. 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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