$CH2S$ was heated with air and underwent the following conversion.

$C{H}_{2}S+5(O_2+3\mathrm{.}78N_2)C{O}_2+H_{2}O+S{O}_2+2\mathrm{.}5O_2+18\mathrm{.}9N_2$

The system temperature was maintained at $1500K$

What are the equilibrium concentrations of $S{O}_2$ and $S{O}_3$ in ppm$?$

$S{O}_2+\frac{1}{2}O2<-S{O}_3$

The $K_p$ value for this reaction at $1500K$ is $0\mathrm{.}04$

You can solve using solver or other methods or assume that the

number of moles transferred is small.

$SO2=40,500ppm$;$SO3=520ppm$

$SO2=0\mathrm{.}0004ppm$;$SO3=0\mathrm{.}0000005ppm$

$SO2=405ppm$;$SO3=52,000ppm$

$SO2=20,100ppm$;$SO3=20,100ppm$