Equilibrium constant, `K_(c)` for the reaction
`N_(2)(g) + 3H_(2) hArr 2NH_(3)(g)` at `500 K` is `0.061`
At a particular time, the analysis shows that composition of the reaction mixture is `3.0` mol `L^(-1) N_(2)`. `2.0 "mol" L^(-1) H_(2)` and `0.5` mol `L^(-1) NH_(3)`. Is the reaction at equilibrium?
If not in which direction does the reaction tend to proceed to reach equilibrium?

Explanation

` N_2(g) +3H_2(g) hArr 2NH_3 (g) ,K_c =0.061 `
For the given set of conditions.
` Q_c = ([NH_3(g) ]^(2))/( [N_2(g) ][H_2(g) ]^(3))= ( 0.500)/((3.00) xx( 2.00) ^(3) ) = 0.021 `
Since ` Q_c lt K_c ` , the reactions is not at equilibrium . it will proceed in the foward directions.