# Problem: Consider the following reaction at a certain temperature:4Fe(s) + 3O2(g) ⇌ 2Fe2O3(s)An equilibrium mixture contains 1.0 mole of Fe, 1.0 x 10-3 mole of O2, and 2.0 moles of Fe2O3 all in a 2.0-L container. Calculate the value of K for this reaction.

🤓 Based on our data, we think this question is relevant for Professor Raja's class at STATEN ISLAND CUNY.

###### FREE Expert Solution

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.

The Kc expression for the reaction is:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{\left[}\mathbf{products}\mathbf{\right]}}{\mathbf{\left[}\mathbf{reactants}\mathbf{\right]}}{\mathbf{=}}\frac{\mathbf{1}}{{\mathbf{\left[}{\mathbf{O}}_{\mathbf{2}}\mathbf{\right]}}^{\mathbf{3}}}}$

5.0 x 10-4 M

###### Problem Details

Consider the following reaction at a certain temperature:

4Fe(s) + 3O2(g) ⇌ 2Fe2O3(s)

An equilibrium mixture contains 1.0 mole of Fe, 1.0 x 10-3 mole of O2, and 2.0 moles of Fe2O3 all in a 2.0-L container. Calculate the value of K for this reaction.