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?

When ${\rm{NaN}}{{\rm{O}}_3}$ is heated in a closed vessel, ${{\rm{O}}_2}$ is liberated and ${\rm{NaN}}{{\rm{O}}_2}$ is left behind. Atequilibrium,(i)Addition of ${\rm{NaN}}{{\rm{O}}_3}$ favours forward reaction(ii) Addition of ${\rm{NaN}}{{\rm{O}}_2}$ favours backward reaction(iii) Increasing pressure favours reverse reaction(iv) Increasing temperature favours forward reaction Correct option is

The following reactions are known to occur in the body,

${\rm{C}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}}\leftrightharpoons{{\rm{H}}_2}{\rm{C}}{{\rm{O}}_3}\leftrightharpoons{{\rm{H}}^ + } + {\rm{HCO}}_3^ -$

If ${\rm{C}}{{\rm{O}}_2}$ escapes from the system, then:

According to Le-Chatelier’s principle, if heat is given to solid-liquid system, then

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:

Indicate the correct answer out of the following for the reaction,

${\rm{N}}{{\rm{H}}_4}{\rm{Cl}} + {{\rm{H}}_2}{\rm{O}}\;\leftrightharpoons{\rm{N}}{{\rm{H}}_4}{\rm{OH}} + {\rm{HCl}}$

Predict the conditions for forward reaction on the basis of Le-Chatelier’s principle for :

$2{\rm{S}}{{\rm{O}}_2}\left( {\rm{g}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right)\;\leftrightharpoons\;2{\rm{S}}{{\rm{O}}_3}\left( {\rm{g}} \right);\;\;\Delta H = \;\; - 198{\rm{\;kJ}}.$

When hydrogen molecules decomposed into it’s atoms which conditions gives maximum yield of H atom?

For reaction $A(g) + B(g)AB(g)$, We start with 2 moles of A and B each. At equilibrium 0.8 moles of AB is formed. Then how much of A changes to AB.

The law of mass action was enunciated by

In the reaction ${A_2}(g) + 4{B_2}(g)\leftrightharpoons2A{B_4}(g),\Delta H < O$ the formation of $A{B_4}$ will be favoured at