Calculate K_c for the reaction Br₂ + H₂O→H⁺ + Br ^- + HOBr at 25 ° C given:
HOBr + H⁺ + 2 e^-→Br^- + H₂O E ° = +1.33 V Br₂ + 2 e^-→2 Br^- E ° = +1.07 V

Question

Calculate K_c for the reaction Br₂ + H₂O→H⁺ + Br ^- + HOBr at 25 ° C given: HOBr + H⁺ + 2 e^-→Br^- + H₂O E ° = +1.33 V Br₂ + 2 e^-→2 Br^- E ° = +1.07 V

Quizplus · Accepted Answer

The correct answer is A because the equilibrium constant for a reaction is related to the standard reduction potentials of the half-reactions involved in the reaction. The more positive the standard reduction potential, the more favorable the reaction is. In this case, the standard reduction potential for the half-reaction involving the reduction of Br2 is more positive than the standard reduction potential for the half-reaction involving the reduction of HOBr. This means that the reaction Br2 + H2O→H+ + Br- + HOBr is more favorable than the reverse reaction, and therefore the equilibrium constant for the reaction will be greater than 1.

Calculate Kc for the Reaction Br2 + H2O→H+ + Br

Calculate K_c for the Reaction Br₂ + H₂O→H⁺ + Br