At high temperatures, iodine molecules can dissociate into iodineatoms. For the reaction12(g) = 21.(g)Kc = 1.27 x 10-4 at 900 °C. A 65.5 g sample of l2 is placed in a 1.00 Lvessel and heated to 900 °C. What will be the molar concentration ofiodine atoms, [1.], in the vessel when the system comes toequilibrium?

Answer: Value of equilibrium constant KC is equal to the ratio of molar concentration of products…

At high temperatures, iodine molecules can dissociate into iodine atoms. For the reaction 1₂(g) = 21 (g) Kc = 1.27 x 10-4 at 900 °C. A 65.5 g sample of l₂ is placed in a 1.00 L vessel and heated to 900 °C. What will be the molar concentration of iodine atoms, [I.], in the vessel when the system comes to equilibrium?

At high temperatures, iodine molecules can dissociate into iodine atoms. For the reaction 1₂(g) = 21 (g) Kc = 1.27 x 10-4 at 900 °C. A 65.5 g sample of l₂ is placed in a 1.00 L vessel and heated to 900 °C. What will be the molar concentration of iodine atoms, [I.], in the vessel when the system comes to equilibrium?

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 45A

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