A fuel oil is analyzed and found to contain $85\mathrm{.}0$ wt$\%$ carbon $($C$),$

$12\mathrm{.}0wt\%$ elemental hydrogen $($H$),1\mathrm{.}7wt\%$ sulfur $($S$)$ and the

remainder noncombustible matter. The oil is burned with $20\mathrm{.}0\%{?}_{?}$

excess air based on complete combustion of the carbon to $C{O}_{2,(g)},$

the hydrogen to $H_2{O}_{(v)},$ and the sulfur to $S{O}_{2,(g)}.$ The oil is burned

completely, but $8\%$ of the carbon forms CO$.$ Assume the air can

be treated as $21$mol$\%O_2$ and $79$mol$\%N_2$ and that the nitrogen

in the air does not react.

Calculate the mole fraction of $C{O}_2$ in the stack gas.

Though the composition does not depend on the total amount of

fuel burned, to make checking your intermediate calculations

easier take $100g$ of the oil burned as the basis for your

calculations. You can ignore the non$-$combustible material in your

calculations since it neither participates in the reactions nor ends

up in the stack gas $($it is ash that drops out as a solid$).$ Make a spice table with $9$ species $($C$,$ H$,$ S$,$ O$2,$ N$2,$ CO$2,$ CO$,$ H$2$O$,$ and SO$2)$