(Solved): Need help with all parts or whatever you can! (Use the table to rationalize concepts)For the followi ...

TABLE 18.1 Standard Electrode Potentials at $25^{?}\mathrm{C}$ For the following reactions: 1. Assign oxidation numbers for each of the elements participating, 2. Identify the oxidant and reductant and write the reduction and oxidation half-reactions 3. Balance the equations 4. Write the net equations in the neutral form (where necessary) 5. Determine if the redox processes are spontaneous under standard conditions a) ${\mathrm{Mn}}^{3+}(\mathrm{aq})+{\mathrm{H}}_2\mathrm{O}(\mathrm{I})?{\mathrm{MnO}}_2(\mathrm{s})+{\mathrm{Mn}}^{2+}(\mathrm{aq})+{\mathrm{H}}^{+}(\mathrm{aq})$ b) ${\mathrm{MnO}}_4^{?}(\mathrm{aq})+{\mathrm{H}}_2{\mathrm{SO}}_3(\mathrm{aq})?{\mathrm{Mn}}^{2+}(\mathrm{aq})+{\mathrm{HSO}}_4^{?}$(aq) c) For the reaction shown in b, predict the qualitative $\mathrm{pH}$ dependence on the net potential for this reaction (that is: increases, decreases, remains the same).