3.192×1034 b.ΔrGc-=-2.895kJmol-1,Kc=3.22 a. E c- cell =E c- cathode -E c- anode =-0.40V-(-0.74)=+0.34V ΔrGc-=-nFE c- cell =-6mol×96400Cmol-1×0.34V =-196860Jmol-1=-196.86kJmol-1 ΔrGc-=--2.303RTlogK 196860=2.303×8.314×298logK logK=34.5014 K=Antilog(34.5014)=3.192×1034 b . Ec- _(cell)=+0.80V-0.77V=+0.03V ΔrGc-=-nFE c- cell =-(1mol)×(96500Cmol-1)×(0.03V) =-2895Jmol-1ΔrGc-=-2.303RTlogK -2895=-2.303×8.314×298×logK or log K=0.5074 or K=Anitlog(0.5074)=3.22