The equilibrium constant, Kc for the reaction
N2(g)+3H2(g) ⇌ 2NH3 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 H2 and 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.
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.
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