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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
\[\ce{N2 (g) + 3H2 (g)⇌2NH3 (g)}\] is 1.7 × 102
Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?
Solution
The given reaction is:
\[\ce{N2 (g) + 3H2 (g)⇌2NH3 (g)}\]
The given concentration of various species is
`["N"_2] = 1.57/20 "mol L"^(-1) ["H"_2] = 1.92/20 " mol L"^(-1)`
`["NH"_3] = 8.13/20 " mol L"^(-1)`
Now, reaction quotient Qc is:
`"Q"_"c" = (["NH"_3]^2)/(["N"_2]["H"_2]^3)`
`= ((8.13)/20)^2/((1.57/20)(1.92/20)^3`)
`= 2.4 xx 10^3`
Since `"Q"_"c" != "K"_"C"` the reaction mixture is not at equilibrium.
Again, `"Q"_"c" > "K"_"c"` Hence, the reaction will proceed in the reverse direction.
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