On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish, (as predicted by applying the Le Chatelier's principle) for the reaction: ${\mathrm{N}}_2 \left(\mathrm{g}\right)+3{\mathrm{H}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)$. Which of the following options is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?

Some quantity of water is contained in a container as shown as shown in figure. As neon is added to this system at constant pressure, the amount of liquid water in the vessel

The thermal dissociation equilibrium reaction of ${\mathrm{CaCO}}_3 \left(\mathrm{s}\right)$ is studied under different conditions
${\mathrm{CaCO}}_3 \left(\mathrm{s}\right)\rightleftharpoons \mathrm{CaO} \left(\mathrm{s}\right)+{\mathrm{CO}}_2 \left(\mathrm{g}\right)$

For this equilibrium reaction, the correct statement(s) is/ (are):