Using the mechanism below, what would be the appropriate equilibrium constant expression for the overall reaction? Step 1: H(aq) + H₂O2(aq) → H3O₂ (aq) Step 2: H3O₂ (aq) + Br (aq) → HOBr(aq) + H₂0(1) Step 3: HOBr(aq) + H*(aq) + Br (aq) → Br₂(aq) + H₂O(1) K= K= K = K= [Br₂] [H₂O]2 [H+]2[Br]2 [H₂O₂] [H+]2[Br]2 [H₂O₂] [Br₂] [Br₂] [H+][Br] [H₂O₂] [Br₂] [H+12[Br-12 [H₂O₂] fast slow fast

Select one for each box

The addition of concentrated nitric acid to each standard solution... Select all that are True. changes the potential of the reference electrode. results in a low pH, which is required for this experiment. results in a wet acid digestion to ensure sample dissolution. results in a relatively constant ionic strength across the standard solutions. results in the required amount of excess nitrate ion. Tries 3/6 Previous Tries

Can it please be explain just like in the upload