For the following half-reactions, answer the questions below. $$ \begin{array}{cc} \mathrm{Co}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Co}^{2+}(a q) & E^{\circ}=+1.953 \mathrm{~V} \\ \mathrm{Fe}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Fe}^{2+}(a q) & E^{\circ}=+0.769 \mathrm{~V} \\ \mathrm{I}_{2}(a q)+2 e^{-} \longrightarrow 2 \mathrm{I}^{-}(a q) & E^{o}=+0.534 \mathrm{~V} \\ \mathrm{~Pb}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Pb}(s) & E^{\circ}=-0.127 \mathrm{~V} \\ \mathrm{Cd}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Cd}(s) & E^{\circ}=-0.402 \mathrm{~V} \\ \mathrm{Mn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Mn}(s) & E^{\circ}=-1.182 \mathrm{~V} \end{array} $$ (a) Which is the weakest reducing agent? (b) Which is the strongest reducing agent? (c) Which is the strongest oxidizing agent? (d) Which is the weakest oxidizing agent? (e) Will \(\mathrm{Pb}(s)\) reduce \(\mathrm{Fe}^{3+}(a q)\) to \(\mathrm{Fe}^{2+}(a q) ?\) (f) Will \(\mathrm{I}^{-}(a q)\) reduce \(\mathrm{Pb}^{2+}(a q)\) to \(\mathrm{Pb}(s) ?\) (g) Which ion(s) can be reduced by \(\mathrm{Pb}(s)\) ? (h) Which if any metal(s) can be oxidized by \(\mathrm{Fe}^{3+}(a q)\) ?

Step by step solution

01

(a) Weakest reducing agent

The weakest reducing agent will have the highest standard reduction potential. In this case, Co redution potential is +1.953 V, which is the highest among the given half-reactions. Therefore, Co^3+(aq) is the weakest reducing agent.

02

(b) Strongest reducing agent

The strongest reducing agent will have the lowest standard reduction potential. In this case, Mn's reduction potential is -1.182 V, which is the lowest among the given half-reactions. Therefore, Mn^2+(aq) is the strongest reducing agent.

03

(c) Strongest oxidizing agent

The strongest oxidizing agent will have the highest standard reduction potential. As determined in part (a), it is the Co^3+(aq) with a standard reduction potential of +1.953 V.

04

(d) Weakest oxidizing agent

The weakest oxidizing agent will have the lowest standard reduction potential. As determined in part (b), it is the Mn^2+(aq) with a standard reduction potential of -1.182 V.

05

(e) Will Pb(s) reduce Fe^3+(aq) to Fe^2+(aq)?

To determine if Pb(s) will spontaneously reduce Fe^3+(aq) to Fe^2+(aq), compare the standard reduction potentials of both half-reactions. Pb's reduction potential is -0.127 V, while Fe^3+'s is +0.769 V. Since Pb's potential is lower than Fe^3+'s, Pb(s) will spontaneously reduce Fe^3+(aq) to Fe^2+(aq).

06

(f) Will I^-(aq) reduce Pb^2+(aq) to Pb(s)?

In order to determine if I^-(aq) will spontaneously reduce Pb^2+(aq) to Pb(s), compare the standard reduction potentials of both half-reactions. I₂ reduction potential is +0.534 V, while Pb^2+'s is -0.127 V. Since I₂'s potential is higher than Pb^2+'s, I^-(aq) will not spontaneously reduce Pb^2+(aq) to Pb(s).

07

(g) Which ions can be reduced by Pb(s)?

To determine which ions can be reduced by Pb(s), compare Pb's standard reduction potential (-0.127 V) with other ions. Pb(s) can reduce ions with a higher reduction potential, which includes: Fe^3+(aq) with a potential of +0.769 V and Co^3+(aq) with a potential of +1.953 V.

08

(h) Which metals can be oxidized by Fe^3+(aq)?

To determine which metals can be oxidized by Fe^3+(aq), compare its standard reduction potential (+0.769 V) with other metals. Fe^3+(aq) can oxidize metals with a lower reduction potential, which includes: Pb(s) with a potential of -0.127 V, Cd(s) with a potential of -0.402 V, and Mn(s) with a potential of -1.182 V.

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