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Suppose a 500. mL flask is filled with 1.8 mol of H₂ and 1.4 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) 2HCI(g) The equilibrium constant K for this reaction is 0.142 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. M

Suppose a 500. mL flask is filled with 1.8 mol of H₂ and 1.4 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) 2HCI(g) The equilibrium constant K for this reaction is 0.142 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. M

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 38A
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Suppose a 500. mL flask is filled with 1.8 mol of H₂ and 1.4 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 0.142 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. M X
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.8 mol of H₂ and 1.4 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 0.142 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. M X
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