To make E cell of the following concentration cell positive, what should be the relative concentration? Pt | Cl₂(1 atm) | Cl⁻(c₁) || Cl⁻(c₂) | Cl₂(1 atm) | Pt

Question

To make E cell ​ of the following concentration cell positive, what should be the relative concentration? Pt | Cl₂(1 atm) | Cl⁻(c₁) || Cl⁻(c₂) | Cl₂(1 atm) | Pt

TestHub · Accepted Answer

For the following electrochemical cell:

Pt | Cl₂ (1 atm) | Cl⁻ (c₁) || Cl⁻(c₂) | Cl₂ (1 atm) | Pt,

the half-cell reactions are:

Anode: Cl⁻ → $\frac{1}{2}$ Cl₂(g) + e⁻

Cathode: $\frac{1}{2}$ Cl₂ + e⁻ → Cl⁻

The $E_{ce ll}$ is given by:

$E_{ce ll} = - 0.059 lo g \frac{[ C l ^{-} ] _{c}}{[ C l ^{-} ] _{a}} = - 0.059 lo g \frac{c _{2}}{c _{1}} = 0.059 lo g \frac{c _{1}}{c _{2}}$

For the $E_{ce ll}$ to be positive, $c_{1} > c_{2}$ .

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