Problem: Given the following half-reactions and associated standard reduction potentials:AuBr4-(aq) + 3e-  →  Au(s) + 4Br-(aq)Eredo= - 0.858VEu3+(aq) + e-  →  Eu2+(aq)Eredo= - 0.43VIO-(aq) + H2O(l) + 2e-  →  I-(aq) + 2OH-(aq)Eredo= + 0.49VSn2+(aq) + 2e-  →  Sn(s)Eredo= - 0.14VWrite the cell reaction for the combination of these half-cell reactions that leads to the largest positive cell emf.

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We’re being asked to determine which among half-cell reactions that lead to the largest positive cell emf.

When a balanced reaction is given, identify the anode and the cathode half-reactions by determining the changes in oxidation states of each species based on the given reaction:

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Given the following half-reactions and associated standard reduction potentials:
AuBr4-(aq) + 3e-  →  Au(s) + 4Br-(aq)
Eredo= - 0.858V
Eu3+(aq) + e-  →  Eu2+(aq)
Eredo= - 0.43V
IO-(aq) + H2O(l) + 2e-  →  I-(aq) + 2OH-(aq)
Eredo= + 0.49V
Sn2+(aq) + 2e-  →  Sn(s)
Eredo= - 0.14V

Write the cell reaction for the combination of these half-cell reactions that leads to the largest positive cell emf.

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