In which of the following reactions will the equilibrium shift to the right if the volume of the container is doubled?

When $NaNO_3$ is heated in a closed vessel,$O_2$ is liberated and $NaNO_2$ is left behind. At equilibrium,

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction is favored at constant temperature by: $(1)$ Adding an inert gas at constant volume $(2)$ Adding $Cl_{2(g)}$ at constant volume $(3)$ Adding an inert gas at constant pressure $(4)$ Increasing the volume of the container $(5)$ Adding $PCl_{5(g)}$ at constant volume

What is the effect of increasing pressure on the dissociation of $PCl_5$ according to the equation $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)} - x \ cal$?

In a reversible reaction,a catalyst will affect the rate of

In which of the following equilibrium reactions does the equilibrium shift to the right when the total pressure is decreased?