. Calculate the standard cell potentials of galvanic cell in
which the following reactions take place:
(i) 2Cr(s) + 3Cd2+(ab) → 2Cr3+ (ab) + 3 Cd
(ii) Fe2+(ab) + Ag+ (ab) → Fe3+ (ab) + Ag(s) Calculate the Δ r Gº
and equilibrium constant of the reactions
Best Answer
Explanation:
Now, ∆ rG° = - n FE°cell
= - (1 mol) (96500 C/mol) (+0.03 V)
= - 2.895 kJ
Also, ∆r G° = - 2.303 R T log Kc -2.895 kJ
= - 2.303 (8.314 Jk-1) (298 K) log Kc
Log Kc = 0.5074
Kc = 3.22
Final Answer:
Standard cell potential (E°cell) = + 0.34 V
∆ rG° = - 196.86kJ
(1) Equilibrium constant (Kc) = 3.17 × 1034
Standard cell potential (E°cell) = + 0.03 V
∆ rG° = - 2.895kJ
(2) Equilibrium constant (Kc) = 3.22
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