A mixture of `1.57 mol` of `N_(2), 1.92 mol` of `H_(2)` and `8.13 mol` of `NH_(3)` is introduced into a `20 L` reaction vessel at `500 K`. At this temperature, the equilibrium constant `K_(c )` for the reaction `N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)` is `1.7xx10^(2)`. Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

Answer

`Q=2.38xx10^3` , NO, reaction is not at equilibrium

Explanation

`Q=([NH_3]^2)/([N_2][H_2]^3)`
`=(8.13/20)^2/((1.57/20)(1.92/20)^3)=2.38xx10^3`
So, reaction is not at equilibrium . Reaction will proceed in the direction of reactants i.e., reverse direction.