Question

Upper n subscript 2 (g) plus 3 upper H subscript 2 (g) double-headed arrow 2 upper N upper H subscript 3 (g). At equilibrium, the concentrations of the different species are as follows. [NH3] = 0.105 M [N2] = 1.1 M [H2] = 1.50 M

Answer 1

Answer:

The equilibrium constant is:

              $k_c=0.0030M^{-2}$

Explanation:

The correct equation is:

•   N₂(g)    +    3H₂(g)    ⇄    2NH₃(g)

Thus, with the equilibrium concentrations you can calculate the equilibrium constant, Kc.

The equation for the equilibrium constant is:

         $k_c=\dfrac{[NH_3]^2}{[N_2]\cdot [H_2]^3}$

Substituting:

        $k_c=\dfrac{(0.105M)^2}{(1.1M)\cdot (1.50M)^3}$

         $k_c=0.0030M^{-2}$