The question asks me to balance the following redox reaction using the half-reaction method:
HClO (aq) + NO (g) --> Cl1- (aq) + HNO2 (aq) (acidic solution)
For half reaction method:
HClO --> Cl-
NO --> HNO2
1, balance atoms other than H, O, Cl and N are already balanced, so continue
HClO --> Cl-
NO --> HNO2
2, balance O, adding H2O
HClO --> Cl- + H2O
H2O + NO --> HNO2
3, balance H adding H+
H+ + HClO --> Cl- + H2O
H2O + NO --> HNO2 + H+
4, balance charges
2e- + H+ + HClO --> Cl- + H2O
H2O + NO --> HNO2 + H+ + e-
5, balance electrons
2e- + H+ + HClO --> Cl- + H2O
2H2O + 2NO --> 2HNO2 + 2H+ + 2e-
6, add all
2e- + H+ + HClO + 2H2O + 2NO --> Cl- + H2O + 2HNO2 + 2H+ + 2e-
7, cancel common terms
HClO + H2O + 2NO --> Cl- + 2HNO2 + H+
8, verify
H--> 3 in left/right
Cl = 1 in left/right
N = 2 in left/right
O = 4 in left/right
charges: 0 in left, 0 in right
this is already balanced in acidic solution ( i.e. H+ is present)
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