Step 1

$\left[\mathrm{HOCl}\right]\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{1}\mathbf{.}\mathbf{0}\mathbf{}\mathbf{mol}}{\mathbf{2}\mathbf{.}\mathbf{0}\mathbf{}\mathbf{L}}$** = 0.5 M**

Step 2

Step 3

${\mathbf{K}}_{\mathbf{c}}\mathbf{}\mathbf{=}\mathbf{}\frac{{\mathbf{\left[}\mathbf{HOCl}\mathbf{\right]}}^{\mathbf{2}}}{\mathbf{\left[}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\right]}\mathbf{\left[}{\mathbf{Cl}}_{\mathbf{2}}\mathbf{\right]}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{090}\mathbf{}\mathbf{=}\mathbf{}\frac{{\mathbf{(}\mathbf{0}\mathbf{.}\mathbf{5}\mathbf{}\mathbf{-}\mathbf{}\mathbf{2}\mathbf{x}\mathbf{)}}^{\mathbf{2}}}{\mathbf{\left(}\mathbf{x}\mathbf{\right)}\mathbf{\left(}\mathbf{x}\mathbf{\right)}}\phantom{\rule{0ex}{0ex}}\sqrt{\mathbf{0}\mathbf{.}\mathbf{090}\mathbf{}}\mathbf{=}\mathbf{}\sqrt{\frac{{\mathbf{(}\mathbf{0}\mathbf{.}\mathbf{5}\mathbf{}\mathbf{-}\mathbf{}\mathbf{2}\mathbf{x}\mathbf{)}}^{\mathbf{2}}}{{\mathbf{\left(}\mathbf{x}\mathbf{\right)}}^{\mathbf{2}}}}$

At 25ºC, *K* = 0.090 for the reaction

H_{2}O(*g*) + Cl_{2}O(*g*) ⇌ 2HOCl(*g*)

Calculate the concentrations of all species at equilibrium for each of the following cases.

b. 1.0 mole of pure HOCl is placed in a 2.0-L flask.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Lazaridis' class at CCNY.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.