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Answer the following in brief. Construct a galvanic cell from the electrodes Co3+ | Co and Mn2+/Mn. E⁢∘Co = 1.82 V, E⁢∘Mn = –1.18 V. Calculate E⁢∘cell - Chemistry

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प्रश्न

Answer the following in brief.

Construct a galvanic cell from the electrodes Co3+ | Co and Mn2+/Mn. \[\ce{E{^{\circ}_{Co}}}\] = 1.82 V, \[\ce{E{^{\circ}_{Mn}}}\] = –1.18 V. Calculate \[\ce{E{^{\circ}_{cell}}}\]

संक्षेप में उत्तर
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उत्तर

Given:

\[\ce{E{^{\circ}_{Co}}}\] = 1.82 V, 

\[\ce{E{^{\circ}_{Mn}}}\] = –1.18 V.

To find: \[\ce{E{^{\circ}_{cell}}}\] and cell representation

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

Calculation: Electrode reactions are

At anode: \[\ce{3(Mn_{(s)} -> Mn{^{2+}_{(aq)}} + 2e-}\]

At cathode: \[\ce{2(Co{^{3+}_{(aq)}} + 3e- -> Co_{(s)})}\]

The cell is composed of Mn (anode), Mn(s) \[\ce{Mn{^{2+}_{(aq)}}}\] and Co (cathode), \[\ce{Co{^{3+}_{(aq)}} | Co_{(s)}}\]

The cell is represented as:

\[\ce{Mn_{(s)} | Mn{^{2+}_{(aq)}} || Co{^{3+}_{(aq)}} | Co_{(s)}}\]

The standard electrode potential is given by

\[\ce{E{^{\circ}_{cell}} = E{^{\circ}_{cathode}} - E{^{\circ}_{anode}}}\]

= 1.82 V – (–1.18 V)

= 1.82 V + 1.18 V

= 3.00 V

The standard cell potential is 3.00 V.

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Electrode Potential and Cell Potential
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अध्याय 5: Electrochemistry - Exercises [पृष्ठ ११८]

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बालभारती Chemistry [English] Standard 12 Maharashtra State Board
अध्याय 5 Electrochemistry
Exercises | Q 3.05 | पृष्ठ ११८

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