The exothermic formation of $ClF_3$ is represented by the equation $Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}$; $\Delta H = -329 \ kJ$. Which of the following will increase the quantity of $ClF_3$ in an equilibrium mixture of $Cl_2, F_2$ and $ClF_3$?

At $25\,^oC$,the equilibrium $SO_2Cl_2(g) \rightleftharpoons SO_2(g) + Cl_2(g)$ is established in a closed vessel. When $Cl_2$ is added to the equilibrium mixture,which of the following statements is/are correct for the system?
$(1)$ Change in concentrations of $SO_2$,$Cl_2$,and $SO_2Cl_2$.
$(2)$ More $Cl_2$ is produced.
$(3)$ The concentration of $SO_2$ decreases and the concentration of $SO_2Cl_2$ increases.

Assertion : $A$ catalyst does not alter the equilibrium constant of a reaction.
Reason : The catalyst forms a complex with the reactants and provides an alternate path with lower energy of activation for the reaction; the forward and the backward reactions are affected to the same extent.

For the endothermic reaction $A_{2} \rightarrow 2A$,which of the following will increase the yield of the monomer $A$?

On increasing temperature,the equilibrium constant of exothermic and endothermic reactions,respectively

In which direction does the equilibrium $C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2_{(g)}}$ shift when the pressure is increased?