Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) H,(g)+ Cl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following cc compound concentration at equilibrium HCl 0.73 M H2 1.2M Cl, 0.90 M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K 0 Explanation Check O2022 McGraw H LLC A RIights Reserved. Terms of Use I Pvacy
Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) H,(g)+ Cl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following cc compound concentration at equilibrium HCl 0.73 M H2 1.2M Cl, 0.90 M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K 0 Explanation Check O2022 McGraw H LLC A RIights Reserved. Terms of Use I Pvacy
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 39A
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![Hydrogen chloride decomposes to form hydrogen and chlorine, like this:
2 HCl(g) H,(g) + Cl,(g)
Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition:
compound concentration at equilibrium
HC1
0.73 М
H2
1.2M
Cl2
0.90M
Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
K = []
%3D
10
Explanation
Check
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Transcribed Image Text:Hydrogen chloride decomposes to form hydrogen and chlorine, like this:
2 HCl(g) H,(g) + Cl,(g)
Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition:
compound concentration at equilibrium
HC1
0.73 М
H2
1.2M
Cl2
0.90M
Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
K = []
%3D
10
Explanation
Check
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