At a certain temperature, the K₂ for the decomposition of H₂S is 0.704.H₂S(g) = H₂(g) + S(g)Initially, only H₂S is present at a pressure of 0.260 atm in a closed container. What is the total pressure in the containerat equilibrium?Ptotal =atm At equilibrium, the concentrations in this system were found to be [N₂] = [O₂] = 0.200 M and [NO] = 0.500 M.N₂(g) + O₂(g) = 2 NO(g)If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibriumis re-established?[NO] final0.550IncorrectM

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At a certain temperature, the Kp for the decomposition of H₂S is 0.704. H₂S(g) → H₂(g) + S(g) Initially, only H₂S is present at a pressure of 0.260 atm in a closed container. What is the total pressure in the container at equilibrium? Ptotal = atm

At a certain temperature, the Kp for the decomposition of H₂S is 0.704. H₂S(g) → H₂(g) + S(g) Initially, only H₂S is present at a pressure of 0.260 atm in a closed container. What is the total pressure in the container at equilibrium? Ptotal = 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 33P

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