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Consider the following reaction: 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) If 0.436 moles of CH₂Cl2 (g), 0.335 moles of CH4, and 0.406 moles of CC14 are at equilibrium in a 17.4 L container at 599 K, the value of the equilibrium constant, Kc, is

Consider the following reaction: 2CH₂Cl2 (9) CH4 (9) + CCl4 (9) If 0.436 moles of CH₂Cl2 (g), 0.335 moles of CH4, and 0.406 moles of CC14 are at equilibrium in a 17.4 L container at 599 K, the value of the equilibrium constant, Kc, is

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
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Consider the following reaction: 2CH₂Cl₂ (9) ⇒ CH4 (9) + CCl4 (9) If 0.436 moles of CH₂ Cl2 (g), 0.335 moles of CH4, and 0.406 moles of CC14 are at equilibrium in a 17.4 L container at 599 K, the value of the equilibrium constant, Ke, is
Transcribed Image Text:Consider the following reaction: 2CH₂Cl₂ (9) ⇒ CH4 (9) + CCl4 (9) If 0.436 moles of CH₂ Cl2 (g), 0.335 moles of CH4, and 0.406 moles of CC14 are at equilibrium in a 17.4 L container at 599 K, the value of the equilibrium constant, Ke, is
Expert Solution
Step 1

Given,

number of moles of CH2Cl2 = 0.436 mol

number of moles of CH4 = 0.335 mol

number of moles of CCl4 = 0.406 mol

The volume of the container = 17.4 L

 

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