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Using the standard reduction potentials , calculate the equilibrium constant for each of the fol- lowing reactions at 298 K: |(a) Fe(s) + Ni²*(aq) → Fe2*(aq) + Ni(s) (b) Co(s) + 2 H*(ag) → Co2* (aq) + H2(8) (c) 10 Br (ag) + 2 MnO, (aq) + 16 H*(aq) 2 Mn2+(aq) + 8 H,0(1) + 5 Br,(1)

Using the standard reduction potentials , calculate the equilibrium constant for each of the fol- lowing reactions at 298 K: |(a) Fe(s) + Ni²*(aq) → Fe2*(aq) + Ni(s) (b) Co(s) + 2 H*(ag) → Co2* (aq) + H2(8) (c) 10 Br (ag) + 2 MnO, (aq) + 16 H*(aq) 2 Mn2+(aq) + 8 H,0(1) + 5 Br,(1)

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.6: Electrochemistry And Thermodynamics
Problem 19.9CYU: Calculate the equilibrium constant at 25 C for the reaction 2 Ag+(aq) + Hg() 2 Ag(s) + Hg2+(aq)
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Using the standard reduction potentials , calculate the equilibrium constant for each of the fol- lowing reactions at 298 K: |(a) Fe(s) + Ni²*(aq) → Fe2*(aq) + Ni(s) (b) Co(s) + 2 H*(ag) → Co2* (aq) + H2(8) (c) 10 Br (ag) + 2 MnO, (aq) + 16 H*(aq) 2 Mn2+(aq) + 8 H,0(1) + 5 Br,(1)
Transcribed Image Text:Using the standard reduction potentials , calculate the equilibrium constant for each of the fol- lowing reactions at 298 K: |(a) Fe(s) + Ni²*(aq) → Fe2*(aq) + Ni(s) (b) Co(s) + 2 H*(ag) → Co2* (aq) + H2(8) (c) 10 Br (ag) + 2 MnO, (aq) + 16 H*(aq) 2 Mn2+(aq) + 8 H,0(1) + 5 Br,(1)
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