Suppose a 500 ml. flask is filled with 1.4 mol of 12 and 1.3 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant & for this reaction is 6.76 at the temperature of the flask, Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.

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
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Suppose a 500 mL. flask is filled with 1.4 mol of 1₂ and 1.3 mol of HI. The following reaction becomes possible:
H₂(g) +1₂(g) → 2H1 (g)
The equilibrium constant X for this reaction is 6.76 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
Transcribed Image Text:Suppose a 500 mL. flask is filled with 1.4 mol of 1₂ and 1.3 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2H1 (g) The equilibrium constant X for this reaction is 6.76 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
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