12HCl + 9Fe(NO3)3 + 18H+ 🔥→ 6Cl2O + 9Fe2+ + 5NO + 22HNO3 + 4H2O
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- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition
- 12HClHydrogen chloride + 9Fe(NO3)3Iron(III) nitrate + 18H+Hydrogen ion6Cl2ODichlorine monoxide + 9Fe2+Iron(II) ion + 5NONitrogen monoxide + 22HNO3Nitric acid + 4H2OWater🔥⟶
The reaction of hydrogen chloride, iron(III) nitrate, and hydrogen ion yields dichlorine monoxide, iron(II) ion, nitrogen monoxide, 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
- 12HClHydrogen chloride + 9Fe(NO3)3Iron(III) nitrate + 18H+Hydrogen ion6Cl2ODichlorine monoxide + 9Fe2+Iron(II) ion + 5NONitrogen monoxide + 22HNO3Nitric acid + 4H2OWater🔥⟶
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 | 12 | Reducing | Hardly oxidizable |
| Fe(NO3)3 | Iron(III) nitrate | 9 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 18 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cl2O | Dichlorine monoxide | 6 | Oxidized | – |
| Fe2+ | Iron(II) ion | 9 | Reduced | – |
| NO | Nitrogen monoxide | 5 | Reduced | – |
| HNO3 | Nitric acid | 22 | – | – |
| H2O | Water | 4 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen chloride and iron(III) nitrate under acidic condition◆
ΔrG 1533.5 kJ/mol K 0.22 × 10−268 pK 268.66
| 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 | 2468.1 | 1533.5 | 3123.6 | – |
per 1 mol of | 205.67 | 127.79 | 260.30 | – |
per 1 mol of | 274.23 | 170.39 | 347.07 | – |
per 1 mol of Hydrogen ion | 137.12 | 85.194 | 173.53 | – |
per 1 mol of | 411.35 | 255.58 | 520.60 | – |
per 1 mol of Iron(II) ion | 274.23 | 170.39 | 347.07 | – |
per 1 mol of | 493.62 | 306.70 | 624.72 | – |
per 1 mol of | 112.19 | 69.705 | 141.98 | – |
per 1 mol of | 617.02 | 383.38 | 780.90 | – |
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 | 2505.9 | – | – | – |
per 1 mol of | 208.83 | – | – | – |
per 1 mol of | 278.43 | – | – | – |
per 1 mol of Hydrogen ion | 139.22 | – | – | – |
per 1 mol of | 417.65 | – | – | – |
per 1 mol of Iron(II) ion | 278.43 | – | – | – |
per 1 mol of | 501.18 | – | – | – |
per 1 mol of | 113.90 | – | – | – |
per 1 mol of | 626.48 | – | – | – |
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] |
| Fe2+ (g) | 2749.93[1] | – | – | – |
| Fe2+ (ao) | -89.1[1] | -78.90[1] | -137.7[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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°, 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°, 2749.93 kJ · mol−1
- ^ ΔfH°, -89.1 kJ · mol−1
- ^ ΔfG°, -78.90 kJ · mol−1
- ^ S°, -137.7 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 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