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12FeO + 2NaH2PO4 ๐Ÿ”ฅโ†’ 6Fe2O3 + 2P + 2NaOH + H2โ†‘

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Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOIron(II) oxide + 2NaH2PO4Sodium dihydrogenphosphate
๐Ÿ”ฅ
โŸถ
6Fe2O3Iron(III) oxide + 2PPhosphorus + 2NaOHSodium hydroxide + H2โ†‘Hydrogen

The reaction of iron(II) oxide and sodium dihydrogenphosphate yields iron(III) oxide, phosphorus, sodium hydroxide, and hydrogen (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

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOIron(II) oxide + 2NaH2PO4Sodium dihydrogenphosphate
๐Ÿ”ฅ
โŸถ
6Fe2O3Iron(III) oxide + 2PPhosphorus + 2NaOHSodium hydroxide + H2โ†‘Hydrogen

General equation

Reaction of oxidizable species and reducible species
Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
๐Ÿ”ฅ
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of iron(II) oxide and sodium dihydrogenphosphate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeOIron(II) oxide12
Reducing
Oxidizable
NaH2PO4Sodium dihydrogenphosphate2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe2O3Iron(III) oxide6
Oxidized
โ€“
PPhosphorus2
Reduced
โ€“
NaOHSodium hydroxide2
โ€“
โ€“
H2Hydrogen1
Reduced
โ€“

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOCrystalline solid + 2NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
6Fe2O3Crystalline solid + 2PCrystalline solidwhite + 2NaOHCrystalline solid + H2โ†‘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
541.2โ€“โ€“โ€“
per 1 mol of
45.10โ€“โ€“โ€“
270.6โ€“โ€“โ€“
per 1 mol of
90.20โ€“โ€“โ€“
per 1 mol of
270.6โ€“โ€“โ€“
per 1 mol of
270.6โ€“โ€“โ€“
per 1 mol of
541.2โ€“โ€“โ€“

Changes in standard condition (2)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOCrystalline solid + 2NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
6Fe2O3Crystalline solid + 2PCrystalline solidred, triclinic + 2NaOHCrystalline solid + H2โ†‘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
506.0โ€“โ€“โ€“
per 1 mol of
42.17โ€“โ€“โ€“
253.0โ€“โ€“โ€“
per 1 mol of
84.33โ€“โ€“โ€“
per 1 mol of
253.0โ€“โ€“โ€“
per 1 mol of
253.0โ€“โ€“โ€“
per 1 mol of
506.0โ€“โ€“โ€“

Changes in standard condition (3)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOCrystalline solid + 2NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
6Fe2O3Crystalline solid + 2PCrystalline solidblack + 2NaOHCrystalline solid + H2โ†‘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
462.6โ€“โ€“โ€“
per 1 mol of
38.55โ€“โ€“โ€“
231.3โ€“โ€“โ€“
per 1 mol of
77.10โ€“โ€“โ€“
per 1 mol of
231.3โ€“โ€“โ€“
per 1 mol of
231.3โ€“โ€“โ€“
per 1 mol of
462.6โ€“โ€“โ€“

Changes in standard condition (4)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOCrystalline solid + 2NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
6Fe2O3Crystalline solid + 2PAmorphous solidred + 2NaOHCrystalline solid + H2โ†‘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
526.2โ€“โ€“โ€“
per 1 mol of
43.85โ€“โ€“โ€“
263.1โ€“โ€“โ€“
per 1 mol of
87.70โ€“โ€“โ€“
per 1 mol of
263.1โ€“โ€“โ€“
per 1 mol of
263.1โ€“โ€“โ€“
per 1 mol of
526.2โ€“โ€“โ€“

Changes in aqueous solution (1)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOCrystalline solid + 2NaH2PO4Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
6Fe2O3Crystalline solid + 2PCrystalline solidwhite + 2NaOHIonized aqueous solution + H2โ†‘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
451.4โ€“โ€“โ€“
per 1 mol of
37.62โ€“โ€“โ€“
225.7โ€“โ€“โ€“
per 1 mol of
75.23โ€“โ€“โ€“
per 1 mol of
225.7โ€“โ€“โ€“
per 1 mol of
225.7โ€“โ€“โ€“
per 1 mol of
451.4โ€“โ€“โ€“

Changes in aqueous solution (2)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
12FeOCrystalline solid + 2NaH2PO4Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
6Fe2O3Crystalline solid + 2PCrystalline solidwhite + 2NaOHIonized aqueous solution + H2โ†‘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
447.2โ€“โ€“โ€“
per 1 mol of
37.27โ€“โ€“โ€“
223.6โ€“โ€“โ€“
per 1 mol of
74.53โ€“โ€“โ€“
per 1 mol of
223.6โ€“โ€“โ€“
per 1 mol of
223.6โ€“โ€“โ€“
per 1 mol of
447.2โ€“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
FeO (cr)-272.0[1]โ€“โ€“โ€“
NaH2PO4 (cr)-1536.8[1]-1386.1[1]127.49[1]116.86[1]
NaH2PO4 (ai)-1536.41[1]-1392.17[1]149.4[1]โ€“
NaH2PO4 (cr)
1 hydrate
-1833.0[1]โ€“โ€“โ€“
NaH2PO4 (cr)
2 hydrate
-2128.4[1]โ€“โ€“โ€“
* (cr):Crystalline solid, (ai):Ionized aqueous solution

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
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
P (cr)
white
0[1]0[1]41.09[1]23.84[1]
P (cr)
red, triclinic
-17.6[1]-12.1[1]22.80[1]21.21[1]
P (cr)
black
-39.3[1]โ€“โ€“โ€“
P (am)
red
-7.5[1]โ€“โ€“โ€“
P (g)314.64[1]278.25[1]163.193[1]20.786[1]
NaOH (cr)-425.609[1]-379.494[1]64.455[1]59.54[1]
NaOH (g)-207.1[1]-210.0[1]228.43[1]48.37[1]
NaOH (ai)-470.114[1]-419.150[1]48.1[1]-102.1[1]
NaOH (cr)
1 hydrate
-734.543[1]-629.338[1]99.50[1]90.17[1]
NaOH (l)
2 hydrate
-1019.076[1]-873.091[1]195.979[1]239.41[1]
NaOH (l)
3.5 hydrate
-1459.798[1]-1236.356[1]286.089[1]354.43[1]
NaOH (l)
4 hydrate
-1605.15[1]-1356.64[1]318.70[1]โ€“
NaOH (l)
5 hydrate
-1894.31[1]-1596.34[1]386.06[1]โ€“
NaOH (l)
7 hydrate
-2469.02[1]-2073.80[1]526.31[1]โ€“
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]โ€“
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (ao):Un-ionized aqueous solution

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)