CH3COONH4 + 8Fe2O3 🔥→ 2FeCO3 + 2Fe(OH)2 + 4Fe3O4 + NH3↑
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The reaction of ammonium acetate and iron(III) oxide yields iron(II) carbonate, iron(II) hydroxide, iron(II,III) oxide, and ammonia (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium acetate and iron(III) oxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of ammonium acetate and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COONH4 | Ammonium acetate | 1 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 8 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCO3 | Iron(II) carbonate | 2 | Redoxed product | – |
| Fe(OH)2 | Iron(II) hydroxide | 2 | Reduced | – |
| Fe3O4 | Iron(II,III) oxide | 4 | Reduced | – |
| NH3 | Ammonia | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium acetate and iron(III) oxide
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 70.9 | – | – | – |
per 1 mol of | 70.9 | – | – | – |
per 1 mol of | 8.86 | – | – | – |
per 1 mol of | 35.5 | – | – | – |
per 1 mol of | 35.5 | – | – | – |
per 1 mol of | 17.7 | – | – | – |
per 1 mol of | 70.9 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium acetate and iron(III) oxide◆
ΔrG 1.8 kJ/mol K 0.48 × 100 pK 0.32
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 73.3 | 1.8 | 241 | – |
per 1 mol of | 73.3 | 1.8 | 241 | – |
per 1 mol of | 9.16 | 0.23 | 30.1 | – |
per 1 mol of | 36.6 | 0.90 | 121 | – |
per 1 mol of | 36.6 | 0.90 | 121 | – |
per 1 mol of | 18.3 | 0.45 | 60.3 | – |
per 1 mol of | 73.3 | 1.8 | 241 | – |
Changes in aqueous solution (2)
- Reaction of ammonium acetate and iron(III) oxide◆
ΔrG −8.2 kJ/mol K 2.73 × 101 pK −1.44
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | 39.1 | −8.2 | 160 | – |
per 1 mol of | 39.1 | −8.2 | 160 | – |
per 1 mol of | 4.89 | −1.0 | 20.0 | – |
per 1 mol of | 19.6 | −4.1 | 80.0 | – |
per 1 mol of | 19.6 | −4.1 | 80.0 | – |
per 1 mol of | 9.78 | −2.0 | 40.0 | – |
per 1 mol of | 39.1 | −8.2 | 160 | – |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| CH3COONH4 (cr) | -616.14[1] | – | – | – |
| CH3COONH4 (ai) | -618.52[1] | -448.61[1] | 200.0[1] | 73.6[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 formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[1] |
| Fe(OH)2 (cr) precipitated | -569.0[1] | -486.5[1] | 88[1] | – |
| Fe(OH)2 (g) | -372[1] | – | – | – |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| 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] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -616.14 kJ · mol−1
- ^ ΔfH°, -618.52 kJ · mol−1
- ^ ΔfG°, -448.61 kJ · mol−1
- ^ S°, 200.0 J · K−1 · mol−1
- ^ Cp°, 73.6 J · K−1 · mol−1
- ^ ΔfH°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 J · K−1 · mol−1
- ^ ΔfH°, -740.57 kJ · mol−1
- ^ ΔfG°, -666.67 kJ · mol−1
- ^ S°, 92.9 J · K−1 · mol−1
- ^ Cp°, 82.13 J · K−1 · mol−1
- ^ ΔfH°, -569.0 kJ · mol−1
- ^ ΔfG°, -486.5 kJ · mol−1
- ^ S°, 88. J · K−1 · mol−1
- ^ ΔfH°, -372. kJ · mol−1
- ^ ΔfH°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 J · K−1 · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1