An voltaic cell was set up in which one half-cell had a silver metal electrode s

Question

An voltaic cell was set up in which one half-cell had a silver metal electrode suspended in AgNO_3(aq) The second half-cell contained a nickel metal electrode that was suspended in NiCl2(aq). The standard reduction potentials at 25 degree C are Ae^1+(aq) + le rightarrow Ag(s) E degree red = +0.80V Ni^2+ (aq) + 2e' rightarrow Ni(s) E degree red = -0.28 V Write the chemical equation for the reaction occurring at the anode. Write the chemical equation for the reaction occurring at the cathode. Determine the standard cell potential for this electrochemical cell. Write the balanced chemical reaction for this electrochemical cell.

Explanation / Answer

From the data of reduction potentials given ,Ag+ is having more reduction potential thanNi+2 and as a results Ag+ gets reduced and oxidation of Ni takes place

(Cathode reaction) reduction: Ag+ + e- ==> Ag . . .Eo = +0.80 V   (1)
( Anode reaction ) oxidation: Ni ==> Ni2+ + 2e- . .Eo = +0.23 V   (2)

Cell potential

Multiply Eq.1 by 2 gives  

2Ag+ + 2e--   --à 2Ag Eo =0.80V (3)

Ni--à Ni+2 +2e- E0= 0.23V (2)

Addition of (3) and (2) gives

2Ag+ + Ni ---à 2Ag+ Ni+2 Eo =0.80 +0.23 =1.03V

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.