Q$13$ Consider the reaction, $2S{O}_2(g)+O_2(g)2S{O}_3(g),$ at $T=525C$ with $H=-197kJ.$ This reaction has an equilibrium constant $K=781$ at this temperature. Which condition$($s$)$ listed below will cause a shift in the reaction equilibrium to RIGHT?

I. If $P_{S{O}_3}=0\mathrm{.}400$atm,$P_{S{O}_2}=0\mathrm{.}050$atm, and $P_{O_2}=0\mathrm{.}050$atm

II$.$ If at equilibrium, $P_{SO3}$ is suddenly decreased by removing $S{O}_3$

III. If at equilibrium, the volume of the vessel is decreased

IV$.$ If at equilibrium, the nonreacting element $Ar(g)$ is added without changing the volume $V.$ If at equilibrium the temperature of the vessel is decreased without changing the volume

a$.$ II$,$ III and V

b$.$ I, II and III

c$.$ II and III

d$.$ II and V

e$.$ III and IV