Problem: For the reaction M2 + N2 ⇌ 2MN, scene A represents the mixture at equilibrium, with M black and N orange. If each molecule represents 0.10 mol and the volume is 1.0 L, how many moles of each substance will be present in scene B when that mixture reaches equilibrium?

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FREE Expert Solution

Equilibrium reaction: M₂ + N₂ ⇌ 2MN

When dealing with equilibrium and K_c:

• K_c → equilibrium units are in molarity 
• K_c is an equilibrium expression:

$\boxed{{\mathbf{K}}_{\mathbf{c}}\mathbf{=}\frac{\mathbf{products}}{\mathbf{reactants}}\mathbf{=}\frac{{\left[\mathrm{MN}\right]}^{\mathbf{2}}}{\left[M_2\right]\left[N_2\right]}}$

Solve for K_c using diagram A:

$$\begin{gathered} {\mathbf{K}}_{\mathbf{c}}\mathbf{=}\frac{{\left[\mathbf{0}\mathbf{.}\mathbf{04}\right]}^{\mathbf{2}}}{\left[\mathbf{0}\mathbf{.}\mathbf{02}\right]\left[\mathbf{0}\mathbf{.}\mathbf{02}\right]} \\ {\mathbf{K}}_{\mathbf{c}}\mathbf{=}\frac{\mathbf{1}\mathbf{.}\mathbf{6}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{3}}}{\mathbf{4}\mathbf{.}\mathbf{0}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{4}}} \end{gathered}$$

K_c = 4.0

ICE Chart for diagram B: