Balance the following redox reactions:
$H_{2} O_{2} (a q) + C l O_{4}^{-} (a q) ⟶ O_{2} (g) + C l O_{2}^{-} (a q)$

{3 H}_{2} O_{2} (a q) + 5 C l O_{4}^{-} (a q) ⟶ {2 O}_{2} (g) + 2 C l O_{2}^{-} (a q) + {2 H}_{2} O (l)

No worries! We‘ve got your back. Try BYJU‘S free classes today!

{2 H}_{2} O_{2} (a q) + C l O_{4}^{-} (a q) ⟶ {2 O}_{2} (g) + C l O_{2}^{-} (a q) + {2 H}_{2} O (l)

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

{2 H}_{2} O_{2} (a q) + 5 C l O_{4}^{-} (a q) ⟶ {2 O}_{2} (g) + 6 C l O_{2}^{-} (a q) + {2 H}_{2} O (l)

No worries! We‘ve got your back. Try BYJU‘S free classes today!

{2 H}_{2} O_{2} (a q) + 3 C l O_{4}^{-} (a q) ⟶ {2 O}_{2} (g) + 7 C l O_{2}^{-} (a q) + {2 H}_{2} O (l)

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B ${2 H}_{2} O_{2} (a q) + C l O_{4}^{-} (a q) ⟶ {2 O}_{2} (g) + C l O_{2}^{-} (a q) + {2 H}_{2} O (l)$
The unbalanced chemical equation is as follows:
$H_{2} O_{2} (a q) + C l O_{4}^{-} (a q) ⟶ O_{2} (g) + C l O_{2}^{-} (a q)$
All atoms except H and O are balanced.
The oxidation number of Cl changes from 7 to 3. The change in the oxidation number is 4.
The oxidation number of O changes from -1 to 0. The change in oxidation number per O atom is 1.
Total change in the oxidation number for 2 oxygen atoms is 2.
To balance the increase in oxidation number with decrease in the oxidation number, multiply $H_{2} O_{2}$ and $O_{2}$ with coefficients 2.
$2 H_{2} O_{2} (a q) + C l O_{4}^{-} (a q) ⟶ 2 O_{2} (g) + C l O_{2}^{-} (a q)$
To balance O atoms, add 2 water molecules on RHS.
${2 H}_{2} O_{2} (a q) + C l O_{4}^{-} (a q) ⟶ {2 O}_{2} (g) + C l O_{2}^{-} (a q) + {2 H}_{2} O (l)$
The oxygen atoms are already balanced.
This is the balanced chemical equation.

Suggest Corrections

Similar questions

H_{2} O_{2} (a q)

{C r}_{2} O_{7}^{2 -} (a q)

{C r}^{3 +} (a q)

H_{2} O_{2} (a q) + {C r}_{2} O_{7}^{2 -} ⟶ O_{2} (g) + {C r}^{3 +} (a q)

H_{2} O_{2} (a q)

{M n}^{2 +} (a q)

M n O_{2}

2 K_{4} [F e {(C N)}_{6}] (a q) + H_{2} O_{2} (a q) ⟶ 2 K_{3} [F e {(C N)}_{6}] (a q) + 2 K O H (a q)

Z n (s) + 2 H^{+} (a q) ⟶ Z n^{2 +} (a q) + H_{2} (g)

2 [F e (C N)_{6}]^{3 -} (a q) + 2 O H^{-} (a q) + H_{2} O_{2} (a q) \to 2 [F e (C N)_{6}]^{4 -} (a q) + 2 H_{2} O (l)

2 [F e (C N)_{6}]^{3 -} (a q) + 2 O H^{-} (a q) + H_{2} O_{2} (a q) \to 2 [F e (C N)_{6}]^{4 -} (a q) + O_{2} (g) + 2 H_{2} O (l)

Join BYJU'S Learning Program