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

`Q_(c)=([NH_(3)]^(2))/([N_(2)][H_(2)]^(3))=((0.5)^(2))/((3.0)(2.0)^(3))=0.0104`
As `Q_(c ) ne K_(c )`, reaction is not in equilibrium.
As `Q_(c ) lt K_(c )` reaction will proceed in the forward direction.