Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.60 mol of Cl₂. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HC1 (g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X Ś
Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.60 mol of Cl₂. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HC1 (g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X Ś
World of Chemistry, 3rd edition
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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 17A
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![Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.60 mol of Cl₂. The following reaction becomes possible:
H₂(g) + Cl₂(g) → 2HC1 (g)
The equilibrium constant K for this reaction is 1.94 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
1
M
X
Ś](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F567b32ff-1565-4059-aab2-63807bc888d8%2Fae6835ab-3f68-4ca0-bfca-2f8c8d1b2fc1%2Fy3fqil8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.60 mol of Cl₂. The following reaction becomes possible:
H₂(g) + Cl₂(g) → 2HC1 (g)
The equilibrium constant K for this reaction is 1.94 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
1
M
X
Ś
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