According to Le Chatelier's principle,adding heat to a solid and liquid in equilibrium with an endothermic nature will cause the:

Which of the following equilibria will shift to the right side on increasing the temperature?

$A$ catalyst can affect a reversible reaction by

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

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.

On addition of an inert gas at constant volume to the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$ at equilibrium,