K3[Fe(CN)6] + 60HNO3 → 3KNO3 + Fe(NO3)3 + 60NO2↑ + 6CO2↑ + 30H2O
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The reaction of potassium hexacyanidoferrate(III) and nitric acid yields potassium nitrate, iron(III) nitrate, nitrogen dioxide, carbon dioxide, 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 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 | 60 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO3 | Potassium nitrate | 3 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 1 | Oxidized | – |
| NO2 | Nitrogen dioxide | 60 | Reduced | – |
| CO2 | Carbon dioxide | 6 | Oxidized | – |
| H2O | Water | 30 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1127.9 kJ/mol K 3.98 × 10197 pK −197.60
| 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 | 1641.9 | −1127.9 | 9291.6 | – |
per 1 mol of | 1641.9 | −1127.9 | 9291.6 | – |
per 1 mol of | 27.365 | −18.798 | 154.86 | – |
per 1 mol of | 547.30 | −375.97 | 3097.2 | – |
per 1 mol of | 1641.9 | −1127.9 | 9291.6 | – |
per 1 mol of | 27.365 | −18.798 | 154.86 | – |
per 1 mol of | 273.65 | −187.98 | 1548.6 | – |
per 1 mol of | 54.730 | −37.597 | 309.72 | – |
Changes in aqueous solution (2)
- Reaction of potassium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1077.6 kJ/mol K 6.13 × 10188 pK −188.79
| 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 | 1520.2 | −1077.6 | 8714.8 | – |
per 1 mol of | 1520.2 | −1077.6 | 8714.8 | – |
per 1 mol of | 25.337 | −17.960 | 145.25 | – |
per 1 mol of | 506.73 | −359.20 | 2904.9 | – |
per 1 mol of | 1520.2 | −1077.6 | 8714.8 | – |
per 1 mol of | 25.337 | −17.960 | 145.25 | – |
per 1 mol of | 253.37 | −179.60 | 1452.5 | – |
per 1 mol of | 50.673 | −35.920 | 290.49 | – |
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 | 1637.7 | – | – | – |
per 1 mol of | 1637.7 | – | – | – |
per 1 mol of | 27.295 | – | – | – |
per 1 mol of | 545.90 | – | – | – |
per 1 mol of | 1637.7 | – | – | – |
per 1 mol of | 27.295 | – | – | – |
per 1 mol of | 272.95 | – | – | – |
per 1 mol of | 54.590 | – | – | – |
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 | 1516.0 | – | – | – |
per 1 mol of | 1516.0 | – | – | – |
per 1 mol of | 25.267 | – | – | – |
per 1 mol of | 505.33 | – | – | – |
per 1 mol of | 1516.0 | – | – | – |
per 1 mol of | 25.267 | – | – | – |
per 1 mol of | 252.67 | – | – | – |
per 1 mol of | 50.533 | – | – | – |
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 |
|---|---|---|---|---|
| KNO3 (cr) | -494.63[1] | -394.86[1] | 133.05[1] | 96.40[1] |
| KNO3 (ai) | -459.74[1] | -394.53[1] | 248.9[1] | -64.9[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] | – | – | – |
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[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] | – |
| 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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -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°, -494.63 kJ · mol−1
- ^ ΔfG°, -394.86 kJ · mol−1
- ^ S°, 133.05 J · K−1 · mol−1
- ^ Cp°, 96.40 J · K−1 · mol−1
- ^ ΔfH°, -459.74 kJ · mol−1
- ^ ΔfG°, -394.53 kJ · mol−1
- ^ S°, 248.9 J · K−1 · mol−1
- ^ Cp°, -64.9 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°, 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°, -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
- ^ 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