Na4[Fe(CN)6] + 14HNO3 → 4NaHCO3 + 20NO↑ + FeCO3 + CO2↑ + 5H2O
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The reaction of sodium hexacyanidoferrate(II) and nitric acid yields sodium hydrogencarbonate, nitrogen monoxide, iron(II) carbonate, 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 sodium hexacyanidoferrate(II) 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(II) and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na4[Fe(CN)6] | Sodium hexacyanidoferrate(II) | 1 | Reducing | Reducing |
| HNO3 | Nitric acid | 14 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHCO3 | Sodium hydrogencarbonate | 4 | Oxidized | – |
| NO | Nitrogen monoxide | 20 | Redoxed product | – |
| FeCO3 | Iron(II) carbonate | 1 | Oxidized | – |
| CO2 | Carbon dioxide | 1 | Oxidized | – |
| H2O | Water | 5 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −2000.28 kJ/mol K 2.72 × 10350 pK −350.43
| 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 | −1078.6 | −2000.28 | 3091.6 | – |
per 1 mol of | −1078.6 | −2000.28 | 3091.6 | – |
per 1 mol of | −77.043 | −142.877 | 220.83 | – |
per 1 mol of | −269.65 | −500.070 | 772.90 | – |
per 1 mol of | −53.930 | −100.014 | 154.58 | – |
per 1 mol of | −1078.6 | −2000.28 | 3091.6 | – |
per 1 mol of | −1078.6 | −2000.28 | 3091.6 | – |
per 1 mol of | −215.72 | −400.056 | 618.32 | – |
Changes in aqueous solution (2)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −1991.91 kJ/mol K 9.28 × 10348 pK −348.97
| 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 | −1098.9 | −1991.91 | 2995.5 | – |
per 1 mol of | −1098.9 | −1991.91 | 2995.5 | – |
per 1 mol of | −78.493 | −142.279 | 213.96 | – |
per 1 mol of | −274.73 | −497.978 | 748.88 | – |
per 1 mol of | −54.945 | −99.5955 | 149.78 | – |
per 1 mol of | −1098.9 | −1991.91 | 2995.5 | – |
per 1 mol of | −1098.9 | −1991.91 | 2995.5 | – |
per 1 mol of | −219.78 | −398.382 | 599.10 | – |
Changes in aqueous solution (3)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −2004.4 kJ/mol K 1.43 × 10351 pK −351.16
| 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 | −1125.8 | −2004.4 | 2946.0 | – |
per 1 mol of | −1125.8 | −2004.4 | 2946.0 | – |
per 1 mol of | −80.414 | −143.17 | 210.43 | – |
per 1 mol of | −281.45 | −501.10 | 736.50 | – |
per 1 mol of | −56.290 | −100.22 | 147.30 | – |
per 1 mol of | −1125.8 | −2004.4 | 2946.0 | – |
per 1 mol of | −1125.8 | −2004.4 | 2946.0 | – |
per 1 mol of | −225.16 | −400.88 | 589.20 | – |
Changes in aqueous solution (4)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −1996.1 kJ/mol K 5.03 × 10349 pK −349.70
| 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 | −1146.1 | −1996.1 | 2849.9 | – |
per 1 mol of | −1146.1 | −1996.1 | 2849.9 | – |
per 1 mol of | −81.864 | −142.58 | 203.56 | – |
per 1 mol of | −286.52 | −499.02 | 712.48 | – |
per 1 mol of | −57.305 | −99.805 | 142.50 | – |
per 1 mol of | −1146.1 | −1996.1 | 2849.9 | – |
per 1 mol of | −1146.1 | −1996.1 | 2849.9 | – |
per 1 mol of | −229.22 | −399.22 | 569.98 | – |
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 |
|---|---|---|---|---|
| Na4[Fe(CN)6] (ai) | -505.0[1] | -352.53[1] | 331.0[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] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[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, (ao):Un-ionized 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°, -505.0 kJ · mol−1
- ^ ΔfG°, -352.53 kJ · mol−1
- ^ S°, 331.0 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°, 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°, -740.57 kJ · mol−1
- ^ ΔfG°, -666.67 kJ · mol−1
- ^ S°, 92.9 J · K−1 · mol−1
- ^ Cp°, 82.13 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