Na3[Fe(CN)6] + 27HNO3 → 3NaHCO3 + Fe(NO3)3 + 24HNO2 + 3N2O3↑ + 3CO2↑
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The reaction of sodium hexacyanidoferrate(III) and nitric acid yields sodium hydrogencarbonate, iron(III) nitrate, nitrous acid, 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 sodium 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 sodium hexacyanidoferrate(III) and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na3[Fe(CN)6] | Sodium hexacyanidoferrate(III) | 1 | Reducing | Reducing |
| HNO3 | Nitric acid | 27 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHCO3 | Sodium hydrogencarbonate | 3 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 1 | – | – |
| HNO2 | Nitrous acid | 24 | Reduced | – |
| N2O3 | Dinitrogen trioxide | 3 | Oxidized | – |
| CO2 | Carbon dioxide | 3 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1803.2 kJ/mol K 8.07 × 10315 pK −315.91
| 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 | −1499.9 | −1803.2 | 1006.4 | – |
per 1 mol of | −1499.9 | −1803.2 | 1006.4 | – |
per 1 mol of | −55.552 | −66.785 | 37.274 | – |
per 1 mol of | −499.97 | −601.07 | 335.47 | – |
per 1 mol of | −1499.9 | −1803.2 | 1006.4 | – |
per 1 mol of | −62.496 | −75.133 | 41.933 | – |
per 1 mol of | −499.97 | −601.07 | 335.47 | – |
per 1 mol of | −499.97 | −601.07 | 335.47 | – |
Changes in aqueous solution (2)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1778.1 kJ/mol K 3.23 × 10311 pK −311.51
| 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 | −1560.8 | −1778.1 | 717.9 | – |
per 1 mol of | −1560.8 | −1778.1 | 717.9 | – |
per 1 mol of | −57.807 | −65.856 | 26.59 | – |
per 1 mol of | −520.27 | −592.70 | 239.3 | – |
per 1 mol of | −1560.8 | −1778.1 | 717.9 | – |
per 1 mol of | −65.033 | −74.087 | 29.91 | – |
per 1 mol of | −520.27 | −592.70 | 239.3 | – |
per 1 mol of | −520.27 | −592.70 | 239.3 | – |
Changes in aqueous solution (3)
- Reaction of sodium 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 | −1504.1 | – | – | – |
per 1 mol of | −1504.1 | – | – | – |
per 1 mol of | −55.707 | – | – | – |
per 1 mol of | −501.37 | – | – | – |
per 1 mol of | −1504.1 | – | – | – |
per 1 mol of | −62.671 | – | – | – |
per 1 mol of | −501.37 | – | – | – |
per 1 mol of | −501.37 | – | – | – |
Changes in aqueous solution (4)
- Reaction of sodium 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 | −1565.0 | – | – | – |
per 1 mol of | −1565.0 | – | – | – |
per 1 mol of | −57.963 | – | – | – |
per 1 mol of | −521.67 | – | – | – |
per 1 mol of | −1565.0 | – | – | – |
per 1 mol of | −65.208 | – | – | – |
per 1 mol of | −521.67 | – | – | – |
per 1 mol of | −521.67 | – | – | – |
Changes in aqueous solution (5)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1806.3 kJ/mol K 2.82 × 10316 pK −316.45
| 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 | −1535.2 | −1806.3 | 897.2 | – |
per 1 mol of | −1535.2 | −1806.3 | 897.2 | – |
per 1 mol of | −56.859 | −66.900 | 33.23 | – |
per 1 mol of | −511.73 | −602.10 | 299.1 | – |
per 1 mol of | −1535.2 | −1806.3 | 897.2 | – |
per 1 mol of | −63.967 | −75.263 | 37.38 | – |
per 1 mol of | −511.73 | −602.10 | 299.1 | – |
per 1 mol of | −511.73 | −602.10 | 299.1 | – |
Changes in aqueous solution (6)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1781.2 kJ/mol K 1.13 × 10312 pK −312.05
| 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 | −1596.1 | −1781.2 | 608.7 | – |
per 1 mol of | −1596.1 | −1781.2 | 608.7 | – |
per 1 mol of | −59.115 | −65.970 | 22.54 | – |
per 1 mol of | −532.03 | −593.73 | 202.9 | – |
per 1 mol of | −1596.1 | −1781.2 | 608.7 | – |
per 1 mol of | −66.504 | −74.217 | 25.36 | – |
per 1 mol of | −532.03 | −593.73 | 202.9 | – |
per 1 mol of | −532.03 | −593.73 | 202.9 | – |
Changes in aqueous solution (7)
- Reaction of sodium 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 | −1539.4 | – | – | – |
per 1 mol of | −1539.4 | – | – | – |
per 1 mol of | −57.015 | – | – | – |
per 1 mol of | −513.13 | – | – | – |
per 1 mol of | −1539.4 | – | – | – |
per 1 mol of | −64.142 | – | – | – |
per 1 mol of | −513.13 | – | – | – |
per 1 mol of | −513.13 | – | – | – |
Changes in aqueous solution (8)
- Reaction of sodium 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 | −1600.3 | – | – | – |
per 1 mol of | −1600.3 | – | – | – |
per 1 mol of | −59.270 | – | – | – |
per 1 mol of | −533.43 | – | – | – |
per 1 mol of | −1600.3 | – | – | – |
per 1 mol of | −66.679 | – | – | – |
per 1 mol of | −533.43 | – | – | – |
per 1 mol of | −533.43 | – | – | – |
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 |
|---|---|---|---|---|
| Na3[Fe(CN)6] (ai) | -158.6[1] | -56.4[1] | 447.3[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] |
* (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 |
|---|---|---|---|---|
| NaHCO3 (cr) | -950.81[1] | -851.0[1] | 101.7[1] | 87.61[1] |
| NaHCO3 (ai) | -932.11[1] | -848.66[1] | 150.2[1] | – |
| NaHCO3 (ao) | -943.9[1] | -849.7[1] | 113.8[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] | – | – | – |
| 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] | – |
| 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, (ao):Un-ionized aqueous solution, (aq):Aqueous solution, (g):Gas, (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°, -158.6 kJ · mol−1
- ^ ΔfG°, -56.4 kJ · mol−1
- ^ S°, 447.3 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°, -950.81 kJ · mol−1
- ^ ΔfG°, -851.0 kJ · mol−1
- ^ S°, 101.7 J · K−1 · mol−1
- ^ Cp°, 87.61 J · K−1 · mol−1
- ^ ΔfH°, -932.11 kJ · mol−1
- ^ ΔfG°, -848.66 kJ · mol−1
- ^ S°, 150.2 J · K−1 · mol−1
- ^ ΔfH°, -943.9 kJ · mol−1
- ^ ΔfG°, -849.7 kJ · mol−1
- ^ S°, 113.8 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°, -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°, 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