A sealed container holds an equilibrium mixture of $N_2O_4(g)$ (colorless) and $NO_2(g)$ (brown). The forward reaction is endothermic. Which of the following changes will NOT result in an increase in the intensity of the brown color within the container?

Consider the equilibrium $CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)$. Increasing the pressure of $CO_2$ will:

For the reaction $PC{l_5}\left( g \right) + C{l_2}(g)\underset{{}}{\overset{{}}{\leftrightharpoons}}PC{l_5}(g),$ the position of equilibrium can be shifted to the right by

For which of the following reactions,${K_p} = {K_c}$ ?

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

The gaseous reaction,

$A + B\leftrightharpoons2C + D + {\cal Q}$ is most favoured at

The dissolution of $NH_4Cl$ in water is an endothermic process. According to Le Chatelier's principle, which of the following will increase the solubility of $NH_4Cl$?

The equilibrium, $2{\rm{S}}{{\rm{O}}_2}\left( {\rm{g}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right)\;\leftrightharpoons\;2{\rm{S}}{{\rm{O}}_3}\left( {\rm{g}} \right)$ shifts forward if:

In a reaction $PC{l_5}PC{l_3} + C{l_2}$, degree of dissociation is 30%, If initial moles of $PC{l_5}$ is one then total moles at equilibrium is

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:

${\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\left( l \right) + {{\rm{C}}_2}{{\rm{H}}_5}{\rm{OH}}\left( l \right)\;\leftrightharpoons\;{\rm{C}}{{\rm{H}}_3}{\rm{COO}}{{\rm{C}}_2}{{\rm{H}}_5}\left( l \right) + {{\rm{H}}_2}{\rm{O}}\left( l \right)$In the above reaction, one mole of each of acetic acid and alcohol are heated in the presence of little conc. ${{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}$. On equilibrium being attained