**Equilibrium Constant Calculation at 539 K**Consider the following equilibrium system at 539 K:\[ \text{2CH}_2\text{Cl}_2(g) \rightleftharpoons \text{CH}_4(g) + \text{CCl}_4(g) \]If an equilibrium mixture of the three gases at 539 K contains \(4.99 \times 10^{-2} \, \text{M CH}_2\text{Cl}_2\), \(5.54 \times 10^{-2} \, \text{M CH}_4\), and \(4.90 \times 10^{-2} \, \text{M CCl}_4\), what is the value of the equilibrium constant \(K\)?\[ K = \](In this context, "M" denotes molarity, which is moles per liter.)

Consider the following equilibrium system at 539 K. 2CH2C12 (g) 2 CH, (g) + CCL4 (g) If an equilibrium mixture of the three gases at 539 K contains 4.99 × 10-² M CH2C12, 5.54 × 10-2 M CH4, and 4.90 × 10-2 M CC14, what is the value of the equilibrium constant K?

Consider the following equilibrium system at 539 K. 2CH2C12 (g) 2 CH, (g) + CCL4 (g) If an equilibrium mixture of the three gases at 539 K contains 4.99 × 10-² M CH2C12, 5.54 × 10-2 M CH4, and 4.90 × 10-2 M CC14, what is the value of the equilibrium constant K?

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

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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Question

**Equilibrium Constant Calculation at 539 K**

Consider the following equilibrium system at 539 K:

\[ \text{2CH}_2\text{Cl}_2(g) \rightleftharpoons \text{CH}_4(g) + \text{CCl}_4(g) \]

If an equilibrium mixture of the three gases at 539 K contains \(4.99 \times 10^{-2} \, \text{M CH}_2\text{Cl}_2\), \(5.54 \times 10^{-2} \, \text{M CH}_4\), and \(4.90 \times 10^{-2} \, \text{M CCl}_4\), what is the value of the equilibrium constant \(K\)?

\[ K = \]

(In this context, "M" denotes molarity, which is moles per liter.)

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