For a cell reaction: Mn+(aq)+ne- → M(s), the Nernst equation for electrode potential at any concentration measured with respect to standard hydrogen electrode is represented as

Question

For a cell reaction: Mn+(aq)+ne- → M(s), the Nernst equation for electrode potential at any concentration measured with respect to standard hydrogen electrode is represented as (A) E(Mn+/M)=E°(Mn+/M)-(RT/nF)ln (1/[Mn+]) (B) E(M/Mn+)=E°(M/Mn+)-(RT/nF)ln ([Mn+]/[M]) (C) E(Mn+/M)=E°(Mn+/M)-(RT/nF)log (1/[M]) (D) E(Mn+/M)=E°(Mn+/M)-(RT/nF)ln [Mn+]

Tardigrade Admin · Accepted Answer

Correct answer is (a) E(Mn+/M)=E°(Mn+/M)-(RT/nF)ln (1/[Mn+])

Q. For a cell reaction : $M_{(a q)}^{n +} + n e^{-} \to M_{(s)}$ , the Nernst equation for electrode potential at any concentration measured with respect to standard hydrogen electrode is represented as

$E_{(M^{n +} / M)} = E_{(M^{n +} / M)}^{\circ} - \frac{RT}{n F} l n \frac{1}{[ M ^{n +} ]}$

$E_{(M / M^{n +})} = E_{(M / M^{n +})}^{\circ} - \frac{RT}{n F} l n \frac{[ M ^{n +} ]}{[ M ]}$

$E_{(M^{n +} / M)} = E_{(M^{n +} / M)}^{\circ} - \frac{RT}{n F} l o g \frac{1}{[ M ]}$

$E_{(M^{n +} / M)} = E_{(M^{n +} / M)}^{\circ} - \frac{RT}{n F} l n [M^{n +}]$

Correct answer is (a) $E_{(M^{n +} / M)} = E_{(M^{n +} / M)}^{\circ} - \frac{RT}{n F} l n \frac{1}{[ M ^{n +} ]}$

Q. For a cell reaction : M(aq)n+​+ne−→M(s)​, the Nernst equation for electrode potential at any concentration measured with respect to standard hydrogen electrode is represented as

E(Mn+/M)​=E(Mn+/M)∘​−nFRT​ln[Mn+]1​

E(M/Mn+)​=E(M/Mn+)∘​−nFRT​ln[M][Mn+]​

E(Mn+/M)​=E(Mn+/M)∘​−nFRT​log[M]1​

E(Mn+/M)​=E(Mn+/M)∘​−nFRT​ln[Mn+]