The equilibrium constant, \( K \), for the following reaction is 10.5 at 350 K.\[ 2\text{CH}_2\text{Cl}_2(\text{g}) \rightleftharpoons \text{CH}_4(\text{g}) + \text{CCl}_4(\text{g}) \]An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains \( 5.43 \times 10^{-2} \) M \(\text{CH}_2\text{Cl}_2\), 0.176 M \(\text{CH}_4\), and 0.176 M \(\text{CCl}_4\). What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.108 mol of \(\text{CCl}_4(\text{g})\) is added to the flask?\[[\text{CH}_2\text{Cl}_2] = \, \underline{\hspace{2cm}} \, \text{M}\]\[[\text{CH}_4] = \, \underline{\hspace{2cm}} \, \text{M}\]\[[\text{CCl}_4] = \, \underline{\hspace{2cm}} \, \text{M}\]

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Answered: The equilibrium constant, K, for the…

Chemistry

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

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Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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