Question

Figure out whether the balanced chemical reaction shown below involves oxidation reduction. If it does figure out which element becomes oxidized by the reaction and which element becomes reduced by the reaction. Pick the correct statement about this reaction from the multiple choices.

4 KMnO₄(aq) + 5 CH₃OH(aq) + 12 HCl(aq) 4 MnCl₂(aq) + 5 HCO₂H(aq) + 4 KCl(aq) + 11 H₂O(l)

a) This reaction is not a redox reaction.
b) In this reaction H becomes oxidized and Cl becomes reduced.
c) In this reaction C becomes oxidized and Cl becomes reduced.
d) In this reaction Mn becomes oxidized and C becomes reduced.
e) In this reaction C becomes oxidized and Mn becomes reduced.

How do I assign electrons to each compound?

Answer 1

Answer : e) In this reaction C becomes oxidized and Mn becomes reduced.

Explanation :

4 KMnO₄(aq) + 5 CH₃OH(aq) + 12 HCl(aq) 4 MnCl₂(aq) + 5 HCO₂H(aq) + 4 KCl(aq) + 11 H₂O(l)

oxidation states in reactants :

Mn in KMnO4 = +7

C in CH3OH = - 2

oxidation state in products :

Mn in MnCl2 = +2

C in HCO2H = +2 .

here

Mn reduced from +7 to +2

C oxidized to -2 to + 2