balance the redox reaction Cr2O7 -²+I- –––> I2 +Cr+³.
Answers
Answer:
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Answer:
Cr
2
O
7
2−
(aq)+3NO
2
−
(aq)+8H
+
(aq)⟶2Cr
3+
(aq)+3NO
3
−
(aq)+4H
2
O(l)
The unbalanced chemical equation is as follows:
Cr
2
O
7
2−
(aq)+HNO
2
(aq)⟶Cr
3+
(aq)+NO
3
−
(aq)
Balance all atoms other than H and O.
Cr
2
O
7
2−
(aq)+HNO
2
(aq)⟶2Cr
3+
(aq)+NO
3
−
(aq)
The oxidation number of Cr changes from +6 to +3. The change in the oxidation number is 3.
Total change in the oxidation number is 6.
The oxidation number of N changes from +3 to +5. The change in the oxidation number is 2.
To balance the increase in the oxidation number with decrease in oxidation number, multiply NO
2
−
and NO
3
−
with 3.
Cr
2
O
7
2−
(aq)+H
+
+3NO
2
−
(aq)⟶2Cr
3+
(aq)+3NO
3
−
(aq)
Balance the O atoms by adding 4 water molecules on RHS.
Cr
2
O
7
2−
(aq)+H
+
+3NO
2
−
(aq)⟶2Cr
3+
(aq)+3NO
3
−
(aq)+4H
2
O
Balance H atoms by adding 7H
+
ions on LHS.
Cr
2
O
7
2−
(aq)+8H
+
+3NO
2
−
(aq)⟶2Cr
3+
(aq)+3NO
3
−
(aq)+4H
2
O
This is the balanced chemical equation
Explanation:
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