Equilibrium constant, `K_(c)` for the reaction, `N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)` at 500K is 0.061. at a particular time, the analysis shows that composition of the reaction mixture is 3.0 `mol*L^(-1)" "N_(2),2.0mol*L^(-1)" "H_(2) and 0.5mol*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))/(3.0xx(2.0)^(3))=0.0104`
For the reaction, `K_(c)=0.061`
Hence, `Q_(c) lt K_(c)`. So the reaction is not at equilibrium and will tend to proceed towards right in the forward direction to reach equilibrium.