Calculating equilibrium composition from an equilibrium constantSuppose a 250. mL flask is filled with 0.10 mol of H₂ and 1.6 mol of HCl. The following reaction becomes possible:H₂(g) + Cl₂(g) → 2HCl(g)The equilibrium constant K for this reaction is 0.280 at the temperature of the flask.Calculate the equilibrium molarity of C1₂. Round your answer to two decimal places.ШмMŚ

Molarity can be calculated by dividing number of moles by volume. Here, volume of the flask = 250 mL…

se a 250. mL flask is filled with 0.10 mol of H₂ and 1.6 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) quilibrium constant K for this reaction is 0.280 at the temperature of the flask. ate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M X S

se a 250. mL flask is filled with 0.10 mol of H₂ and 1.6 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) quilibrium constant K for this reaction is 0.280 at the temperature of the flask. ate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M X S

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 61QRT

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