rules for balancing redox reaction by oxidation number method and ion electron method
Answers
Answer:
The unbalanced chemical equation is given below:
S
2−
(aq)+I
2
(s)⟶SO
4
2−
(aq)+I
−
(aq)
Balance all atoms except H and O,
S
2−
(aq)+4I
2
(s)⟶SO
4
2−
(aq)+8I
−
(aq)
The oxidation number of S changes from −2 to +6.
The net change in the oxidation number is 8.
The oxidation number of iodine changes from 0 to −1.
The net change in the oxidation number per I atom is 1.
Total change in the oxidation number for 8 I atoms is 8.
Thus, the increase in the oxidation number is equal to the decrease in the oxidation number.
Balance O atoms by adding 4 water molecules to LHS,
S
2−
(aq)+4I
2
(s)+4H
2
O(l)⟶8I
−
(aq)+SO
4
2−
(aq)
Balance H atoms by adding 8 H
+
to the RHS,
S
2−
(aq)+4I
2
(s)+4H
2
O(l)⟶8I
−
(aq)+SO
4
2−
(aq)+8H
+
(aq)
This is the balanced chemical equation.
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Can You Solve These Questions?
In the following redox reactions, what is the value of f?
I. aMnO
4
−
+bFe
2+
+cH
+
⟶dMn
2+
+eFe
3+
+fH
2
O
II. aCr
2
O
7
2−
+bFe
2+
+cH
+
⟶dCr
3+
+eFe
3+
+fH
2
O
III. aMnO
4
−
+bH
2
O
2
+cH
+
⟶dMn
2+
+eO
2
+fH
2
O
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View Answer
Balance the following equation by ion electron method.
MnO
4
−
+H
+
+H
2
O
2
→Mn
2+
+H
2
O+O
2