19.1 Exercise 15

The standard reduction potential for the reaction $\left[\text{Co} \left(\text{H}_{2} \text{O}\right)_{6}\right]^{3+} \left(a q\right) + \text{e}^{-} \rightarrow \left[\left(\text{Co} \left(\right. \text{H}\right)_{2} \text{O} \left.\right)_{6}\right]^{2+} \left(a q\right)$ is about 1.8 V. The reduction potential for the reaction $\left[\text{Co} \left(\text{NH}_{3}\right)_{6}\right]^{3+} \left(a q\right) + \text{e}^{-} \rightarrow \left[\text{Co} \left(\text{NH}_{3}\right)_{6}\right]^{2+} \left(a q\right)$ is +0.1 V. Calculate the cell potentials to show whether the complex ions, [Co(H₂O)₆]²⁺ and/or [Co(NH₃)₆]²⁺, can be oxidized to the corresponding cobalt(III) complex by oxygen.