A galvanic cell Mn() Mn2 (aq) | Ni(aq)/Nis) is constructed using a completely im

Question

A galvanic cell Mn() Mn2 (aq) | Ni(aq)/Nis) is constructed using a completely immersed Ma electrode that weighs 35.1 g and a Ni electrode immersed in 430 ml of 1.00 M Ni2+(aq) solution. A steady current of 0.0505 A is drawn from the cell as the electrons move from the Mn electrode to the Ni electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Ni electrode gained when the cell is completely discharged? d what is the concentration of the Ni2 aq when the cell is completely discharged? (Assume that the limiting reactant is io% reacted) Ar

Explanation / Answer

For the given electrochemical cell

(a) moles Mn = 35.1 g/54.94 g/mol = 0.640 moles

moles Ni2+ = 1.0 M x 0.430 L = 0.430 moles

limiting reactant = Ni2+

(b) moles electron used = 0.430 moles x 2 = 0.860 mol e-

coulombs charge needed = 0.860 mole e- x 96485 = 82977.1 C

time required for compete discharge = 82977.1/0.0505 A = 1643111 s

(c) mass of Ni electrode when complete discharge = 0.430 moles x 58.7 g/mol = 25.241 g

(d) Concentration of Ni2+ when the cell is completely discharged = 0.0 M

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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