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NCERT Class XI Chemistry Equilibrium Solutions

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Question : 12 of 73
Marks: +1, -0
A mixture of 1.57 mol of N2\mathrm{N}_2, 1.92 mol of H2\mathrm{H}_2 and 8.13 mol of NH3\mathrm{NH}_3 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)\mathrm{N}_{2(g)} + 3\mathrm{H}_{2(g)} ⇌ 2NH3(g)2\mathrm{NH}_{3(g)} is 1.7 × 10210^2. Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?
Solution:  
The reaction is : N2(g)+3H2(g)\mathrm{N}_{2(g)} + 3\mathrm{H}_{2(g)} ⇌ 2NH3(g)2\mathrm{NH}_{3(g)}
QcQ_c = [NH3]2[N2][H2]3\frac{[\mathrm{NH}_3]^2}{[\mathrm{N}_2][\mathrm{H}_2]^3} = (8.1320 mol L−1)2(1.5720 mol L−1)(1.9220 mol L−1)3\frac{\left(\frac{8.13}{20}\,\mathrm{mol\,L^{-1}}\right)^2}{\left(\frac{1.57}{20}\,\mathrm{mol\,L^{-1}}\right)\left(\frac{1.92}{20}\,\mathrm{mol\,L^{-1}}\right)^3} = 2.38 × 10310^3
As QcQ_c ≠ KcK_c, the reaction mixture is not in equilibrium.
As QcQ_c > KcK_c, the net reaction will be in the backward direction.
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