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

`N_2(g) + 3H_2(g) hArr 2NH_3(g)`
`Q=[NH_3]^2/([N_2][H_2]^3)`
`Q=(0.50)^2/((3.0)xx(2.0)^3)`=0.0104
Since `Q_c ne K_c`, the reaction is not in equilibrium . As `Q_c lt K_c` the reaction will proceed to form more products i.e., in forward direction.