The reaction $SO_2 + Cl_2 \rightleftharpoons SO_2Cl_2$ is exothermic. If some $SO_2$ is added to the equilibrium mixture at constant volume,then ...........

In which of the following equilibrium reactions,the equilibrium would shift to the right,if total pressure is increased?

In the gaseous equilibrium $H_2X_2 + \text{heat} \rightleftharpoons 2HX$,the formation of $HX$ will be favoured by

For the reaction: $A + B + Q \rightleftharpoons C + D$,if the temperature is increased,then the concentration of the products will

Consider the equilibrium $CO_{(g)} + 3H_{2(g)} \rightleftharpoons CH_{4(g)} + H_2O_{(g)}$. If the pressure applied over the system increases by two-fold at constant temperature,then which of the following statements are correct?
$(A)$ Concentration of reactants and products increases.
$(B)$ Equilibrium will shift in the forward direction.
$(C)$ Equilibrium constant increases since the concentration of products increases.
$(D)$ Equilibrium constant remains unchanged as the concentration of reactants and products remain the same.
Choose the correct answer from the options given below:

In the $N_2 + 3H_2 \rightleftharpoons 2NH_3$ reversible reaction,an increase in pressure will favour: