The equilibrium constants of the following are

N₂ + 3H₂ $$\rightleftharpoons$$ 2NH₃;     K₁

N₂ + O₂ $$\rightleftharpoons$$ 2NO;     K₂

H₂ + $${1 \over 2}$$O₂ $$\rightleftharpoons$$ H₂O;     K₃

The equilibrium constant (K) of the reaction :

2NH₃ + $${5 \over 2}$$ O₂ $$\rightleftharpoons$$ 2NO + 3H₂O will be

The reaction quotient (Q) for the reaction

N_2(g) + 3H_2(g) $$\rightleftharpoons$$ 2NH_3(g) is given by

$$Q = {{{{\left[ {N{H_3}} \right]}^2}} \over {\left[ {{N_2}} \right]{{\left[ {{H_2}} \right]}^3}}}$$.

The reaction will proceed from right to left if

Reaction BaO_2(g) $$\rightleftharpoons$$ BaO_(s) + O_2(g); $$\Delta $$H = +ve. In equilibrium condition, pressure of O₂ depends on

For any reversible reaction, if we increase concentration of the reactants, then effect on equilibrium constant