Consider the endothermic reaction: $N_2O_4(g) \rightleftharpoons 2NO_2(g)$. A sealed container filled with an equilibrium mixture of $N_2O_4$ and $NO_2$ is suddenly immersed in an ice bath. Which of the following changes will occur initially?

In chemical reaction, $A\;\leftrightharpoons\;B$, the system will be known in equilibrium when

The melting points of most of the solid substances increase with an increase of pressure. However, ice melts at a temperature lower than its usual melting point when the pressure is increased. This is because:

Raising the temperature of a reversible chemical reaction :

What happens to the yield on application of high pressure in the Haber’s synthesis of ammonia?

On addition of an inert gas at constant volume to the reaction, ${{\rm{N}}_2} + 3{{\rm{H}}_2}\,\leftrightharpoons\,\,2{\rm{N}}{{\rm{H}}_3}$ at equilibrium:

Raising the temperature of a reversible chemical reaction :

The melting points of most of the solid substances increase with an increase of pressure. However, ice melts at a temperature lower than its usual melting point when the pressure is increased. This is because:

The reaction quotient $\left( Q \right)$ for the reaction is given by: ${{\rm{N}}_2}\left( {\rm{g}} \right) + 3{{\rm{H}}_2}\left( {\rm{g}} \right)\leftrightharpoons2{\rm{N}}{{\rm{H}}_3};Q = \frac{{{{\left[ {{\rm{N}}{{\rm{H}}_3}} \right]}^2}}}{{\left[ {{{\rm{N}}_2}} \right]{{\left[ {{{\rm{H}}_2}} \right]}^3}}}$The reaction will proceed from right to left if:

Which favours the backward reaction in a chemical equilibrium?

The Haber's process for the manufacture of ammonia is usually carried out at about $500^\circ C$. If a temperature of about $250^\circ C$ was used instead of $500^\circ C$: