In: Chemistry
Balance the following redox reactions
1) SO3-(aq) + MnO4-(aq) ->
SO42-(aq) + Mn2+ (aq) in acidic
solution
2) H2O2(aq) + ClO2(aq) ->
ClO2-(aq) + O2(g) in basic solution
(1)
SO32-(aq) + MnO4-(aq) -> SO42-(aq) + Mn2+ (aq)
(i) Separate the oxidation half and reduction half reactions.
Oxidation half reaction Reduction half reaction
SO32-(aq) --------> SO42-(aq) MnO4-(aq) ---------> Mn2+ (aq)
(ii) Balance atoms ohter than O and H
SO32-(aq) --------> SO42-(aq) MnO4-(aq) ---------> Mn2+ (aq)
(iii) To balance Oxygens in acidic medium add H2O molecules to the side where O's are required.
SO32-(aq) + H2O (l) --------> SO42-(aq) MnO4-(aq) ---------> Mn2+ (aq) + 4 H2O (l)
(iv) To balance hydrogens i acidic medium add H+ ions to the side where H's are required.
SO32-(aq) + H2O (l) --------> SO42-(aq) + 2H+ (aq.) MnO4-(aq) + 8H+(aq.) --------->Mn2+ (aq)+4H2O (v) To balance charge add electrons to the side positive charge is more.
SO32-(aq)+H2O(l) --------> SO42-(aq)+2H+(aq.)+2e MnO4-(aq)+8H+(aq.)+5e ------->Mn2+ (aq)+4H2O
(vi) To balance electrons multiply OHR by 5 and RHR by 2
5SO32-(aq)+5H2O(l)--->5SO42-(aq)+10H+(aq.)+10e 2MnO4-(aq)+16H+(aq.)+10e --->2Mn2+(aq)+8H2O
(vii) Add OHR and RHR to get balanced equation
5SO32-(aq)+5H2O(l)--->5SO42-(aq)+10H+(aq.)+10e
2MnO4-(aq)+16H+(aq.)+10e --->2Mn2+(aq)+8H2O
Balanced equation:
5SO32-(aq) + 2MnO4-(aq) + 6H+(aq.) ------> 5SO42-(aq) + 2Mn2+(aq) + 3 H2O (l)