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In: Chemistry

Show the calculation of the oxidation number (charge) of ONLY the atoms which are changing in...

Show the calculation of the oxidation number (charge) of ONLY the atoms which are changing in the following redox equations and then show how they are used to balance the following redox equation. MnO + PbO2 + HNO3 → HMnO4 + Pb(NO3)2 + H2O

Expert Solution

The unbalanced chemical equation is

Mn atoms and Pb atoms are balanced on both sides of equation.

The oxidation number of Mn increases from (in MnO) to (in ). The increasse in the oxidation number of Mn is .

In MnO, the oxidation number of O is . Let x be the oxidation number of Mn.

In , the oxidation numbers of H and O are respectively. Let x be the oxidation number of Mn

The oxidation number of lead decreases from (in ) to (in ). The decrease in the oxidation number of Pb is

In , the oxidation number of O is . Let x be the oxidation number of Pb.

In , the oxidation numbers of N and O are resectively. Let x be the oxidation number of Pb

Multiply Mn species with 2 and Pb species with 5. This will balance increase in oxidation number of Mn with decrease in oxidation number of lead.

Balance N atoms by multiplying HNO3 with 10

There are 42 O atoms on left hand side of equation and 39 O atoms on right hand side of equation.

To balance O atoms, add 3 water molecules to the right hand side of equation.

H atoms are balanced. This is balanced chemical equation.

queen_honey_blossom answered 1 year ago

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