2FeS + 6HNO3 🔥→ 2Fe(NO3)3 + 2H2S↑ + H2↑
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- Reaction of iron(II) sulfide and nitric acid
The reaction of iron(II) sulfide and nitric acid yields iron(III) nitrate, hydrogen sulfide, and (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) sulfide and nitric acid
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of iron(II) sulfide and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeS | Iron(II) sulfide | 2 | Reducing | Reducing |
| HNO3 | Nitric acid | 6 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidized | – |
| H2S | Hydrogen sulfide | 2 | – | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of iron(II) sulfide and nitric acid◆
ΔrG 124.6 kJ/mol K 0.15 × 10−21 pK 21.83
| 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 | 61.5 | 124.6 | −209.9 | – |
per 1 mol of | 30.8 | 62.30 | −105.0 | – |
per 1 mol of | 10.3 | 20.77 | −34.98 | – |
per 1 mol of | 30.8 | 62.30 | −105.0 | – |
per 1 mol of | 30.8 | 62.30 | −105.0 | – |
| 61.5 | 124.6 | −209.9 | – |
Changes in aqueous solution (2)
- Reaction of iron(II) sulfide and nitric acid◆
ΔrG 142.2 kJ/mol K 0.12 × 10−24 pK 24.91
| 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 | 57.3 | 142.2 | 236 | – |
per 1 mol of | 28.6 | 71.10 | 118 | – |
per 1 mol of | 9.55 | 23.70 | 39.3 | – |
per 1 mol of | 28.6 | 71.10 | 118 | – |
per 1 mol of | 28.6 | 71.10 | 118 | – |
| 57.3 | 142.2 | 236 | – |
Changes in aqueous solution (3)
- Reaction of iron(II) sulfide and nitric acid◆
ΔrG 136.0 kJ/mol K 0.15 × 10−23 pK 23.83
| 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 | 23.4 | 136.0 | −379 | – |
per 1 mol of | 11.7 | 68.00 | −190 | – |
per 1 mol of | 3.90 | 22.67 | −63.2 | – |
per 1 mol of | 11.7 | 68.00 | −190 | – |
per 1 mol of | 11.7 | 68.00 | −190 | – |
| 23.4 | 136.0 | −379 | – |
Changes in aqueous solution (4)
- Reaction of iron(II) sulfide and nitric acid◆
ΔrG 153.6 kJ/mol K 0.12 × 10−26 pK 26.91
| 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 | 19.2 | 153.6 | 67 | – |
per 1 mol of | 9.60 | 76.80 | 34 | – |
per 1 mol of | 3.20 | 25.60 | 11 | – |
per 1 mol of | 9.60 | 76.80 | 34 | – |
per 1 mol of | 9.60 | 76.80 | 34 | – |
| 19.2 | 153.6 | 67 | – |
Changes in aqueous solution (5)
- Reaction of iron(II) sulfide and nitric 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 | 53.1 | – | – | – |
per 1 mol of | 26.6 | – | – | – |
per 1 mol of | 8.85 | – | – | – |
per 1 mol of | 26.6 | – | – | – |
per 1 mol of | 26.6 | – | – | – |
| 53.1 | – | – | – |
Changes in aqueous solution (6)
- Reaction of iron(II) sulfide and nitric 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 | 48.9 | – | – | – |
per 1 mol of | 24.4 | – | – | – |
per 1 mol of | 8.15 | – | – | – |
per 1 mol of | 24.4 | – | – | – |
per 1 mol of | 24.4 | – | – | – |
| 48.9 | – | – | – |
Changes in aqueous solution (7)
- Reaction of iron(II) sulfide and nitric 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 | 15.0 | – | – | – |
per 1 mol of | 7.50 | – | – | – |
per 1 mol of | 2.50 | – | – | – |
per 1 mol of | 7.50 | – | – | – |
per 1 mol of | 7.50 | – | – | – |
| 15.0 | – | – | – |
Changes in aqueous solution (8)
- Reaction of iron(II) sulfide and nitric 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 | 10.8 | – | – | – |
per 1 mol of | 5.40 | – | – | – |
per 1 mol of | 1.80 | – | – | – |
per 1 mol of | 5.40 | – | – | – |
per 1 mol of | 5.40 | – | – | – |
| 10.8 | – | – | – |
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 |
|---|---|---|---|---|
| FeS (cr) iron-rich pyrrhotite, α | -100.0[1] | -100.4[1] | 60.29[1] | 50.54[1] |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (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 |
|---|---|---|---|---|
| Fe(NO3)3 (ai) | -670.7[1] | -338.3[1] | 123.4[1] | – |
| Fe(NO3)3 (aq) | -674.9[1] | – | – | – |
| Fe(NO3)3 (cr) 9 hydrate | -3285.3[1] | – | – | – |
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (ai):Ionized aqueous solution, (aq):Aqueous solution, (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°, -100.0 kJ · mol−1
- ^ ΔfG°, -100.4 kJ · mol−1
- ^ S°, 60.29 J · K−1 · mol−1
- ^ Cp°, 50.54 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -670.7 kJ · mol−1
- ^ ΔfG°, -338.3 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -674.9 kJ · mol−1
- ^ ΔfH°, -3285.3 kJ · mol−1
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1