# Problem: What is the value of the equilibrium constant at 500 °C for the formation of NH  3 according to the following equation?N2(g) + 3H2(g) ⇌ 2NH3(g)An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 °C was found to contain 1.35 M H 2, 1.15 M N2, and 4.12 × 10−1 M NH3.

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###### FREE Expert Solution

We’re being asked to determine the equilibrium constant at 500˚C for this reaction:

N2(g) + 3 H2(g)  2 NH3(g)

Recall that the equilibrium constant is the ratio of the products and reactants

We use Kp when dealing with pressure and Kc when dealing with concentration:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{products}}}{{\mathbf{P}}_{\mathbf{reactants}}}}$     $\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{\left[}\mathbf{products}\mathbf{\right]}}{\mathbf{\left[}\mathbf{reactants}\mathbf{\right]}}}$

Note that solid and liquid compounds are ignored in the equilibrium expression.

###### Problem Details

What is the value of the equilibrium constant at 500 °C for the formation of NH  3 according to the following equation?

N2(g) + 3H2(g) ⇌ 2NH3(g)

An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 °C was found to contain 1.35 M H 2, 1.15 M N2, and 4.12 × 10−1 M NH3.