4FeSO4 🔥→ 2Fe2O3 + 4S + 5O2↑
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- Decomposition of iron(II) sulfate
Decomposition of iron(II) sulfate yields iron(III) oxide, , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of iron(II) sulfate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of iron(II) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSO4 | Iron(II) sulfate | 4 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe2O3 | Iron(III) oxide | 2 | Oxidized | – |
| 4 | Reduced | – | ||
| 5 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of iron(II) sulfate◆
ΔrG 1798.8 kJ/mol K 0.73 × 10−315 pK 315.14
| 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 | 2065.2 | 1798.8 | 897.7 | 42.72 |
per 1 mol of | 516.30 | 449.70 | 224.4 | 10.68 |
per 1 mol of | 1032.6 | 899.40 | 448.9 | 21.36 |
| 516.30 | 449.70 | 224.4 | 10.68 | |
| 413.04 | 359.76 | 179.5 | 8.544 |
Changes in standard condition (2)
- Decomposition of iron(II) sulfate
| 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 | 2066.5 | – | – | – |
per 1 mol of | 516.63 | – | – | – |
per 1 mol of | 1033.3 | – | – | – |
| 516.63 | – | – | – | |
| 413.30 | – | – | – |
Changes in aqueous solution (1)
- Decomposition of iron(II) sulfate◆
ΔrG 1798.8 kJ/mol K 0.73 × 10−315 pK 315.14
| 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 | 2065.2 | 1798.8 | 897.7 | 42.72 |
per 1 mol of | 516.30 | 449.70 | 224.4 | 10.68 |
per 1 mol of | 1032.6 | 899.40 | 448.9 | 21.36 |
| 516.30 | 449.70 | 224.4 | 10.68 | |
| 413.04 | 359.76 | 179.5 | 8.544 |
Changes in aqueous solution (2)
- Decomposition of iron(II) sulfate◆
ΔrG 1880.8 kJ/mol K 0.31 × 10−329 pK 329.50
| 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 | 2006.7 | 1880.8 | 426.5 | – |
per 1 mol of | 501.68 | 470.20 | 106.6 | – |
per 1 mol of | 1003.4 | 940.40 | 213.3 | – |
| 501.68 | 470.20 | 106.6 | – | |
| 401.34 | 376.16 | 85.30 | – |
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 |
|---|---|---|---|---|
| FeSO4 (cr) | -928.4[1] | -820.8[1] | 107.5[1] | 100.58[1] |
| FeSO4 (ai) | -998.3[1] | -823.43[1] | -117.6[1] | – |
| FeSO4 (cr) 1 hydrate | -1243.69[1] | – | – | – |
| FeSO4 (cr) 4 hydrate | -2129.2[1] | – | – | – |
| FeSO4 (cr) 7 hydrate | -3014.57[1] | -2509.87[1] | 409.2[1] | 394.47[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) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[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°, -928.4 kJ · mol−1
- ^ ΔfG°, -820.8 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ Cp°, 100.58 J · K−1 · mol−1
- ^ ΔfH°, -998.3 kJ · mol−1
- ^ ΔfG°, -823.43 kJ · mol−1
- ^ S°, -117.6 J · K−1 · mol−1
- ^ ΔfH°, -1243.69 kJ · mol−1
- ^ ΔfH°, -2129.2 kJ · mol−1
- ^ ΔfH°, -3014.57 kJ · mol−1
- ^ ΔfG°, -2509.87 kJ · mol−1
- ^ S°, 409.2 J · K−1 · mol−1
- ^ Cp°, 394.47 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°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1