3FeI2 + 7HNO3 + 9H+ 🔥→ 3Fe3+ + 3HIO3 + 7NO↑ + 5H2O + 3HI↑
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- Reaction of iron(II) iodide and nitric acid under acidic condition
- 3FeI2Iron(II) iodide + 7HNO3Nitric acid + 9H+Hydrogen ion3Fe3+Iron(III) ion + 3HIO3Iodic acid + 7NO↑Nitrogen monoxide + 5H2OWater + 3HI↑Hydrogen iodide🔥⟶
The reaction of iron(II) iodide, nitric acid, and hydrogen ion yields iron(III) ion, iodic acid, nitrogen monoxide, water, and hydrogen iodide (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) iodide and nitric acid under acidic condition
- 3FeI2Iron(II) iodide + 7HNO3Nitric acid + 9H+Hydrogen ion3Fe3+Iron(III) ion + 3HIO3Iodic acid + 7NO↑Nitrogen monoxide + 5H2OWater + 3HI↑Hydrogen iodide🔥⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of iron(II) iodide and nitric acid under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeI2 | Iron(II) iodide | 3 | Reducing | Oxidizable |
| HNO3 | Nitric acid | 7 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 9 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Fe3+ | Iron(III) ion | 3 | Oxidized | – |
| HIO3 | Iodic acid | 3 | Oxidized | – |
| NO | Nitrogen monoxide | 7 | Reduced | – |
| H2O | Water | 5 | – | Water |
| HI | Hydrogen iodide | 3 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) iodide and nitric acid under acidic condition◆
ΔrG 338.3 kJ/mol K 0.54 × 10−59 pK 59.27
| 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 | 553.0 | 338.3 | 718.2 | – |
per 1 mol of | 184.3 | 112.8 | 239.4 | – |
per 1 mol of | 79.00 | 48.33 | 102.6 | – |
per 1 mol of Hydrogen ion | 61.44 | 37.59 | 79.80 | – |
per 1 mol of Iron(III) ion | 184.3 | 112.8 | 239.4 | – |
per 1 mol of | 184.3 | 112.8 | 239.4 | – |
per 1 mol of | 79.00 | 48.33 | 102.6 | – |
per 1 mol of | 110.6 | 67.66 | 143.6 | – |
per 1 mol of | 184.3 | 112.8 | 239.4 | – |
Changes in standard condition (2)
- Reaction of iron(II) iodide and nitric acid under acidic condition◆
ΔrG 178.5 kJ/mol K 0.53 × 10−31 pK 31.27
| 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 | 308.0 | 178.5 | 432.3 | – |
per 1 mol of | 102.7 | 59.50 | 144.1 | – |
per 1 mol of | 44.00 | 25.50 | 61.76 | – |
per 1 mol of Hydrogen ion | 34.22 | 19.83 | 48.03 | – |
per 1 mol of Iron(III) ion | 102.7 | 59.50 | 144.1 | – |
per 1 mol of | 102.7 | 59.50 | 144.1 | – |
per 1 mol of | 44.00 | 25.50 | 61.76 | – |
per 1 mol of | 61.60 | 35.70 | 86.46 | – |
per 1 mol of | 102.7 | 59.50 | 144.1 | – |
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 |
|---|---|---|---|---|
| FeI2 (cr) | -113.0[1] | – | – | – |
| FeI2 (g) | 60.7[1] | – | – | – |
| FeI2 (ai) | -199.6[1] | -182.05[1] | 84.9[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] |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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 |
|---|---|---|---|---|
| Fe3+ (g) | 5712.8[1] | – | – | – |
| Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[1] | – |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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] |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (ai):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°, -113.0 kJ · mol−1
- ^ ΔfH°, 60.7 kJ · mol−1
- ^ ΔfH°, -199.6 kJ · mol−1
- ^ ΔfG°, -182.05 kJ · mol−1
- ^ S°, 84.9 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°, 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°, 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°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 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°, -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
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1