# Problem: The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4- ions by periodate ion (IO4-) in acid solution.b. Calculate E° and ΔG° at 25°C for each reaction.

###### FREE Expert Solution

Write the half cell reactions:

IO4-  + 2 H+ 2 e→   IO3-  +  H2O                    E° = 1.60 V (reduction → cathode)

MnO4+ 8 H+  + 5e- →  Mn2+  + 4 H2          E° = 1.51 V (oxidation → anode)

81% (14 ratings) ###### Problem Details

The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4- ions by periodate ion (IO4-) in acid solution.

b. Calculate E° and ΔG° at 25°C for each reaction.

Frequently Asked Questions

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.

What textbook is this problem found in?

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.