Question

Answer the following questions using data from Table 11.1 (all under standard conditions).

a. Is${\mathbf{H}}^{\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$ capable of oxidizing$\mathbf{Cu}\mathbf{\left(}\mathbf{s}\mathbf{\right)}$ to${\mathbf{Cu}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$?

b. Is${\mathbf{Fe}}^{\mathbf{3}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$ capable of oxidizing ${\mathbf{I}}^{\mathbf{-}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$?

c. Is${\mathbf{H}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$ capable of reducing ${\mathbf{Ag}}^{\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$?

d. Is${\mathbf{Fe}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$ capable of reducing ${\mathbf{Cr}}^{\mathbf{3}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}{\mathbf{toCr}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$?

Short answer

a. ${\text{H}}^{\text{+}}\left(\mathrm{aq}\right)$is not capable of oxidizing${\text{Cu}}^{2+}\left(\text{aq}\right)$

b.${\text{Fe}}^{\text{3+}}\left(\text{aq}\right)$ is capableof oxidizing${\text{I}}^{\text{-}}\left(\text{aq}\right)$

c. ${\text{H}}_{\text{2}}\left(\text{g}\right)$is capable of reducing${\text{Ag}}^{+}\left(\text{aq}\right)$

d.${\text{Fe}}^{2+}\left(\mathrm{aq}\right)$ is not capable of oxidizing${\text{Cr}}^{\text{3+}}\left(\text{aq}\right){\text{toCr}}^{2+}\left(\text{aq}\right)$

Step-by-step solution

Definition of oxidizing

An oxidizing agent is acompound or element that is present in a redox(oxidation-reduction) reaction which receives electrons originating from a different species.

oxidizing CU2+(aq)

$\begin{array}{l}{\mathrm{E}}_{\mathrm{cell}}^0={\mathrm{E}}_{\mathrm{cathode}}+{\mathrm{E}}_{\begin{array}{l}\mathrm{anode}\\ \end{array}}\\ {\mathrm{E}}_{\mathrm{cell}}^0=\left(0.00\mathrm{V}\right)-\left(0.34\mathrm{V}\right)\\ {\mathrm{E}}_{\mathrm{cell}}^0=-0.34\mathrm{V}\end{array}$

oxidizing I-(aq)

$\begin{array}{l}{\mathrm{E}}_{\mathrm{cell}}^0={\mathrm{E}}_{\mathrm{cathode}}+{\mathrm{E}}_{\begin{array}{l}\mathrm{anode}\\ \end{array}}\\ {\mathrm{E}}_{\mathrm{cell}}^0=\left(0.77\mathrm{V}\right)-\left(0.54\mathrm{V}\right)\\ {\mathrm{E}}_{\mathrm{cell}}^0=1.31\mathrm{V}\end{array}$

reducing Ag+(aq)

$\begin{array}{l}{\mathrm{E}}_{\mathrm{cell}}^0={\mathrm{E}}_{\mathrm{cathode}}+{\mathrm{E}}_{\begin{array}{l}\mathrm{anode}\\ \end{array}}\\ {\mathrm{E}}_{\mathrm{cell}}^0=\left(0.80\mathrm{V}\right)-\left(0.00\mathrm{V}\right)\\ {\mathrm{E}}_{\mathrm{cell}}^0=0.80\mathrm{V}\end{array}$

oxidizing Cr3+(aq)toCr2+(aq)

$\begin{array}{l}{\mathrm{E}}_{\mathrm{cell}}^0={\mathrm{E}}_{\mathrm{cathode}}+{\mathrm{E}}_{\begin{array}{l}\mathrm{anode}\\ \end{array}}\\ {\mathrm{E}}_{\mathrm{cell}}^0=\left(-0.77\mathrm{V}\right)-\left(0.41\mathrm{V}\right)\\ {\mathrm{E}}_{\mathrm{cell}}^0=-0.36\mathrm{V}\end{array}$