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A student ran the following reaction in the laboratory at 543 K: PCI3(g) + Cl2(g) =PCI5(g) When she introduced 6.64x10-2 moles of PCI3(g) and 8.35x10-2 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 5.24x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc = Submit Answer Retry Entire Group No more group attempts remain

A student ran the following reaction in the laboratory at 543 K: PCI3(g) + Cl2(g) =PCI5(g) When she introduced 6.64x10-2 moles of PCI3(g) and 8.35x10-2 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 5.24x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc = Submit Answer Retry Entire Group No more group attempts remain

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
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 53QRT: Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15...
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A student ran the following reaction in the laboratory at 543 K: PCI3(g) + Cl2(g) =PCI5(g) When she introduced 6.64x10-2 moles of PCI2(g) and 8.35×10-2 moles of Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of Cl,(g) to be 5.24x10 2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = Submit Answer Retry Entire Group No more group attempts remain
Transcribed Image Text:A student ran the following reaction in the laboratory at 543 K: PCI3(g) + Cl2(g) =PCI5(g) When she introduced 6.64x10-2 moles of PCI2(g) and 8.35×10-2 moles of Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of Cl,(g) to be 5.24x10 2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = Submit Answer Retry Entire Group No more group attempts remain
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