Question

Question 7.21 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–1 N2, 2.0 mol L–1 H2 and 0.5 mol L–1 NH3. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

Class XI Equilibrium Page 226

Answer 1

N2(g) + 3H2(g) == 2NH3(g); Kc = 0.061 at 500K

Given, [ N2] = 3.0 mol/L
[ H2 ] = 2.0 mol/L
[ NH3 ] = 0.5 mol/L

$now, Q_c=\frac{[NH_3]^2}{[N_2][H_2]^3}$

Qc = (0.5)²/3 × 2³ = 0.0104
but Kc = 0.061
so, Kc ≠ Qc , equilibrium has not been attained.
here, Kc > Qc , the reaction will proceed from left to right . e.g., towards formation of more products.

Answer 2

Answer:

a backward reaction occcurs

Explanation: