🤓 Based on our data, we think this question is relevant for Professor Randles' class at UCF.
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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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.
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Based on our data, we think this problem is relevant for Professor Randles' class at UCF.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.