When $I_2$ dissociates to its atomic form the following reaction occurs:
$I_{2(g)} \rightleftharpoons 2I_{(g)} ; \Delta_r H^o = +150 \ kJ \ mol^{-1}$
The forward reaction is favoured at:

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

Which of the following equilibria is not affected by a change in the volume of the flask?

Does the number of moles of reaction products increase,decrease,or remain the same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
$(a)$ $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$
$(b)$ $CaO_{(s)} + CO_{2(g)} \rightleftharpoons CaCO_{3(s)}$
$(c)$ $3Fe_{(s)} + 4H_{2}O_{(g)} \rightleftharpoons Fe_{3}O_{4(s)} + 4H_{2(g)}$

The increase of pressure on the ice $\rightleftharpoons$ water system at constant temperature will lead to:

The equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$ is attained at $25 ^\circ C$ in a closed container and an inert gas helium is introduced. Which of the following statements is correct?