Question

Predict whether the following reaction feasible or not? 

Cu²⁺ (aq) + 2Ag(s) → Cu(s) + 2Ag⁺(aq)

Answer 1

From the electrochemical series, E° values of and Ag are, 

Cu = + 0.34 V 

Ag = + 0.80 V

Since the reduction potential of Ag is more than tha Cu, this means that silver has greater tendency to reduced in comparison to copper. Thus, the reduction of Ag occurs more readily than Cu. This can be represented as:

Ag⁺ (aq) + e → Ag(s)

Since reduction potential of copper is less than silver, it can be easily oxidized as compared to silver as shown below:

Cu(s) → Cu²⁺ (aq) + 2e^-

Therefore, silver will be reduced and copper will be oxidized and above reaction is not feasible.