Question

For a cell reaction : $M^{n+}_{\left(aq\right)}+ne^{-} \to M_{\left(s\right)}$, the Nernst equation for electrode potential at any concentration measured with respect to standard hydrogen electrode is represented as

• A. $E_{\left(M^{n+}/M\right)}=E^{\circ}_{\left(M^{n+}/M\right)}-\frac{RT}{nF}ln \frac{1}{\left[M^{n+}\right]}$
• B. $E_{\left(M/M^{n+}\right)}=E^{\circ}_{\left(M/M^{n+}\right)}-\frac{RT}{nF}ln \frac{\left[M^{n+}\right]}{\left[M\right]}$
• C. $E_{\left(M^{n+}/M\right)}=E^{\circ}_{\left(M^{n+}/M\right)}-\frac{RT}{nF}log \frac{1}{\left[M\right]}$
• D. $E_{\left(M^{n+}/M\right)}=E^{\circ}_{\left(M^{n+}/M\right)}-\frac{RT}{nF}ln \left[M^{n+}\right]$

Answer 1

Answer: (A)

Correct answer is (a) $E_{\left(M^{n+}/M\right)}=E^{\circ}_{\left(M^{n+}/M\right)}-\frac{RT}{nF}ln \frac{1}{\left[M^{n+}\right]}$