A mixture of 0.585 M \( \text{H}_2\text{O} \), 0.455 M \( \text{Cl}_2\text{O} \), and 0.715 M \( \text{HClO} \) are enclosed in a vessel at 25°C.\[ \text{H}_2\text{O(g)} + \text{Cl}_2\text{O(g)} \rightleftharpoons 2 \text{HOCl(g)} \quad K_c = 0.0900 \text{ at } 25°C \]Calculate the equilibrium concentrations of each gas at 25°C.\[\begin{align*}[\text{H}_2\text{O}] &= \hspace{4cm} \text{M} \\[\text{Cl}_2\text{O}] &= \hspace{4cm} \text{M} \\[\text{HOCl}] &= \hspace{4cm} \text{M}\end{align*}\]

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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A mixture of 0.585 M \( \text{H}_2\text{O} \), 0.455 M \( \text{Cl}_2\text{O} \), and 0.715 M \( \text{HClO} \) are enclosed in a vessel at 25°C.

\[ \text{H}_2\text{O(g)} + \text{Cl}_2\text{O(g)} \rightleftharpoons 2 \text{HOCl(g)} \quad K_c = 0.0900 \text{ at } 25°C \]

Calculate the equilibrium concentrations of each gas at 25°C.

\[
\begin{align*}
[\text{H}_2\text{O}] &= \hspace{4cm} \text{M} \\
[\text{Cl}_2\text{O}] &= \hspace{4cm} \text{M} \\
[\text{HOCl}] &= \hspace{4cm} \text{M}
\end{align*}
\]

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Here a mixture of 0.585 H2O ,0.455 M Cl2O and 0.715M HClO are enclosed in a vessel at 25°C. We have to determine the equilibrium concentrations of each species if equilibrium constant is 0.09 at 25°C..

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