For the reaction $2 \ HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)} - Q \ kJ$,the equilibrium constant depends upon

For the reaction $A + B \rightleftharpoons C + D$,the equilibrium constant is $K$. If the initial moles of $A$ and $B$ are $1.0 \ mol$ each,what will be the value of the equilibrium constant in a second experiment under the same conditions if the initial moles of $A$ and $B$ are $2 \ mol$ and $3 \ mol$ respectively?

Explain solid-liquid equilibrium by giving an example.

For the equilibrium system $H_2 + I_2 \rightleftharpoons 2HI$,if the concentration of the reactants is increased at $25\,^oC$,what happens to the value of $K_c$?

Predict which of the following reactions will have an appreciable concentration of both reactants and products:
$(a)$ $Cl_{2(g)} \longleftrightarrow 2Cl_{(g)};$ $K_{c}=5 \times 10^{-39}$
$(b)$ $Cl_{2(g)}+2NO_{(g)} \longleftrightarrow 2NOCl_{(g)};$ $K_{c}=3.7 \times 10^{8}$
$(c)$ $Cl_{2(g)}+2NO_{2(g)} \longleftrightarrow 2NO_{2}Cl_{(g)};$ $K_{c}=1.8$

If the value of equilibrium constant for a particular reaction is $1.6 \times 10^{12}$,then at equilibrium the system will contain: