For the following reaction

One could increase the concentration of $BaC{O}_{3(g)}$ at equilibrium by

a$)$ decreasing the pressure b$)$ increasing the temperature

c$)$ increasing the volume d$)$ adding more $C{O}_2(g)$

e$)$ adding a catalyst

If the temperature of an exothermic reaction increases, what will happen to the value of the equilibrium constant?

a$)$ it will increase b$)$ it will decrease

c$)$ it will remain the same d$)$ there is not enough information provided to answer

Which system, initially at equilibrium, reacts toward the left upon an increase in external pressure, but toward the right upon an increase in temperature?

a$)2N{O}_2(g)+54kJ4(8)2NO(g)+O_2(g)$

b$)H_{2(g)}+I_{2(g)}$ in & $2HI+$ heat

c$)PC{l}_{3(g)}+C{l}_{2(g)}o+PC{l}_5$oxH$=+16\mathrm{.}6k\frac{J}{m}ol$

d$)$ CaO$(s)+C{O}_2(g)+CaC{O}_3(s)+$ heat

e$)N_2(g)+3H_2(g)$