The equilibrium constant, K, for the following reaction is 9.52×102 at 350 K: CH4(g) + CCl4(g)2CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.207 moles of CH4 and 0.207 moles of CCI are introduced into a 1.00 L vessel at 350 K. [CH4] [CCl4] [CH2Cl2] = = M Σ Σ Σ Submit Answer 2 question attempts remaining
The equilibrium constant, K, for the following reaction is 9.52×102 at 350 K: CH4(g) + CCl4(g)2CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.207 moles of CH4 and 0.207 moles of CCI are introduced into a 1.00 L vessel at 350 K. [CH4] [CCl4] [CH2Cl2] = = M Σ Σ Σ Submit Answer 2 question attempts remaining
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 56QRT
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