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Suppose a 500. ml flask is filled with 0.50 mol of H₂ and 0.20 mol of HCI. The following reaction becomes possible: H₂(g) + Cl₂ (g) 2HCl(g) 1 The equilibrium constant K for this reaction is 7.23 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. 2 M X Ś

Suppose a 500. ml flask is filled with 0.50 mol of H₂ and 0.20 mol of HCI. The following reaction becomes possible: H₂(g) + Cl₂ (g) 2HCl(g) 1 The equilibrium constant K for this reaction is 7.23 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. 2 M X Ś

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.52QE: Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium...
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Suppose a 500. mL. flask is filled with 0.50 mol of H₂ and 0.20 mol of HCI. The following reaction becomes possible: H₂(g) + Cl₂ (g) 2HCl(g) 1 The equilibrium constant K for this reaction is 7.23 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X Ś
Transcribed Image Text:Suppose a 500. mL. flask is filled with 0.50 mol of H₂ and 0.20 mol of HCI. The following reaction becomes possible: H₂(g) + Cl₂ (g) 2HCl(g) 1 The equilibrium constant K for this reaction is 7.23 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X Ś
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