The equilibrium constant for dissociation of dinitrogen tetroxide N2O4(g) ↔ 2 NO2(g) is KP = 0.308763 at 298.0 K If the total equilibrium pressure at 298.0 K is 0.86 bar, what is the partial pressure of NO2(g)?
The equilibrium constant for dissociation of dinitrogen tetroxide N2O4(g) ↔ 2 NO2(g) is KP = 0.308763 at 298.0 K If the total equilibrium pressure at 298.0 K is 0.86 bar, what is the partial pressure of NO2(g)?
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...
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The equilibrium constant for dissociation of dinitrogen tetroxide
N2O4(g) ↔ 2 NO2(g)
is KP = 0.308763 at 298.0 K
If the total equilibrium pressure at 298.0 K is 0.86 bar, what is the partial pressure of NO2(g)?
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