8HCl + 2Fe(NO3)3 + 4H+ 🔥→ 3Cl2O + 6HNO2 + 2FeCl2+ + 3H2O
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- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition
- 8HClHydrogen chloride + 2Fe(NO3)3Iron(III) nitrate + 4H+Hydrogen ion3Cl2ODichlorine monoxide + 6HNO2Nitrous acid + 2FeCl2+Iron(III) chloride ion + 3H2OWater🔥⟶
The reaction of hydrogen chloride, iron(III) nitrate, and hydrogen ion yields dichlorine monoxide, nitrous acid, iron(III) chloride ion, 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
- 8HClHydrogen chloride + 2Fe(NO3)3Iron(III) nitrate + 4H+Hydrogen ion3Cl2ODichlorine monoxide + 6HNO2Nitrous acid + 2FeCl2+Iron(III) chloride ion + 3H2OWater🔥⟶
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 | 8 | Reducing | Hardly oxidizable |
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 4 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cl2O | Dichlorine monoxide | 3 | Oxidized | – |
| HNO2 | Nitrous acid | 6 | Reduced | – |
| FeCl2+ | Iron(III) chloride ion | 2 | – | – |
| H2O | Water | 3 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition◆
ΔrG 717.3 kJ/mol K 0.22 × 10−125 pK 125.67
| 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 | 986.3 | 717.3 | 897 | – |
per 1 mol of | 123.3 | 89.66 | 112 | – |
per 1 mol of | 493.1 | 358.6 | 449 | – |
per 1 mol of Hydrogen ion | 246.6 | 179.3 | 224 | – |
per 1 mol of | 328.8 | 239.1 | 299 | – |
per 1 mol of | 164.4 | 119.5 | 150 | – |
per 1 mol of Iron(III) chloride ion | 493.1 | 358.6 | 449 | – |
per 1 mol of | 328.8 | 239.1 | 299 | – |
Changes in standard condition (2)
- 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 | 994.7 | – | – | – |
per 1 mol of | 124.3 | – | – | – |
per 1 mol of | 497.4 | – | – | – |
per 1 mol of Hydrogen ion | 248.7 | – | – | – |
per 1 mol of | 331.6 | – | – | – |
per 1 mol of | 165.8 | – | – | – |
per 1 mol of Iron(III) chloride ion | 497.4 | – | – | – |
per 1 mol of | 331.6 | – | – | – |
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 |
|---|---|---|---|---|
| Cl2O (g) | 80.3[1] | 97.9[1] | 266.21[1] | 45.40[1] |
| HNO2 (g) cis | -77.99[1] | -42.94[1] | 248.76[1] | 44.77[1] |
| HNO2 (g) trans | -80.12[1] | -45.24[1] | 249.22[1] | 46.07[1] |
| HNO2 (g) | -79.5[1] | -46.0[1] | 254.1[1] | 45.6[1] |
| HNO2 (ao) | -119.2[1] | -50.6[1] | 135.6[1] | – |
| FeCl2+ (ao) | -180.3[1] | -143.9[1] | -113[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, (cr):Crystalline solid, (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°, -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°, 80.3 kJ · mol−1
- ^ ΔfG°, 97.9 kJ · mol−1
- ^ S°, 266.21 J · K−1 · mol−1
- ^ Cp°, 45.40 J · K−1 · mol−1
- ^ ΔfH°, -77.99 kJ · mol−1
- ^ ΔfG°, -42.94 kJ · mol−1
- ^ S°, 248.76 J · K−1 · mol−1
- ^ Cp°, 44.77 J · K−1 · mol−1
- ^ ΔfH°, -80.12 kJ · mol−1
- ^ ΔfG°, -45.24 kJ · mol−1
- ^ S°, 249.22 J · K−1 · mol−1
- ^ Cp°, 46.07 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -46.0 kJ · mol−1
- ^ S°, 254.1 J · K−1 · mol−1
- ^ Cp°, 45.6 J · K−1 · mol−1
- ^ ΔfH°, -119.2 kJ · mol−1
- ^ ΔfG°, -50.6 kJ · mol−1
- ^ S°, 135.6 J · K−1 · mol−1
- ^ ΔfH°, -180.3 kJ · mol−1
- ^ ΔfG°, -143.9 kJ · mol−1
- ^ S°, -113. 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