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1. Dichromate ion $\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}\right)$ in acidic solution is a good oxidizing agent. Which of the following oxidations can be accomplished with dichromate ion in acidic solution? Explain a. $\mathrm{Sn}^{2+}(\mathrm{aq})$ to $\mathrm{Sn}^{4+}(\mathrm{aq})$ b. $\mathrm{Ag}(\mathrm{s})$ to $\mathrm{Ag}^{+}(\mathrm{aq})$
2. For each of the following cell diagrams a. $\operatorname{Pt}(\mathrm{s})\left|\mathrm{Fe}^{2+}(\mathrm{aq}), \mathrm{Fe}^{3+}(\mathrm{aq}) \|\left|\mathrm{Ag}^{+}(\mathrm{aq})\right| \mathrm{Ag}(\mathrm{s})\right.$ b. $\mathrm{Pt}(\mathrm{s})\left|\mathrm{Mn}^{2+}(\mathrm{aq}), \mathrm{MnO}_{4}^{-}(\mathrm{aq})\right|\left|\mathrm{Cu}^{2+}(\mathrm{aq})\right| \mathrm{Cu}(\mathrm{s})$ i. calculate the $E_{\text {cell }}^{o}$ ii. what is the change in Gibbs free energy? iii. is the cell reaction spontaneous or nonspontaneous? Explain.
3. Will the following reaction $$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2 \cdot}(\mathrm{aq})+14 \mathrm{H}^{+}+6 \mathrm{Ag}(\mathrm{~s}) \longrightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+6 \mathrm{Ag}^{+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) E_{\text {cell }}=-0.023 \mathrm{~V}$$ be spontaneous if $\left[\mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}\right]=[\mathrm{Ag}+]=0.675 \mathrm{M},\left[\mathrm{Cr}^{3+}\right]=0.6 \mathrm{M}$ and $\mathrm{pH}=2$ ? Explain.
4. Define the following terms a) Oxidation b) Oxidizing agent c) Salt bridge d) Liquid junction e) Standard electrode potential