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 | Br2 | Br- (1.0 M) || Br- (x M) from [PbBr4]2- | Br2 | Pt Cell H Pt | Br2 | Br- (x M) || BrO3- (0.43 M), H+ (1.00 M) | Br2 | Pt Given: E° for the reduction of Br2 to Br- = +1.07 V > Given that the electrochemical cell L gives a potential of 0.0570 V, determine the concentration of bromide ions present in its cathode half-cell. > Given: Equilibrium concentration of Pb2+ in the cathode of L = 0.15 M and Equilibrium concentration of [PbBr4]2- in the cathode of L = 0.32 M. Determine the equilibrium constant for the formation of [PbBr4]2-. > Given that the electrochemical cell H gives a potential of 0.350 V, determine the standard potential for the reduction of BrO3- to Br2
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 | Br2 | Br- (1.0 M) || Br- (x M) from [PbBr4]2- | Br2 | Pt |
| Cell H |
Pt | Br2 | Br- (x M) || BrO3- (0.43 M), H+ (1.00 M) | Br2 | Pt |
Given: E° for the reduction of Br2 to Br- = +1.07 V
> Given that the
> Given: Equilibrium concentration of Pb2+ in the cathode of L = 0.15 M and Equilibrium concentration of [PbBr4]2- in the cathode of L = 0.32 M. Determine the equilibrium constant for the formation of [PbBr4]2-.
> Given that the electrochemical cell H gives a potential of 0.350 V, determine the standard potential for the reduction of BrO3- to Br2
Step by step
Solved in 7 steps with 2 images
