A student ran the following reaction in the laboratory at 427 K: PCl5(g) PCl3(g) + Cl2(g) When she introduced 4.21 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of PCl5(g) to be 4.17 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 427 K: PCl5(g) PCl3(g) + Cl2(g) When she introduced 4.21 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of PCl5(g) to be 4.17 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
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 41QRT: Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures.
2 NOCl(g) ⇌ 2 NO(g) +...
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A student ran the following reaction in the laboratory at 427 K:
PCl5(g) PCl3(g) + Cl2(g)
When she introduced 4.21 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of PCl5(g) to be 4.17 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
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