# Answer the following in brief. Construct a galvanic cell from the electrodes Co3+ | Co and Mn2+| Mn.ECo∘ = 1.82 V, EMn∘ = - 1.18 V. Calculate Ecell∘ - Chemistry

Construct a galvanic cell from the electrodes Co3+ | Co and Mn2+| Mn.
"E"_"Co"^circ = 1.82 V, "E"_"Mn"^circ = - 1.18 V. Calculate "E"_"cell"^circ

#### Solution

Given:

"E"_"Co"^circ = 1.82 V,

"E"_"Mn"^circ = - 1.18 V.

To find: "E"_"cell"^circ and cell representation

Formulae: "E"_"cell"^circ = "E"_"Cathode"^circ - "E"_"anode"^circ

Calculation: Electrode reactions are

At anode: 3("Mn"_(("s")) -> "Mn"_(("aq"))^(2+) + 2"e"^-)

At cathode: 2("Co"_(("aq"))^(3+) + 3"e"^(-) -> "Co"_(("s")))

The cell is composed of Mn (anode), Mn(s) |"Mn"_(("aq"))^(2+) and "Co" ("cathode"), "Co"_(("aq"))^(3+)| "Co"_(("s"))

The cell is represented as:

"Mn"_(("s")) |"Mn"_(("aq"))^(2+)| |"Co"_(("aq"))^(3+)|  "Co"_(("s"))

The standard electrode potential is given by

"E"_"cell"^circ = "E"_"Cathode"^circ - "E"_"anode"^circ

= 1.82 V - (- 1.18 V)

= 3.00 V

The standard cell potential is 3.00 V.

Concept: Electrode Potential and Cell Potential
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#### APPEARS IN

Balbharati Chemistry 12th Standard HSC for Maharashtra State Board
Chapter 5 Electrochemistry
Exercise | Q 3.05 | Page 118