The correct answer is : 2
.712 = .770 - \(\frac{.058}{2}\log[\frac{Fe^{2+}}{Fe^{3+}}]^2\)
-.058 = .-058 \(\log\frac{[Fe^{2+}]}{[Fe^{3+}]}\)
\(\frac{Fe^{2+}}{Fe^{3+}}=10=t\)
\(\frac{t}{5}=2\)
For the given cell: \[ {Fe}^{2+}(aq) + {Ag}^+(aq) \to {Fe}^{3+}(aq) + {Ag}(s) \] The standard cell potential of the above reaction is given. The standard reduction potentials are given as: \[ {Ag}^+ + e^- \to {Ag} \quad E^\circ = x \, {V} \] \[ {Fe}^{2+} + 2e^- \to {Fe} \quad E^\circ = y \, {V} \] \[ {Fe}^{3+} + 3e^- \to {Fe} \quad E^\circ = z \, {V} \] The correct answer is: