Calculate the cell potential of this reaction under standard reaction conditions.?

NetherCraft 0

The standard reduction potentials of lithium metal and chlorine gas are as follows:

Reaction Reduction potential

(V)

Li+(aq)+e−→Li(s) −3.04

Cl2(g)+2e−→2Cl−(aq) +1.36

In a galvanic cell, the two half-reactions combine to

2Li(s)+Cl2(g)→2Li+(aq)+2Cl−(aq)

Calculate the cell potential of this reaction under standard reaction conditions.

ΔG∘=−nFE∘cell

where n is the number of moles of electrons transferred and F=96,500J/V⋅mol e− is the Faraday constant.

1 Answer

  • Reduction takes place at the cathode: Cl2(g) + 2e- =>2Cl-(aq) Eº=+1.36 V

    Oxidation takes place at the anode: Li(s) => Li+(aq) + e- Eº=-3.04 V

    Ecell = Ecathode – Eanode

    Ecell = 1.36 – (-3.04) = 4.4 V

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