Equilibrium constant, `K_(c)` for the reaction,
`N_(2(g))+3H_(2(g))hArr2NH_(3(g))`,
at `500 K` is `0.061 litre^(2) "mole"^(-2)`. At a particular time, the analysis shows that composition of the reaction mixture is `3.00 mol litre^(-1)N_(2)`, `2.00 mol litre^(-1)H_(2)`, and `0.500 mol litre^(-1)NH_(3)`. Is the reaction at equilibrium? If not, in which direction does the reaction tend to proceed to reach equilibrium?

Explanation

`Q=([NH_(3)]^(2))/([H_(2)]^(3)[N_(2)])=((0.5)^(2))/((2.0)^(3)xx(3.0))=(0.25)/(24)`
`=0.0104 ne K_(c)`.
`:.` The reaction is not in equilibrium.
`:.` Reaction proceeds from left to right.
`:' Q lt K_(c)`.