Determine the free energy in $kJ$ for the aerobic reaction in question $3$ i$)$ under standard conditions and ii$)$ when $pH$ is $6,$ oxygen is $0\mathrm{.}2$atm, hydrogen sulfide is $0\mathrm{.}5$atm, and sulfate is $0\mathrm{.}5M?[$free energies shown in table below$]$

$\backslash$table$[[$Carbon compound,Carbon compound,Metal,Nonmetal,Nitrogen compound$],[CO,-137\mathrm{.}34,$Glutamine, $-529\mathrm{.}7,C{u}^{+},+50\mathrm{.}28,H_{2}O,N_2\mathrm{.}0$

a$)$ Balance the reaction of hydrogen sulfide $(H_2(S))$ being oxidized to sulfate $(S{O}_4^{2-})$ under aerobic conditions.

b$)$ Balance the reaction when hydrogen sulfide is oxidized with iron $(F{e}^{3+})$ as the electron acceptor.

c$)$ Write out the complete balanced reaction from the following $2$ half reactions:

$CO\frac{2}{?}$ methanol $6$ e$-$ and $N\frac{O_3}{1}\frac{?}{2N_{2}5}$ e$-$