Question

With the help of the electro-chemical series, check the feasibility of the redox reaction: $Ni(s)+2Ag^{+}(aq) \longrightarrow Ni^{2+}(aq)+2Ag(s)$

Answer 1

Electrochemical series is an arrangement of various redox equilibria in the order of their electrode potential.

If a metal (A) is above another metal (B) in the electrochemical series then it can easily reduce $B^+$ ions to metal B by releasing electrons.

E⁰$Ni^{2+}/Ni= - 0.25 V$ and E⁰$Ag^+/Ag= - 0.80 V$

$Ni(s)+2Ag^+(aq)\rightarrow Ni_2+(aq)+2Ag(s)$

The E⁰ values indicate that Ni (A) is above Ag (B) in electrochemical series and hence the given redox reaction is feasible.

Answer 2

If a metal (A) is above another metal (B) in the electrochemical series then it can easily reduce B^+B+ions to metal B by releasing electrons.

E⁰Ni^{2+}/Ni= - 0.25 VNi2+/Ni=−0.25V and E⁰Ag^+/Ag= - 0.80 VAg+/Ag=−0.80V

Ni(s)+2Ag^+(aq)\rightarrow Ni_2+(aq)+2Ag(s)Ni(s)+2Ag+(aq)→Ni2​+(aq)+2Ag(s)

The E⁰ values indicate that Ni (A) is above Ag (B) in electrochemical series and hence the given redox reaction is feasible.