At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases. 2HI (g) ---> <----- I2 (g) + 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 at a pressure of 0.213 atm? Partial pressure of hydrogen = _____ atm Partial pressure of iodine = _____ atm
At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases. 2HI (g) ---> <----- I2 (g) + 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 at a pressure of 0.213 atm? Partial pressure of hydrogen = _____ atm Partial pressure of iodine = _____ atm
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 76AP: Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the...
Related questions
Question
At 800 K, hydrogen iodide can decompose into hydrogen and iodine gases.
2HI (g) ---> <----- I2 (g) + 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 at a pressure of 0.213 atm?
Partial pressure of hydrogen = _____ atm
Partial pressure of iodine = _____ atm
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax