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16FeO + 3NaH2PO4 ๐Ÿ”ฅโ†’ 8Fe2O3 + 2P + Na3PO4 + 3H2โ†‘

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Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOIron(II) oxide + 3NaH2PO4Sodium dihydrogenphosphate
๐Ÿ”ฅ
โŸถ
8Fe2O3Iron(III) oxide + 2PPhosphorus + Na3PO4Sodium phosphate + 3H2โ†‘Hydrogen

The reaction of iron(II) oxide and sodium dihydrogenphosphate yields iron(III) oxide, phosphorus, sodium phosphate, 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
16FeOIron(II) oxide + 3NaH2PO4Sodium dihydrogenphosphate
๐Ÿ”ฅ
โŸถ
8Fe2O3Iron(III) oxide + 2PPhosphorus + Na3PO4Sodium phosphate + 3H2โ†‘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) oxide16
Reducing
Oxidizable
NaH2PO4Sodium dihydrogenphosphate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Fe2O3Iron(III) oxide8
Oxidized
โ€“
PPhosphorus2
Reduced
โ€“
Na3PO4Sodium phosphate1
โ€“
โ€“
H2Hydrogen3
Reduced
โ€“

Thermodynamic changes

Changes in standard condition (1)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOCrystalline solid + 3NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
8Fe2O3Crystalline solid + 2PCrystalline solidwhite + Na3PO4Crystalline solid + 3H2โ†‘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
28.21โ€“โ€“โ€“
150.5โ€“โ€“โ€“
per 1 mol of
56.42โ€“โ€“โ€“
per 1 mol of
225.7โ€“โ€“โ€“
per 1 mol of
451.4โ€“โ€“โ€“
per 1 mol of
150.5โ€“โ€“โ€“

Changes in standard condition (2)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOCrystalline solid + 3NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
8Fe2O3Crystalline solid + 2PCrystalline solidred, triclinic + Na3PO4Crystalline solid + 3H2โ†‘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
416.2โ€“โ€“โ€“
per 1 mol of
26.01โ€“โ€“โ€“
138.7โ€“โ€“โ€“
per 1 mol of
52.02โ€“โ€“โ€“
per 1 mol of
208.1โ€“โ€“โ€“
per 1 mol of
416.2โ€“โ€“โ€“
per 1 mol of
138.7โ€“โ€“โ€“

Changes in standard condition (3)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOCrystalline solid + 3NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
8Fe2O3Crystalline solid + 2PCrystalline solidblack + Na3PO4Crystalline solid + 3H2โ†‘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
372.8โ€“โ€“โ€“
per 1 mol of
23.30โ€“โ€“โ€“
124.3โ€“โ€“โ€“
per 1 mol of
46.60โ€“โ€“โ€“
per 1 mol of
186.4โ€“โ€“โ€“
per 1 mol of
372.8โ€“โ€“โ€“
per 1 mol of
124.3โ€“โ€“โ€“

Changes in standard condition (4)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOCrystalline solid + 3NaH2PO4Crystalline solid
๐Ÿ”ฅ
โŸถ
8Fe2O3Crystalline solid + 2PAmorphous solidred + Na3PO4Crystalline solid + 3H2โ†‘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
436.4โ€“โ€“โ€“
per 1 mol of
27.27โ€“โ€“โ€“
145.5โ€“โ€“โ€“
per 1 mol of
54.55โ€“โ€“โ€“
per 1 mol of
218.2โ€“โ€“โ€“
per 1 mol of
436.4โ€“โ€“โ€“
per 1 mol of
145.5โ€“โ€“โ€“

Changes in aqueous solution (1)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOCrystalline solid + 3NaH2PO4Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
8Fe2O3Crystalline solid + 2PCrystalline solidwhite + Na3PO4Ionized aqueous solution + 3H2โ†‘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
369.7โ€“โ€“โ€“
per 1 mol of
23.11โ€“โ€“โ€“
123.2โ€“โ€“โ€“
per 1 mol of
46.21โ€“โ€“โ€“
per 1 mol of
184.8โ€“โ€“โ€“
per 1 mol of
369.7โ€“โ€“โ€“
per 1 mol of
123.2โ€“โ€“โ€“

Changes in aqueous solution (2)

Reaction of iron(II) oxide and sodium dihydrogenphosphate
16FeOCrystalline solid + 3NaH2PO4Ionized aqueous solution
๐Ÿ”ฅ
โŸถ
8Fe2O3Crystalline solid + 2PCrystalline solidwhite + Na3PO4Ionized aqueous solution + 3H2โ†‘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
357.1โ€“โ€“โ€“
per 1 mol of
22.32โ€“โ€“โ€“
119.0โ€“โ€“โ€“
per 1 mol of
44.64โ€“โ€“โ€“
per 1 mol of
178.6โ€“โ€“โ€“
per 1 mol of
357.1โ€“โ€“โ€“
per 1 mol of
119.0โ€“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]
Na3PO4 (cr)-1917.40[1]-1788.80[1]173.80[1]153.47[1]
Na3PO4 (ai)-1997.9[1]-1804.5[1]-43.3[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, (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)