Suppose a 250. mL flask is filled with 0.70 mol of H₂ and 0.60 mol of HCI. The following reaction becomes possible: H2(g) + Cl2(g) 2HCI (g) - The equilibrium constant K for this reaction is 0.156 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places. M X
Suppose a 250. mL flask is filled with 0.70 mol of H₂ and 0.60 mol of HCI. The following reaction becomes possible: H2(g) + Cl2(g) 2HCI (g) - The equilibrium constant K for this reaction is 0.156 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places. M X
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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
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.70 mol of H₂ and 0.60 mol of HCI. The following reaction becomes possible:
H2(g) + Cl2(g) 2HCI (g)
-
The equilibrium constant K for this reaction is 0.156 at the temperature of the flask.
Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
M
X
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