P$2$ Material Balance

$(45$ Marks$)$

fod in $10\%$ excess of the amolnt theoretically required to oxtdize all sulfur in the ore to SO$.$ A pyrite $($FeS$5)$ conversion of $85\%$ is obtained, with $40\%$ of FeS comvened to sulfur dioxide $($SO$)$ and the rest forming sulfur trioxide $($SO$).$ Two strearns lesve the furnace: a gas stheam containing $S{O}_3,S{O}_2,O_2,$ and $N_2,$ and a solid stream comatitine unconverted pyrite, ferric oxide $($Fe$2$O$3),$ and inert. The following reactions the place in the furnace:

$Fe{S}_2(s)+\frac{15}{2}{O}_2(g)F{e}_2{O}_3(s)+4S{O}_3(g)$

$2Fe{S}_2(s)+\frac{11}{2}{O}_2(g)F{e}_2{O}_3(s)+4S{O}_2(g)$

a$.$ Using $100k\frac{g}{m}in$ of ore as a basis, calculate the rate of Fer. production $)$ in the outlet solid stream, and the total molar flow and composition of the outlet gas stream.

The molecular weight of $Fe=55\mathrm{.}84\frac{g}{m}ol$ The molecular weight of $S=32\mathrm{.}06\frac{g}{m}ol$ The molecular weight of $O=16\mathrm{.}00\frac{g}{m}ol$

Figure $1$ Furnace for Ferric Oxide Production