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:
cathode → reduction → oxidation number decreases
anode → oxidation → oxidation number increases
For ions: charge of the ion = oxidation number
For neutral atoms/compound: oxidation number = 0
Determine the half-cell potentials (refer to the Standard Reduction Potential Table)
F2 + 2 e- → 2 F- E°cell = 2.87 V
MnO4- + 8H+ + 5 e- → Mn2+ + 4 H2O E°cell = 1.51 V
Calculate E° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in Table 17‑1.
b. MnO4- (aq) + F - (aq) → F2 (aq) + Mn2+ (aq)
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.