Consider the following equilibrium process

$2S{O}_3(g)2S{O}_2(g)+O_2(g),H=2198k\frac{J}{m}ol$

How will the concentrations of $S{O}_2,O_2,$ and $S{O}_3$ be affected in each scenario?

$($a$)$ the temperature is increased

$($b$)$ the pressure is decreased by increasing the volume of the container

$($c$)$ the concentration of $O_2$ is increased

$($d$)a$ is added catalyst

$4.$ Predict the shift in the equilibrium position that will occur for each of the following reactions at equilibrium when the volume of the reaction container is increased.

$PC{l}_3(g)+C{l}_2(g)PC{l}_5(g)$

$2NB{r}_3(g)N_2(g)+3B{r}_2(g)$

$CO(g)+C{l}_2(g)COC{l}_2(g)$

$MgC{O}_3(s)MgO(s)+C{O}_2(g)$