In the Haber-Bosch process for ammonia synthesis, $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, the reaction is exothermic. To maximize ammonia yield at high pressure, which catalyst would theoretically be most effective, assuming all are equally active at standard conditions?

Which favours the backward reaction in a chemical equilibrium?

The solubility product ($K_{sp}$) of $AgCl$ in water at 25°C is $1.8 imes 10^{-10}$. A solution of $AgCl$ in water is in equilibrium with solid $AgCl$. If a small amount of $NaCl$ is added to this saturated solution, what will happen to the solubility ($s$) and $K_{sp}$ of $AgCl$?

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

The active mass of 45 g of ${\rm{KCl}}$ in a 3 L flask would be

The change in pressure will not affect the equilibrium constant for

Consider the equilibrium: $2NO_2(g) \rightleftharpoons N_2O_4(g)$. Adding more $N_2O_4$ will:

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

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 active mass of 45 g of ${\rm{KCl}}$ in a 3 L flask would be

For the reason, $PC{l_5}_{_{(g)}}\underset{{}}{\overset{{}}{\leftrightharpoons}}PC{l_3}_{_{(g)}} + C{l_2}_{_{(g)}}$ the forward reaction at constant temperature is favoured by