The equilibrium constant, Kc for the reaction

N2(g)+3H2(g) ⇌ 2NH at 500 K is 0.061

At a specific time, from the analysis, we can conclude that the composition of the reaction mixture is 3.0 mol L –1 N2, 2.0 mol L–1 Hand 0.5 mol L–1 NH3. Find out whether the reaction is at equilibrium or not? Find in which direction the reaction proceeds to reach equilibrium.

Asked by Abhisek | 1 year ago |  80

##### Solution :-

N2(g) + 3H2(g)     2NH3

At a particular time:  3.0 mol L-1 ,  2.0mol L-1  , 0.5 mol L-1

So,

$$Qc=\dfrac{[NH_{3}]^{2}}{[N_{2}][H_{2}]^{3}}\\ \\$$

$$=\dfrac{(0.5)^{2}}{(3.0)(2.0)^{3}}\\ \\$$

$$=0.0104$$

It is given that Kc=0.061

$$Qc \neq K_{c}$$, the reaction is not at equilibrium.

$$Qc < K_{c}$$​,

the reaction preceeds in the forward direction to reach at equilibrium.

Answered by Pragya Singh | 1 year ago

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