🤓 Based on our data, we think this question is relevant for Professor Sharma's class at UM.

$\overline{){\mathbf{K}}_{\mathbf{c}}\mathbf{}\mathbf{=}\frac{\left[C\right]}{\mathbf{\left[}\mathbf{A}\mathbf{\right]}\mathbf{\left[}\mathbf{B}\mathbf{\right]}}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{4}\mathbf{}\mathbf{=}\frac{\mathbf{x}}{(1.0-x)(1.0-x)}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{4}\mathbf{(}\mathbf{1}\mathbf{.}\mathbf{0}\mathbf{-}\mathbf{x}\mathbf{)}(1.0-x)\mathbf{}\mathbf{=}\mathbf{}\mathbf{x}$

Consider the following reaction and associated equilibrium constant: aA(g) + bB(g) ⇌ cC(g); K_{c} = 4.0

Find the equilibrium concentrations of A, B, and C for a = 1, b = 1, and c = 1. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction.