Consider the following reactions:
(i) C2O42−→ CO2 (ii) SO42− → SO32−
(iii) MnO42−→ MnO4− (iv) Fe3+→ Fe2+
Choose the correct answer:-
A. (i) & (ii) shows oxidation
B. (iii) & (iv) shows reduction
C. (i) & (iii) shows oxidation
D. (iii) & (iv) shows oxidation
Answers
Answer:
B) (iii) and (iv) shows reduction
Answer:
The unbalanced redox reaction is MnO
4
−
+C
2
O
4
2−
+H
+
→Mn
2+
+CO
2
+H
2
O
Balance C atoms.
MnO
4
−
+C
2
O
4
2−
+H
+
→Mn
2+
+2CO
2
+H
2
O
The oxidation number of Mn decreases from +7 to +2.
The decrease in the oxidation number is 7−2=5
The oxidation number of C increases from +3 to +4.
The increase in the oxidation number for 1 C atom is 4−3=1
The increase in the oxidation number for 2 C atom is 2×1=2
To balance the increase in the oxidation number with decrease in the oxidation number, multiply Mn containing species with 2 and C containing species with 5.
2MnO
4
−
+5C
2
O
4
2−
→2Mn
2+
+10CO
2
Balance O atoms by adding 8 water molecules to the products side.
2MnO
4
−
+5C
2
O
4
2−
→2Mn
2+
+10CO
2
+8H
2
O
Balance H atoms by adding 16 H
+
ions to the reactants side.
2MnO
4
−
+5C
2
O
4
2−
+16H
+
→2Mn
2+
+10CO
2
+8H
2
O
This is the balanced equation.
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