Equilibrium constant, Kc for the reaction.
N2(g)+3H2(g↔2NH3(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−1N2,2.0molL−1H2 and 0.5 mol L−1NH3, Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?
The given reaction is:
N2(g)+3H2(g)↔2NH3(g)At a particular time:3.0mol L−12.0mol L−10.5mol L−1
Qc=[NH3]2[N2][H2]3=(0.5)2(3.0)(2.0)3=0.0104
It is given that Kc=0.061
Since Qc≠Kc, the reaction is not at equilobrium,
Since, Qc<Kc, the reaction will proceed in the forward to reach equilibrium.