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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

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter17: Solubility And Complex-ion Equilibria
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Problem 17.103QP: Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia....
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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 =
Transcribed Image Text: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+] =
Transcribed Image Text: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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