ANSWER : C) H + = 2 & H2O = 1
Consider given reaction, Bi2O3 (s) + OCl - (aq) Cl - (aq) + BiO3- (aq)
Oxidation no. of Bi changes from +3 to +5 , hence it is oxidized. We can write oxidation half equation as
Bi2O3 (s) BiO3- (aq)
Oxidation no. of Cl changes from +1 to -1 , hence Cl is reduced. We can write reduction half equation as
OCl - (aq) Cl - (aq)
Now, balance the half equations for atoms other than O and H.
Oxidation : Bi2O3 (s) 2 BiO3- (aq)
Reduction : OCl - (aq) Cl - (aq)
Balance half equations for O atoms by adding H2O to the side of half equations with less number of O atoms.
Oxidation : Bi2O3 (s) + 3 H2O (l) 2 BiO3- (aq)
Reduction : OCl - (aq) Cl - (aq) + H2O (l)
Balance half equations for H atoms by adding H + to the side of half equations with less number of H atoms.
Oxidation : Bi2O3 (s) + 3 H2O (l) 2 BiO3- (aq) + 6 H + (aq)
Reduction : OCl - (aq) + 2 H + (aq) Cl - (aq) + H2O (l)
Balance half equations for charge by adding electrons. Charge on L.H.S must be equal to R.H.S of half equation.
Oxidation : Bi2O3 (s) + 3 H2O (l) 2 BiO3- (aq) + 6 H + (aq) + 4 e -
Reduction : OCl - (aq) + 2 H + (aq) + 2 e - Cl - (aq) + H2O (l)
To make electrons equal in both equation, multiply reduction half equation by 2.
Oxidation : Bi2O3 (s) + 3 H2O (l) 2 BiO3- (aq) + 6 H + (aq) + 4 e -
Reduction : 2 OCl - (aq) + 4 H + (aq) + 4 e - 2 Cl - (aq) + 2 H2O (l)
Add two equations to get overall equation.
Bi2O3 (s) + 3 H2O (l) 2 BiO3- (aq) + 6 H + (aq) + 4 e -
2 OCl - (aq) + 4 H + (aq) + 4 e - 2 Cl - (aq) + 2 H2O (l)
Overall : Bi2O3 (s) + 2 OCl - (aq) + H2O (l) 2 BiO3- (aq) + 2 Cl - (aq) + 2 H + (aq)
ANSWER : H + = 2 & H2O = 1
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