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2Fe(NO3)3 + 12H2O ๐Ÿ’งโšกโ†’ 2Fe(OH)3 + 6NH2OH + 9O2โ†‘

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Electrolysis of aqueous iron(III) nitrate with water as non-redox agent
2Fe(NO3)3Iron(III) nitrate + 12H2OWater
๐Ÿ’งโšก
โŸถ
2Fe(OH)3Iron(III) hydroxide + 6NH2OHHydroxylamine + 9O2โ†‘Oxygen

Electrolysis of aqueous iron(III) nitrate yields iron(III) hydroxide, hydroxylamine, and oxygen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Electrolysis of aqueous iron(III) nitrate with water as non-redox agent
2Fe(NO3)3Iron(III) nitrate + 12H2OWater
๐Ÿ’งโšก
โŸถ
2Fe(OH)3Iron(III) hydroxide + 6NH2OHHydroxylamine + 9O2โ†‘Oxygen

General equation

Electrolysis of aqueous solution with water as non redox agent
Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent
๐Ÿ’งโšก
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous iron(III) nitrate with water as non-redox agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Fe(NO3)3Iron(III) nitrate2
Self redox agent
Very soluble in water
H2OWater12
โ€“
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe(OH)3Iron(III) hydroxide2
โ€“
โ€“
NH2OHHydroxylamine6
Reduced
โ€“
O2Oxygen9
Oxidized
โ€“

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous iron(III) nitrate with water as non-redox agent
2Fe(NO3)3Ionized aqueous solution + 12H2OLiquid
๐Ÿ’งโšก
โŸถ
2Fe(OH)3Un-ionized aqueous solution + 6NH2OHAqueous solution + 9O2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
โ€“โ€“โ€“โ€“
per 1 mol of
Hydroxylamine
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“

Changes in aqueous solution (2)

Electrolysis of aqueous iron(III) nitrate with water as non-redox agent
2Fe(NO3)3Ionized aqueous solution + 12H2OLiquid
๐Ÿ’งโšก
โŸถ
2Fe(OH)3Un-ionized aqueous solution + 6NH2OHAqueous solution + 9O2โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
โ€“โ€“โ€“โ€“
per 1 mol of
Hydroxylamine
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“

Changes in aqueous solution (3)

Electrolysis of aqueous iron(III) nitrate with water as non-redox agent
2Fe(NO3)3Aqueous solution + 12H2OLiquid
๐Ÿ’งโšก
โŸถ
2Fe(OH)3Un-ionized aqueous solution + 6NH2OHAqueous solution + 9O2โ†‘Gas
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
โ€“โ€“โ€“โ€“
per 1 mol of
Hydroxylamine
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“

Changes in aqueous solution (4)

Electrolysis of aqueous iron(III) nitrate with water as non-redox agent
2Fe(NO3)3Aqueous solution + 12H2OLiquid
๐Ÿ’งโšก
โŸถ
2Fe(OH)3Un-ionized aqueous solution + 6NH2OHAqueous solution + 9O2โ†‘Un-ionized aqueous solution
Standard enthalpy
of reaction
ฮ”rHยฐ
kJ ยท molโˆ’1		Standard
Gibbs energy
of reaction
ฮ”rGยฐ
kJ ยท molโˆ’1		Standard entropy
of reaction
ฮ”rSยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard heat
capacity of reaction
at constant pressure
ฮ”rCpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
per 1 mol of
Equation
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“
โ€“โ€“โ€“โ€“
per 1 mol of
Hydroxylamine
โ€“โ€“โ€“โ€“
per 1 mol of
โ€“โ€“โ€“โ€“

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Fe(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]โ€“
Fe(NO3)3 (aq)-674.9[1]โ€“โ€“โ€“
Fe(NO3)3 (cr)
9 hydrate
-3285.3[1]โ€“โ€“โ€“
H2O (cr)โ€“โ€“โ€“โ€“
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (l):Liquid, (g):Gas

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ฮ”fHยฐ
kJ ยท molโˆ’1		Standard Gibbs
energy of
formation
ฮ”fGยฐ
kJ ยท molโˆ’1		Standard
molar entropy
Sยฐ
J ยท Kโˆ’1 ยท molโˆ’1		Standard molar
heat capacity at
constant pressure
Cpยฐ
J ยท Kโˆ’1 ยท molโˆ’1
Fe(OH)3 (cr)
precipitated
-823.0[1]-696.5[1]106.7[1]โ€“
Fe(OH)3 (ao)โ€“-659.3[1]โ€“โ€“
NH2OH (cr)-114.2[1]โ€“โ€“โ€“
NH2OH (aq)-98.3[1]โ€“โ€“โ€“
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]โ€“
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (aq):Aqueous solution, (g):Gas

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)