8Na4[Fe(CN)6] + 98HNO3 → 32NaHCO3 + 8Fe(NO3)3 + 61N2O↑ + 16CO2↑ + 33H2O
Last updated:
The reaction of sodium hexacyanidoferrate(II) and nitric acid yields sodium hydrogencarbonate, iron(III) nitrate, dinitrotgen monoxide, 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) | 8 | Reducing | Reducing |
| HNO3 | Nitric acid | 98 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHCO3 | Sodium hydrogencarbonate | 32 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 8 | Oxidized | – |
| N2O | Dinitrotgen monoxide | 61 | Redoxed product | – |
| CO2 | Carbon dioxide | 16 | Oxidized | – |
| H2O | Water | 33 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −23919.6 kJ/mol K 3.41 × 104190 pK −4190.53
| 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 | −21555.3 | −23919.6 | 7936.1 | – |
per 1 mol of | −2694.41 | −2989.95 | 992.01 | – |
per 1 mol of | −219.952 | −244.078 | 80.981 | – |
per 1 mol of | −673.603 | −747.487 | 248.00 | – |
per 1 mol of | −2694.41 | −2989.95 | 992.01 | – |
per 1 mol of | −353.366 | −392.125 | 130.10 | – |
per 1 mol of | −1347.21 | −1494.97 | 496.01 | – |
per 1 mol of | −653.191 | −724.836 | 240.49 | – |
Changes in aqueous solution (2)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −23785.5 kJ/mol K 1.09 × 104167 pK −4167.04
| 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 | −21880.0 | −23785.5 | 6397.9 | – |
per 1 mol of | −2735.00 | −2973.19 | 799.74 | – |
per 1 mol of | −223.265 | −242.709 | 65.285 | – |
per 1 mol of | −683.750 | −743.297 | 199.93 | – |
per 1 mol of | −2735.00 | −2973.19 | 799.74 | – |
per 1 mol of | −358.689 | −389.926 | 104.88 | – |
per 1 mol of | −1367.50 | −1486.59 | 399.87 | – |
per 1 mol of | −663.030 | −720.773 | 193.88 | – |
Changes in aqueous solution (3)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23138.3 | – | – | – |
per 1 mol of | −2892.29 | – | – | – |
per 1 mol of | −236.105 | – | – | – |
per 1 mol of | −723.072 | – | – | – |
per 1 mol of | −2892.29 | – | – | – |
per 1 mol of | −379.316 | – | – | – |
per 1 mol of | −1446.14 | – | – | – |
per 1 mol of | −701.161 | – | – | – |
Changes in aqueous solution (4)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23462.9 | – | – | – |
per 1 mol of | −2932.86 | – | – | – |
per 1 mol of | −239.417 | – | – | – |
per 1 mol of | −733.216 | – | – | – |
per 1 mol of | −2932.86 | – | – | – |
per 1 mol of | −384.638 | – | – | – |
per 1 mol of | −1466.43 | – | – | – |
per 1 mol of | −710.997 | – | – | – |
Changes in aqueous solution (5)
- Reaction of sodium hexacyanidoferrate(II) 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 | −21588.9 | – | – | – |
per 1 mol of | −2698.61 | – | – | – |
per 1 mol of | −220.295 | – | – | – |
per 1 mol of | −674.653 | – | – | – |
per 1 mol of | −2698.61 | – | – | – |
per 1 mol of | −353.916 | – | – | – |
per 1 mol of | −1349.31 | – | – | – |
per 1 mol of | −654.209 | – | – | – |
Changes in aqueous solution (6)
- Reaction of sodium hexacyanidoferrate(II) 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 | −21913.6 | – | – | – |
per 1 mol of | −2739.20 | – | – | – |
per 1 mol of | −223.608 | – | – | – |
per 1 mol of | −684.800 | – | – | – |
per 1 mol of | −2739.20 | – | – | – |
per 1 mol of | −359.239 | – | – | – |
per 1 mol of | −1369.60 | – | – | – |
per 1 mol of | −664.048 | – | – | – |
Changes in aqueous solution (7)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23171.9 | – | – | – |
per 1 mol of | −2896.49 | – | – | – |
per 1 mol of | −236.448 | – | – | – |
per 1 mol of | −724.122 | – | – | – |
per 1 mol of | −2896.49 | – | – | – |
per 1 mol of | −379.867 | – | – | – |
per 1 mol of | −1448.24 | – | – | – |
per 1 mol of | −702.179 | – | – | – |
Changes in aqueous solution (8)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23496.5 | – | – | – |
per 1 mol of | −2937.06 | – | – | – |
per 1 mol of | −239.760 | – | – | – |
per 1 mol of | −734.266 | – | – | – |
per 1 mol of | −2937.06 | – | – | – |
per 1 mol of | −385.189 | – | – | – |
per 1 mol of | −1468.53 | – | – | – |
per 1 mol of | −712.015 | – | – | – |
Changes in aqueous solution (9)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −23952.9 kJ/mol K 2.33 × 104196 pK −4196.37
| 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 | −21932.6 | −23952.9 | 6771.3 | – |
per 1 mol of | −2741.57 | −2994.11 | 846.41 | – |
per 1 mol of | −223.802 | −244.417 | 69.095 | – |
per 1 mol of | −685.394 | −748.528 | 211.60 | – |
per 1 mol of | −2741.57 | −2994.11 | 846.41 | – |
per 1 mol of | −359.551 | −392.670 | 111.00 | – |
per 1 mol of | −1370.79 | −1497.06 | 423.21 | – |
per 1 mol of | −664.624 | −725.845 | 205.19 | – |
Changes in aqueous solution (10)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −23818.8 kJ/mol K 7.47 × 104172 pK −4172.87
| 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 | −22257.3 | −23818.8 | 5233.1 | – |
per 1 mol of | −2782.16 | −2977.35 | 654.14 | – |
per 1 mol of | −227.115 | −243.049 | 53.399 | – |
per 1 mol of | −695.541 | −744.337 | 163.53 | – |
per 1 mol of | −2782.16 | −2977.35 | 654.14 | – |
per 1 mol of | −364.874 | −390.472 | 85.789 | – |
per 1 mol of | −1391.08 | −1488.67 | 327.07 | – |
per 1 mol of | −674.464 | −721.782 | 158.58 | – |
Changes in aqueous solution (11)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23515.6 | – | – | – |
per 1 mol of | −2939.45 | – | – | – |
per 1 mol of | −239.955 | – | – | – |
per 1 mol of | −734.862 | – | – | – |
per 1 mol of | −2939.45 | – | – | – |
per 1 mol of | −385.502 | – | – | – |
per 1 mol of | −1469.72 | – | – | – |
per 1 mol of | −712.594 | – | – | – |
Changes in aqueous solution (12)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23840.2 | – | – | – |
per 1 mol of | −2980.03 | – | – | – |
per 1 mol of | −243.267 | – | – | – |
per 1 mol of | −745.006 | – | – | – |
per 1 mol of | −2980.03 | – | – | – |
per 1 mol of | −390.823 | – | – | – |
per 1 mol of | −1490.01 | – | – | – |
per 1 mol of | −722.430 | – | – | – |
Changes in aqueous solution (13)
- Reaction of sodium hexacyanidoferrate(II) 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 | −21966.2 | – | – | – |
per 1 mol of | −2745.78 | – | – | – |
per 1 mol of | −224.145 | – | – | – |
per 1 mol of | −686.444 | – | – | – |
per 1 mol of | −2745.78 | – | – | – |
per 1 mol of | −360.102 | – | – | – |
per 1 mol of | −1372.89 | – | – | – |
per 1 mol of | −665.642 | – | – | – |
Changes in aqueous solution (14)
- Reaction of sodium hexacyanidoferrate(II) 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 | −22290.9 | – | – | – |
per 1 mol of | −2786.36 | – | – | – |
per 1 mol of | −227.458 | – | – | – |
per 1 mol of | −696.591 | – | – | – |
per 1 mol of | −2786.36 | – | – | – |
per 1 mol of | −365.425 | – | – | – |
per 1 mol of | −1393.18 | – | – | – |
per 1 mol of | −675.482 | – | – | – |
Changes in aqueous solution (15)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23549.2 | – | – | – |
per 1 mol of | −2943.65 | – | – | – |
per 1 mol of | −240.298 | – | – | – |
per 1 mol of | −735.913 | – | – | – |
per 1 mol of | −2943.65 | – | – | – |
per 1 mol of | −386.052 | – | – | – |
per 1 mol of | −1471.83 | – | – | – |
per 1 mol of | −713.612 | – | – | – |
Changes in aqueous solution (16)
- Reaction of sodium hexacyanidoferrate(II) 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 | −23873.8 | – | – | – |
per 1 mol of | −2984.22 | – | – | – |
per 1 mol of | −243.610 | – | – | – |
per 1 mol of | −746.056 | – | – | – |
per 1 mol of | −2984.22 | – | – | – |
per 1 mol of | −391.374 | – | – | – |
per 1 mol of | −1492.11 | – | – | – |
per 1 mol of | −723.448 | – | – | – |
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] | – |
| 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] | – | – | – |
| N2O (g) | 82.05[1] | 104.20[1] | 219.85[1] | 38.45[1] |
| N2O (aq) | 56.1[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, (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°, -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°, -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°, 82.05 kJ · mol−1
- ^ ΔfG°, 104.20 kJ · mol−1
- ^ S°, 219.85 J · K−1 · mol−1
- ^ Cp°, 38.45 J · K−1 · mol−1
- ^ ΔfH°, 56.1 kJ · 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