10FeO + Ca3(PO4)2 🔥→ 5Fe2O3 + 2P + 3CaO
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- Reaction of iron(II) oxide and calcium phosphate
The reaction of iron(II) oxide and calcium phosphate yields iron(III) oxide, , and calcium oxide (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 iron(II) oxide and calcium phosphate
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of iron(II) oxide and calcium phosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeO | Iron(II) oxide | 10 | Reducing | Oxidizable |
| Ca3(PO4)2 | Calcium phosphate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2O3 | Iron(III) oxide | 5 | Oxidized | – |
| 2 | Reduced | – | ||
| CaO | Calcium oxide | 3 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 814.5 | – | – | – |
per 1 mol of | 81.45 | – | – | – |
per 1 mol of | 814.5 | – | – | – |
per 1 mol of | 162.9 | – | – | – |
| 407.3 | – | – | – | |
per 1 mol of | 271.5 | – | – | – |
Changes in standard condition (2)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 779.3 | – | – | – |
per 1 mol of | 77.93 | – | – | – |
per 1 mol of | 779.3 | – | – | – |
per 1 mol of | 155.9 | – | – | – |
| 389.6 | – | – | – | |
per 1 mol of | 259.8 | – | – | – |
Changes in standard condition (3)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 735.9 | – | – | – |
per 1 mol of | 73.59 | – | – | – |
per 1 mol of | 735.9 | – | – | – |
per 1 mol of | 147.2 | – | – | – |
| 367.9 | – | – | – | |
per 1 mol of | 245.3 | – | – | – |
Changes in standard condition (4)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 799.5 | – | – | – |
per 1 mol of | 79.95 | – | – | – |
per 1 mol of | 799.5 | – | – | – |
per 1 mol of | 159.9 | – | – | – |
| 399.8 | – | – | – | |
per 1 mol of | 266.5 | – | – | – |
Changes in standard condition (5)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 803.6 | – | – | – |
per 1 mol of | 80.36 | – | – | – |
per 1 mol of | 803.6 | – | – | – |
per 1 mol of | 160.7 | – | – | – |
| 401.8 | – | – | – | |
per 1 mol of | 267.9 | – | – | – |
Changes in standard condition (6)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 768.4 | – | – | – |
per 1 mol of | 76.84 | – | – | – |
per 1 mol of | 768.4 | – | – | – |
per 1 mol of | 153.7 | – | – | – |
| 384.2 | – | – | – | |
per 1 mol of | 256.1 | – | – | – |
Changes in standard condition (7)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 725.0 | – | – | – |
per 1 mol of | 72.50 | – | – | – |
per 1 mol of | 725.0 | – | – | – |
per 1 mol of | 145.0 | – | – | – |
| 362.5 | – | – | – | |
per 1 mol of | 241.7 | – | – | – |
Changes in standard condition (8)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 788.6 | – | – | – |
per 1 mol of | 78.86 | – | – | – |
per 1 mol of | 788.6 | – | – | – |
per 1 mol of | 157.7 | – | – | – |
| 394.3 | – | – | – | |
per 1 mol of | 262.9 | – | – | – |
Changes in aqueous solution (1)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 814.5 | – | – | – |
per 1 mol of | 81.45 | – | – | – |
per 1 mol of | 814.5 | – | – | – |
per 1 mol of | 162.9 | – | – | – |
| 407.3 | – | – | – | |
per 1 mol of | 271.5 | – | – | – |
Changes in aqueous solution (2)
- Reaction of iron(II) oxide and calcium phosphate
| 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 | 803.6 | – | – | – |
per 1 mol of | 80.36 | – | – | – |
per 1 mol of | 803.6 | – | – | – |
per 1 mol of | 160.7 | – | – | – |
| 401.8 | – | – | – | |
per 1 mol of | 267.9 | – | – | – |
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 |
|---|---|---|---|---|
| FeO (cr) | -272.0[1] | – | – | – |
| Ca3(PO4)2 (cr) β, low temp. form | -4120.8[1] | -3884.7[1] | 236.0[1] | 227.82[1] |
| Ca3(PO4)2 (cr) α, high temp. form | -4109.9[1] | -3875.5[1] | 240.91[1] | 231.58[1] |
| Ca3(PO4)2 (ai) | -4183.2[1] | -3698.1[1] | -599.9[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 |
|---|---|---|---|---|
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
| (cr) white | 0[1] | 0[1] | 41.09[1] | 23.84[1] |
| (cr) red, triclinic | -17.6[1] | -12.1[1] | 22.80[1] | 21.21[1] |
| (cr) black | -39.3[1] | – | – | – |
| (am) red | -7.5[1] | – | – | – |
| (g) | 314.64[1] | 278.25[1] | 163.193[1] | 20.786[1] |
| CaO (cr) | -635.09[1] | -604.03[1] | 39.75[1] | 42.80[1] |
| CaO (g) | – | – | – | – |
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas
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°, -272.0 kJ · mol−1
- ^ ΔfH°, -4120.8 kJ · mol−1
- ^ ΔfG°, -3884.7 kJ · mol−1
- ^ S°, 236.0 J · K−1 · mol−1
- ^ Cp°, 227.82 J · K−1 · mol−1
- ^ ΔfH°, -4109.9 kJ · mol−1
- ^ ΔfG°, -3875.5 kJ · mol−1
- ^ S°, 240.91 J · K−1 · mol−1
- ^ Cp°, 231.58 J · K−1 · mol−1
- ^ ΔfH°, -4183.2 kJ · mol−1
- ^ ΔfG°, -3698.1 kJ · mol−1
- ^ S°, -599.9 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.09 J · K−1 · mol−1
- ^ Cp°, 23.84 J · K−1 · mol−1
- ^ ΔfH°, -17.6 kJ · mol−1
- ^ ΔfG°, -12.1 kJ · mol−1
- ^ S°, 22.80 J · K−1 · mol−1
- ^ Cp°, 21.21 J · K−1 · mol−1
- ^ ΔfH°, -39.3 kJ · mol−1
- ^ ΔfH°, -7.5 kJ · mol−1
- ^ ΔfH°, 314.64 kJ · mol−1
- ^ ΔfG°, 278.25 kJ · mol−1
- ^ S°, 163.193 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -635.09 kJ · mol−1
- ^ ΔfG°, -604.03 kJ · mol−1
- ^ S°, 39.75 J · K−1 · mol−1
- ^ Cp°, 42.80 J · K−1 · mol−1