SELECT * FROM question_mgmt as q WHERE id=3023 AND status=1 SELECT id,question_no,question,chapter FROM question_mgmt as q WHERE courseId=2 AND subId=9 AND chapterId=48 and ex_no='1' AND status=1 ORDER BY CAST(question_no AS UNSIGNED)

Question:

A mixture of 1.57 mol of N2, 1.92 mol of H2 and 8.13 mol of NH3 is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant, Kc for the reaction N2 (g) + 3H2 (g) ↔ 2NH3 (g) is 1.7 × 102.

Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

Answer:

The given reaction is:

N2 (g) + 3H2 (g) ↔ 2NH3 (g)

The given concetration of various species is:

N2  = 1.57/20 molL-1

H2 = 1.92/20 molL-1

NH3 =  8.13/20 molL-1

Now, reaction quotient Qc is:

Qc  = (8.13/20)2  /  (1.57/20) (1.92/20)3

        = 2.4 x 10-3

Since,Qc ≠  Kc the reaction mixture is not at equilibrium.

Again, Qc >  Kc. Hence, the reaction will proceed in the reverse direction.


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