please answer all Student A prepared a concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]²- asthe source of bromide ions. On the other hand, Student B prepared a galvanic cell (H), where the bromide ionconcentration in the anode is equal to that in the cathode of cell L.Cell LPt(s) | Br21) | Br (ag) (1.0 M) || Br-(ag) (x M) from [PbBr4] (ag) Br2(1) | Pt(s)Cell HPt(s) | Br21) | Br(ag) (x M) || BrO3(aq) (0.43 M), H*(ag) (1.00 M) | Br2) | Pt(s)Given: Ereduction Br2(/Br-(ag) = 1.07 V c) Write the overall redox reaction for the electrochemical cell H.d) Given that the electrochemical cell H gives a potential of 0.350 V, determine the standard potential forthe reduction of BrO3 (ag) to Br2(1).

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Student A prepared a concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]²- as the source of bromide ions. On the other hand, Student B prepared a galvanic cell (H), where the bromide ion concentration in the anode is equal to that in the cathode of cell L. Cell L Pt(s) | Br2) | Br (39) (1.0 M) || Br-(ag) (x M) from [PbBr4] (ag) Br2(1) | Pt(s) Cell H Pt(s) | Br21) | Br (ag) (x M) || BrO3 (ag) (0.43 M), H(aq) (1.00 M) | Br2) | Pt(s) Given: Ereduction Br2)/Br-(ag) = 1.07 V

Student A prepared a concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]²- as the source of bromide ions. On the other hand, Student B prepared a galvanic cell (H), where the bromide ion concentration in the anode is equal to that in the cathode of cell L. Cell L Pt(s) | Br2) | Br (39) (1.0 M) || Br-(ag) (x M) from [PbBr4] (ag) Br2(1) | Pt(s) Cell H Pt(s) | Br21) | Br (ag) (x M) || BrO3 (ag) (0.43 M), H(aq) (1.00 M) | Br2) | Pt(s) Given: Ereduction Br2)/Br-(ag) = 1.07 V

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.4QAP: Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose...

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