K3[Fe(CN)6] + 19HNO3 → 3KHCO3 + Fe(NO3)3 + 4NH4NO3 + 7N2O3↑ + 3CO2↑
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The reaction of potassium hexacyanidoferrate(III) and nitric acid yields potassium hydrogencarbonate, iron(III) nitrate, ammonium nitrate, dinitrogen trioxide, and carbon dioxide (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 potassium hexacyanidoferrate(III) 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 potassium hexacyanidoferrate(III) and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K3[Fe(CN)6] | Potassium hexacyanidoferrate(III) | 1 | Reducing | Reducing |
| HNO3 | Nitric acid | 19 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KHCO3 | Potassium hydrogencarbonate | 3 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 1 | – | – |
| NH4NO3 | Ammonium nitrate | 4 | – | – |
| N2O3 | Dinitrogen trioxide | 7 | Redoxed product | – |
| CO2 | Carbon dioxide | 3 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1683.4 kJ/mol K 8.30 × 10294 pK −294.92
| 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 | −1322.5 | −1683.4 | 1211.5 | – |
per 1 mol of | −1322.5 | −1683.4 | 1211.5 | – |
per 1 mol of | −69.605 | −88.600 | 63.763 | – |
per 1 mol of | −440.83 | −561.13 | 403.83 | – |
per 1 mol of | −1322.5 | −1683.4 | 1211.5 | – |
per 1 mol of | −330.63 | −420.85 | 302.88 | – |
per 1 mol of | −188.93 | −240.49 | 173.07 | – |
per 1 mol of | −440.83 | −561.13 | 403.83 | – |
Changes in aqueous solution (2)
- Reaction of potassium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1658.2 kJ/mol K 3.19 × 10290 pK −290.50
| 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 | −1383.4 | −1658.2 | 923.1 | – |
per 1 mol of | −1383.4 | −1658.2 | 923.1 | – |
per 1 mol of | −72.811 | −87.274 | 48.58 | – |
per 1 mol of | −461.13 | −552.73 | 307.7 | – |
per 1 mol of | −1383.4 | −1658.2 | 923.1 | – |
per 1 mol of | −345.85 | −414.55 | 230.8 | – |
per 1 mol of | −197.63 | −236.89 | 131.9 | – |
per 1 mol of | −461.13 | −552.73 | 307.7 | – |
Changes in aqueous solution (3)
- Reaction of potassium hexacyanidoferrate(III) 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 | −1326.7 | – | – | – |
per 1 mol of | −1326.7 | – | – | – |
per 1 mol of | −69.826 | – | – | – |
per 1 mol of | −442.23 | – | – | – |
per 1 mol of | −1326.7 | – | – | – |
per 1 mol of | −331.68 | – | – | – |
per 1 mol of | −189.53 | – | – | – |
per 1 mol of | −442.23 | – | – | – |
Changes in aqueous solution (4)
- Reaction of potassium hexacyanidoferrate(III) 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 | −1387.6 | – | – | – |
per 1 mol of | −1387.6 | – | – | – |
per 1 mol of | −73.032 | – | – | – |
per 1 mol of | −462.53 | – | – | – |
per 1 mol of | −1387.6 | – | – | – |
per 1 mol of | −346.90 | – | – | – |
per 1 mol of | −198.23 | – | – | – |
per 1 mol of | −462.53 | – | – | – |
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 |
|---|---|---|---|---|
| K3[Fe(CN)6] (cr) | -249.8[1] | -129.6[1] | 426.06[1] | – |
| K3[Fe(CN)6] (ai) | -195.4[1] | -120.4[1] | 577.8[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| KHCO3 (cr) | -963.2[1] | -863.5[1] | 115.5[1] | – |
| KHCO3 (ai) | -944.37[1] | -870.04[1] | 193.7[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] | – | – | – |
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
| N2O3 (l) | 50.29[1] | – | – | – |
| N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[1] |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (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°, -249.8 kJ · mol−1
- ^ ΔfG°, -129.6 kJ · mol−1
- ^ S°, 426.06 J · K−1 · mol−1
- ^ ΔfH°, -195.4 kJ · mol−1
- ^ ΔfG°, -120.4 kJ · mol−1
- ^ S°, 577.8 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°, -963.2 kJ · mol−1
- ^ ΔfG°, -863.5 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ ΔfH°, -944.37 kJ · mol−1
- ^ ΔfG°, -870.04 kJ · mol−1
- ^ S°, 193.7 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°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 J · K−1 · mol−1
- ^ ΔfH°, 50.29 kJ · mol−1
- ^ ΔfH°, 83.72 kJ · mol−1
- ^ ΔfG°, 139.46 kJ · mol−1
- ^ S°, 312.28 J · K−1 · mol−1
- ^ Cp°, 65.61 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 J · K−1 · mol−1