3Fe + 4H2SO4 → 3FeSO4 + S + 4H2O
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- Reaction of and sulfuric acid
The reaction of and sulfuric acid yields iron(II) sulfate, , and water (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 and sulfuric acid
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 and sulfuric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Reducing | Reducing | ||
| H2SO4 | Sulfuric acid | 4 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeSO4 | Iron(II) sulfate | 3 | Oxidized | – |
| 1 | Reduced | – | ||
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and sulfuric acid◆
ΔrG −650.9 kJ/mol K 1.08 × 10114 pK −114.03
| 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 | −672.6 | −650.9 | −75.5 | −5.40 |
| −224.2 | −217.0 | −25.2 | −1.80 | |
per 1 mol of | −168.2 | −162.7 | −18.9 | −1.35 |
per 1 mol of | −224.2 | −217.0 | −25.2 | −1.80 |
| −672.6 | −650.9 | −75.5 | −5.40 | |
per 1 mol of | −168.2 | −162.7 | −18.9 | −1.35 |
Changes in standard condition (2)
- Reaction of and sulfuric acid
| 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 | −672.2 | – | – | – |
| −224.1 | – | – | – | |
per 1 mol of | −168.1 | – | – | – |
per 1 mol of | −224.1 | – | – | – |
| −672.2 | – | – | – | |
per 1 mol of | −168.1 | – | – | – |
Changes in aqueous solution
- Reaction of and sulfuric acid◆
ΔrG −432.8 kJ/mol K 6.66 × 1075 pK −75.82
| 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 | −291.4 | −432.8 | 471.7 | 1722 |
| −97.13 | −144.3 | 157.2 | 574.0 | |
per 1 mol of | −72.85 | −108.2 | 117.9 | 430.5 |
per 1 mol of | −97.13 | −144.3 | 157.2 | 574.0 |
| −291.4 | −432.8 | 471.7 | 1722 | |
per 1 mol of | −72.85 | −108.2 | 117.9 | 430.5 |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 27.28[1] | 25.10[1] |
| (g) | 416.3[1] | 370.7[1] | 180.490[1] | 25.677[1] |
| H2SO4 (cr) | – | – | – | – |
| H2SO4 (l) | -813.989[1] | -690.003[1] | 156.904[1] | 138.91[1] |
| H2SO4 (ai) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
| H2SO4 (l) 1 hydrate | -1127.621[1] | -950.383[1] | 211.54[1] | 214.85[1] |
| H2SO4 (l) 2 hydrate | -1427.100[1] | -1199.650[1] | 276.40[1] | 260.83[1] |
| H2SO4 (l) 3 hydrate | -1720.402[1] | -1443.980[1] | 345.39[1] | 318.95[1] |
| H2SO4 (l) 4 hydrate | -2011.199[1] | -1685.863[1] | 414.59[1] | 382.21[1] |
| H2SO4 (l) 6.5 hydrate | -2733.256[1] | -2285.734[1] | 587.89[1] | 570.28[1] |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (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 |
|---|---|---|---|---|
| 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) 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] |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (l):Liquid
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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 27.28 J · K−1 · mol−1
- ^ Cp°, 25.10 J · K−1 · mol−1
- ^ ΔfH°, 416.3 kJ · mol−1
- ^ ΔfG°, 370.7 kJ · mol−1
- ^ S°, 180.490 J · K−1 · mol−1
- ^ Cp°, 25.677 J · K−1 · mol−1
- ^ ΔfH°, -813.989 kJ · mol−1
- ^ ΔfG°, -690.003 kJ · mol−1
- ^ S°, 156.904 J · K−1 · mol−1
- ^ Cp°, 138.91 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1
- ^ ΔfH°, -1127.621 kJ · mol−1
- ^ ΔfG°, -950.383 kJ · mol−1
- ^ S°, 211.54 J · K−1 · mol−1
- ^ Cp°, 214.85 J · K−1 · mol−1
- ^ ΔfH°, -1427.100 kJ · mol−1
- ^ ΔfG°, -1199.650 kJ · mol−1
- ^ S°, 276.40 J · K−1 · mol−1
- ^ Cp°, 260.83 J · K−1 · mol−1
- ^ ΔfH°, -1720.402 kJ · mol−1
- ^ ΔfG°, -1443.980 kJ · mol−1
- ^ S°, 345.39 J · K−1 · mol−1
- ^ Cp°, 318.95 J · K−1 · mol−1
- ^ ΔfH°, -2011.199 kJ · mol−1
- ^ ΔfG°, -1685.863 kJ · mol−1
- ^ S°, 414.59 J · K−1 · mol−1
- ^ Cp°, 382.21 J · K−1 · mol−1
- ^ ΔfH°, -2733.256 kJ · mol−1
- ^ ΔfG°, -2285.734 kJ · mol−1
- ^ S°, 587.89 J · K−1 · mol−1
- ^ Cp°, 570.28 J · K−1 · mol−1
- ^ 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°, 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°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1