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  3. 14NH4Cl + 10Fe2O3 ๐Ÿ”ฅโ†’ 4NOโ†‘ + 7FeCl2 + 13Fe(OH)2 + 10NH3โ†‘

14NH4Cl + 10Fe2O3 ๐Ÿ”ฅโ†’ 4NOโ†‘ + 7FeCl2 + 13Fe(OH)2 + 10NH3โ†‘

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Reaction of ammonium chloride and iron(III) oxide
14NH4ClAmmonium chloride + 10Fe2O3Iron(III) oxide
๐Ÿ”ฅ
โŸถ
4NOโ†‘Nitrogen monoxide + 7FeCl2Iron(II) chloride + 13Fe(OH)2Iron(II) hydroxide + 10NH3โ†‘Ammonia

The reaction of ammonium chloride and iron(III) oxide yields nitrogen monoxide, iron(II) chloride, iron(II) hydroxide, and ammonia (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 ammonium chloride and iron(III) oxide
14NH4ClAmmonium chloride + 10Fe2O3Iron(III) oxide
๐Ÿ”ฅ
โŸถ
4NOโ†‘Nitrogen monoxide + 7FeCl2Iron(II) chloride + 13Fe(OH)2Iron(II) hydroxide + 10NH3โ†‘Ammonia

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
โŸถ
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium chloride and iron(III) oxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4ClAmmonium chloride14
Reducing
Reducing
Fe2O3Iron(III) oxide10
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NONitrogen monoxide4
Oxidized
โ€“
FeCl2Iron(II) chloride7
Reduced
โ€“
Fe(OH)2Iron(II) hydroxide13
Reduced
โ€“
NH3Ammonia10
โ€“
โ€“

Thermodynamic changes

Changes in standard condition

Reaction of ammonium chloride and iron(III) oxide
โ—†
ฮ”rG2003.3 kJ/mol
K0.11 ร— 10โˆ’350
pK350.96
14NH4ClCrystalline solid + 10Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
4NOโ†‘Gas + 7FeCl2Crystalline solid + 13Fe(OH)2Crystalline solidprecipitated + 10NH3โ†‘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
2754.42003.32539โ€“
per 1 mol of
196.74143.09181.4โ€“
per 1 mol of
275.44200.33253.9โ€“
per 1 mol of
688.60500.82634.8โ€“
per 1 mol of
393.49286.19362.7โ€“
per 1 mol of
211.88154.10195.3โ€“
per 1 mol of
275.44200.33253.9โ€“

Changes in aqueous solution (1)

Reaction of ammonium chloride and iron(III) oxide
โ—†
ฮ”rG2272.8 kJ/mol
K0.66 ร— 10โˆ’398
pK398.18
14NH4ClIonized aqueous solution + 10Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
4NOโ†‘Gas + 7FeCl2Un-ionized aqueous solution + 13Fe(OH)2Crystalline solidprecipitated + 10NH3โ†‘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€“2272.8โ€“โ€“
per 1 mol of
โ€“162.34โ€“โ€“
per 1 mol of
โ€“227.28โ€“โ€“
per 1 mol of
โ€“568.20โ€“โ€“
per 1 mol of
โ€“324.69โ€“โ€“
per 1 mol of
โ€“174.83โ€“โ€“
per 1 mol of
โ€“227.28โ€“โ€“

Changes in aqueous solution (2)

Reaction of ammonium chloride and iron(III) oxide
โ—†
ฮ”rG2172.3 kJ/mol
K0.27 ร— 10โˆ’380
pK380.57
14NH4ClIonized aqueous solution + 10Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
4NOโ†‘Gas + 7FeCl2Un-ionized aqueous solution + 13Fe(OH)2Crystalline solidprecipitated + 10NH3โ†‘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€“2172.3โ€“โ€“
per 1 mol of
โ€“155.16โ€“โ€“
per 1 mol of
โ€“217.23โ€“โ€“
per 1 mol of
โ€“543.08โ€“โ€“
per 1 mol of
โ€“310.33โ€“โ€“
per 1 mol of
โ€“167.10โ€“โ€“
per 1 mol of
โ€“217.23โ€“โ€“

Changes in aqueous solution (3)

Reaction of ammonium chloride and iron(III) oxide
โ—†
ฮ”rG1837.1 kJ/mol
K0.14 ร— 10โˆ’321
pK321.85
14NH4ClIonized aqueous solution + 10Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
4NOโ†‘Gas + 7FeCl2Ionized aqueous solution + 13Fe(OH)2Crystalline solidprecipitated + 10NH3โ†‘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
1976.31837.1486โ€“
per 1 mol of
141.16131.2234.7โ€“
per 1 mol of
197.63183.7148.6โ€“
per 1 mol of
494.07459.27122โ€“
per 1 mol of
282.33262.4469.4โ€“
per 1 mol of
152.02141.3237.4โ€“
per 1 mol of
197.63183.7148.6โ€“

Changes in aqueous solution (4)

Reaction of ammonium chloride and iron(III) oxide
โ—†
ฮ”rG1736.6 kJ/mol
K0.58 ร— 10โˆ’304
pK304.24
14NH4ClIonized aqueous solution + 10Fe2O3Crystalline solid
๐Ÿ”ฅ
โŸถ
4NOโ†‘Gas + 7FeCl2Ionized aqueous solution + 13Fe(OH)2Crystalline solidprecipitated + 10NH3โ†‘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
1634.51736.6โˆ’325โ€“
per 1 mol of
116.75124.04โˆ’23.2โ€“
per 1 mol of
163.45173.66โˆ’32.5โ€“
per 1 mol of
408.63434.15โˆ’81.3โ€“
per 1 mol of
233.50248.09โˆ’46.4โ€“
per 1 mol of
125.73133.58โˆ’25.0โ€“
per 1 mol of
163.45173.66โˆ’32.5โ€“

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
NH4Cl (cr)-314.43[1]-202.87[1]94.6[1]84.1[1]
NH4Cl (ai)-299.66[1]-210.52[1]169.9[1]-56.5[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
* (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
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
FeCl2 (cr)-341.79[1]-302.30[1]117.95[1]76.65[1]
FeCl2 (g)-148.5[1]โ€“โ€“โ€“
FeCl2 (ai)-423.4[1]-341.34[1]-24.7[1]โ€“
FeCl2 (ao)โ€“-279.1[1]โ€“โ€“
FeCl2 (cr)
2 hydrate
-953.1[1]โ€“โ€“โ€“
FeCl2 (cr)
4 hydrate
-1549.3[1]โ€“โ€“โ€“
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]โ€“
Fe(OH)2 (g)-372[1]โ€“โ€“โ€“
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]โ€“
* (g):Gas, (cr):Crystalline solid, (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)