[Hemidol]

8. Consider the following net ionic equation for a redox reaction:

2 MnO4 2– + 2 H2O + -> 2 MnO4– + 2 OH– + H2
(a) Which reactant gets oxidized? (b) Which reactant gets reduced?
(c) Which reactant is the oxidizing agent? (d) Which reactant is the reducing agent?


My answers:

(a) MnO4
(b) H2O
(c) H2O
(d) MnO4

Are these correct?

NOTE: In the equation 2 MnO4 2– + 2 H2O + -> 2 MnO4– + 2 OH– + H2 those "-" signs are charges that are superscripts, like "to the power of", I wasn't sure how to make the tags on here using BBCode.


Thanks for reading.

[Borek]

H[ѕub]3[/ѕub]O[ѕup]+[/ѕup] -> H₃O⁺

Answers look OK, that is assuming MnO4 means MnO₄^2-...