Suppose the reaction $PCl_{5(s)} \rightleftharpoons PCl_{3(s)} + Cl_{2(g)}$ is in a closed vessel at equilibrium. What is the effect on the equilibrium concentration of $Cl_{2(g)}$ by adding $PCl_{5(s)}$ at constant temperature?

$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,$\Delta H = +q \ cal$. The formation of $HI$ is:

The equilibrium $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ shifts forward,if

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

The rate of reaction of which of the following is not affected by pressure?

Consider the reaction equilibrium,$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$; $\Delta H^\circ = -198 \ kJ$. On the basis of Le Chatelier's principle,the condition favourable for the forward reaction is