Practicing Success
At the reduction-electrode this reaction takes place, A2+ + 2e- ⇔ A. Which is/are correct relation for electrode potential? |
E = EoA2+/A - \(\frac{RT}{2F}\)ln\(\frac{[A]}{[A^{2+}]}\) E = EoA2+/A + \(\frac{RT}{2F}\)ln\(\frac{[A]}{[A^{2+}]}\) E = EoA2+/A + \(\frac{RT}{F}\)ln\(\frac{[A]}{[A^{2+}]}\) E = EoA2+/A - \(\frac{RT}{F}\)ln\(\frac{[A]}{[A^{2+}]}\) |
E = EoA2+/A - \(\frac{RT}{2F}\)ln\(\frac{[A]}{[A^{2+}]}\) |
The electrode potential at any concentration measured with respect to standard hydrogen electrode can be represented by: E = EoM2+/M - \(\frac{RT}{nF}\)ln\(\frac{[M]}{[M^{2+}]}\) |