At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases. At this temperature, K=0.0169 . What are the partial pressures at equilibrium of the hydrogen and iodine if initially a sealed flask at 800 K contains only HI at a pressure of 0.242 atm? 2.4)[References]At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases.2HI(g) = I2 (9) + H2 (g)At this temperature, K = 0.0169. What are the partial pressures at equilibrium of the hydrogen and iodine if initially a sealed flask at 800 K contains only HI at a pressure of 0.242 atm?Partial pressure of hydrogen =atmPartial pressure of iodine =atmSubmit AnswerTry Another Version4 item attempts remaining

The reaction is: H2 (g) + I2 (g) → 2 HI (g) K is 0.0169 Initial partial pressures of hydrogen gas…

At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases. 2HI(9) =12(9) +H2(9) At this temperature, K = 0.0169. What are the partial pressures at equilibrium of the hydrogen and iodine if initially a sealed flask at 800 K contains only HI at a pressure of 0.242 atm? Partial pressure of hydrogen = atm Partial pressure of iodine = atm

At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases. 2HI(9) =12(9) +H2(9) At this temperature, K = 0.0169. What are the partial pressures at equilibrium of the hydrogen and iodine if initially a sealed flask at 800 K contains only HI at a pressure of 0.242 atm? Partial pressure of hydrogen = atm Partial pressure of iodine = atm

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...

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