The following concentrations were obtained for the formation of NH3 fr

1.	The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K. [N2] = 1.5 x 10-2 M, [H2] = 3.0 x 10-2 M and [NH3] = 1.2 x 10-2 M. Calculate equilibrium constant.
Answer» For the reaction, N₂ (g) + 3H₂ (g) ⇌ 2NH₃(g) Equilibrium constant K_c = \(\frac{[NH_3]^2}{[N_2][H_2]^3}\) = \(\frac{(1.2\times10^{-2})^2}{(1.5\times10^{-12})(3\times10^{-2})^3}\) = 0.106 x 10⁴ = 1.06 x 10³

The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K. [N2] = 1.5 x 10-2 M, [H2] = 3.0 x 10-2 M and [NH3] = 1.2 x 10-2 M. Calculate equilibrium constant.

Answer»

For the reaction,

N₂ (g) + 3H₂ (g) ⇌ 2NH₃(g)

Equilibrium constant

K_c = \(\frac{[NH_3]^2}{[N_2][H_2]^3}\)

= \(\frac{(1.2\times10^{-2})^2}{(1.5\times10^{-12})(3\times10^{-2})^3}\)

= 0.106 x 10⁴

= 1.06 x 10³

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The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500K. [N2] = 1.5 x 10-2 M, [H2] = 3.0 x 10-2 M and [NH3] = 1.2 x 10-2 M. Calculate equilibrium constant.

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