# H2O2+2Fe(OH)2 -> 2Fe(OH)3   2PbO+C->2Pb+CO2  NiO+H2->Ni+H20 See description below       Use oxidation numbers to identify what element is being reduced and oxidized in following...

H2O2+2Fe(OH)2 -> 2Fe(OH)3

2PbO+C->2Pb+CO2

NiO+H2->Ni+H20

See description below

Use oxidation numbers to identify what element is being reduced and oxidized in following reactions. Identify reducing agents. Show all work. this all part of one question.

jeew-m | Certified Educator

`H_2O_2+2Fe(OH)_2 -> 2Fe(OH)_3 `

Oxidation number of O in `H_2O_2` = -1

Oxidation number of O in `Fe(OH)_3` = -2

Oxidation number of Fe in `Fe(OH)_2` = +2

Oxidation number of Fe in `Fe(OH)_3` = +3

Oxidation number of O in `H_2O_2` has reduced to -1 to -2. So `H_2O_2` is the reducing agent.

Oxidation number of Fe in `Fe(OH)_2` has increased from +2 to +3.

`PbO+C->2Pb+CO_2`

Oxidation number of Pb in PbO = +2

Oxidation number of Pb in Pb = 0

Oxidation number of C in C = 0

Oxidation number of C in `CO_2` = +4

Oxidation number of Pb in PbO has reduced to +2 to 0. So PbO is the reducing agent.

Oxidation number of C has increased from 0 to +4.

`NiO+H_2->Ni+H_2O`

Oxidation number of Ni in NiO = +2

Oxidation number of Ni in Ni = 0

Oxidation number of H in `H_2` = 0

Oxidation number of H in `H_2O` = +1

Oxidation number of Ni in NiO has reduced to +2 to 0. So NiO is the reducing agent.

Oxidation number of H has increased from 0 to +1.