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Question

Balance the following equation.

HNO3+HBrNO+Br2+H2O

A
2HNO3+6HBr2NO+3Br2+4H2O
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B
2HNO3+3HBr2NO+3Br2+4H2O
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C
2HNO3+4HBr2NO+5Br2+4H2O
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D
None of these
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Solution

The correct option is A 2HNO3+6HBr2NO+3Br2+4H2O
The unbalanced redox equation is as follows:
HNO3+HBrNO+Br2+H2O
Balance all atoms other than H and O.
HNO3+2HBrNO+Br2+H2O
The oxidation number of bromine changes from -1 to 0. The change in the oxidation number of one bromine atom is 1. Total change in the oxidation number for 2 bromine atoms is 2.
The oxidation number of nitrogen changes from +5 to +2. The change in the oxidation number of nitrogen is 3.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying
HBr and Br2 with 3 and by multiplying HNO3 and NO with 2.
2HNO3+6HBr2NO+3Br2+H2O
O atoms are balanced by adding 3 water molecules on RHS.
2HNO3+6HBr2NO+3Br2+4H2O
Hydrogen atoms are balanced.
Hence, this is the balanced chemical equation.

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