At 286 K and a total equilibrium pressure of 0.972 atm, the fractional dissociation of NO is 0.276 for the reaction2NO(g)N2(g) + O2(g)This means that 276 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp.Kp = When excess Ag metal is added to 0.180 L of 1.380 M Fe³+ (aq) at 298K, the following equilibrium is established:Ag+ (aq) + Fe2+ (aq)Ag(s) + Fe3³+ (aq)(1) If the equilibrium concentration of Ag+ is 0.530 M, what is the value of K?K=(2) Using the value of K from part (1), calculate the new equilibrium concentrations of the three species in solution, if the volume of the solution is increased to 0.497 L by the addition of pure water?[Ag+] =[Fe²+] =[Fe³+] =

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At 286 K and a total equilibrium pressure of 0.972 atm, the fractional dissociation of NO is 0.276 for the reaction 2NO(g) N2(g) + O₂(g) This means that 276 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp

At 286 K and a total equilibrium pressure of 0.972 atm, the fractional dissociation of NO is 0.276 for the reaction 2NO(g) N2(g) + O₂(g) This means that 276 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp

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

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

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Question

At 286 K and a total equilibrium pressure of 0.972 atm, the fractional dissociation of NO is 0.276 for the reaction
2NO(g)
N2(g) + O2(g)
This means that 276 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp.
Kp =

When excess Ag metal is added to 0.180 L of 1.380 M Fe³+ (aq) at 298K, the following equilibrium is established:
Ag+ (aq) + Fe2+ (aq)
Ag(s) + Fe3³+ (aq)
(1) If the equilibrium concentration of Ag+ is 0.530 M, what is the value of K?
K=
(2) Using the value of K from part (1), calculate the new equilibrium concentrations of the three species in solution, if the volume of the solution is increased to 0.497 L by the addition of pure water?
[Ag+] =
[Fe²+] =
[Fe³+] =

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