2HCl + 3Fe(NO3)3 + 9H+ 🔥→ Cl2 + 2NO2 + 3Fe3+ + 7HNO3 + 2H2O
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- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition
- 2HClHydrogen chloride + 3Fe(NO3)3Iron(III) nitrate + 9H+Hydrogen ion+ 2NO2Nitrogen dioxide + 3Fe3+Iron(III) ion + 7HNO3Nitric acid + 2H2OWater🔥⟶
The reaction of hydrogen chloride, iron(III) nitrate, and hydrogen ion yields , nitrogen dioxide, iron(III) ion, nitric acid, 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 hydrogen chloride and iron(III) nitrate under acidic condition
- 2HClHydrogen chloride + 3Fe(NO3)3Iron(III) nitrate + 9H+Hydrogen ion+ 2NO2Nitrogen dioxide + 3Fe3+Iron(III) ion + 7HNO3Nitric acid + 2H2OWater🔥⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species under acidic condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCl | Hydrogen chloride | 2 | Reducing | Hardly oxidizable |
| Fe(NO3)3 | Iron(III) nitrate | 3 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 9 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Oxidized | – | ||
| NO2 | Nitrogen dioxide | 2 | Reduced | – |
| Fe3+ | Iron(III) ion | 3 | – | – |
| HNO3 | Nitric acid | 7 | – | – |
| H2O | Water | 2 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition◆
ΔrG 112.9 kJ/mol K 0.17 × 10−19 pK 19.78
| 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 | 244.1 | 112.9 | 436.9 | – |
per 1 mol of | 122.0 | 56.45 | 218.4 | – |
per 1 mol of | 81.37 | 37.63 | 145.6 | – |
per 1 mol of Hydrogen ion | 27.12 | 12.54 | 48.54 | – |
| 244.1 | 112.9 | 436.9 | – | |
per 1 mol of | 122.0 | 56.45 | 218.4 | – |
per 1 mol of Iron(III) ion | 81.37 | 37.63 | 145.6 | – |
per 1 mol of | 34.87 | 16.13 | 62.41 | – |
per 1 mol of | 122.0 | 56.45 | 218.4 | – |
Changes in standard condition (2)
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition◆
ΔrG 119.8 kJ/mol K 0.10 × 10−20 pK 20.99
| 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 | 220.7 | 119.8 | 335 | – |
per 1 mol of | 110.3 | 59.90 | 168 | – |
per 1 mol of | 73.57 | 39.93 | 112 | – |
per 1 mol of Hydrogen ion | 24.52 | 13.31 | 37.2 | – |
| 220.7 | 119.8 | 335 | – | |
per 1 mol of | 110.3 | 59.90 | 168 | – |
per 1 mol of Iron(III) ion | 73.57 | 39.93 | 112 | – |
per 1 mol of | 31.53 | 17.11 | 47.9 | – |
per 1 mol of | 110.3 | 59.90 | 168 | – |
Changes in standard condition (3)
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition
| 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 | 256.7 | – | – | – |
per 1 mol of | 128.3 | – | – | – |
per 1 mol of | 85.57 | – | – | – |
per 1 mol of Hydrogen ion | 28.52 | – | – | – |
| 256.7 | – | – | – | |
per 1 mol of | 128.3 | – | – | – |
per 1 mol of Iron(III) ion | 85.57 | – | – | – |
per 1 mol of | 36.67 | – | – | – |
per 1 mol of | 128.3 | – | – | – |
Changes in standard condition (4)
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition
| 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 | 233.3 | – | – | – |
per 1 mol of | 116.7 | – | – | – |
per 1 mol of | 77.77 | – | – | – |
per 1 mol of Hydrogen ion | 25.92 | – | – | – |
| 233.3 | – | – | – | |
per 1 mol of | 116.7 | – | – | – |
per 1 mol of Iron(III) ion | 77.77 | – | – | – |
per 1 mol of | 33.33 | – | – | – |
per 1 mol of | 116.7 | – | – | – |
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 |
|---|---|---|---|---|
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[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] | – | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (g):Gas, (ai):Ionized aqueous solution, (aq):Aqueous solution, (cr):Crystalline solid, (ao):Un-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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[1] |
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[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] |
| 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] |
* (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid
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°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 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°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, 33.18 kJ · mol−1
- ^ ΔfG°, 51.31 kJ · mol−1
- ^ S°, 240.06 J · K−1 · mol−1
- ^ Cp°, 37.20 J · K−1 · mol−1
- ^ ΔfH°, 5712.8 kJ · mol−1
- ^ ΔfH°, -48.5 kJ · mol−1
- ^ ΔfG°, -4.7 kJ · mol−1
- ^ S°, -315.9 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°, -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