Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe3+ (aq) + 3 e- → Fe(s) H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1) E' = -0.04 V E' = -0.8698 V K =
Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe3+ (aq) + 3 e- → Fe(s) H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1) E' = -0.04 V E' = -0.8698 V K =
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.127QP
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![Calculate the equilibrium constant, K, for the reaction shown at 25 °C.
Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq)
The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are
Fe3+ (aq) + 3 e- → Fe(s)
H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1)
E' = -0.04 V
E' = -0.8698 V
K =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2ae0572-200a-4e41-9421-873c158e29a5%2Fed420f91-d0c9-45d4-87dc-7d823e6b7908%2F9wi818a_processed.png&w=3840&q=75)
Transcribed Image Text:Calculate the equilibrium constant, K, for the reaction shown at 25 °C.
Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq)
The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are
Fe3+ (aq) + 3 e- → Fe(s)
H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1)
E' = -0.04 V
E' = -0.8698 V
K =
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