8Na4[Fe(CN)6] + 98HNO3 → 32NaHCO3 + 8Fe(NO3)3 + 61N2O↑ + 16H2CO3 + 17H2O
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The reaction of sodium hexacyanidoferrate(II) and nitric acid yields sodium hydrogencarbonate, iron(III) nitrate, dinitrotgen monoxide, carbonic acid, 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 | – |
| H2CO3 | Carbonic acid | 16 | Oxidized | – |
| H2O | Water | 17 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −23785.1 kJ/mol K 9.32 × 104166 pK −4166.97
| 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 | −21880.3 | −23785.1 | 6396.1 | – |
per 1 mol of | −2735.04 | −2973.14 | 799.51 | – |
per 1 mol of | −223.268 | −242.705 | 65.266 | – |
per 1 mol of | −683.759 | −743.284 | 199.88 | – |
per 1 mol of | −2735.04 | −2973.14 | 799.51 | – |
per 1 mol of | −358.693 | −389.920 | 104.85 | – |
per 1 mol of | −1367.52 | −1486.57 | 399.76 | – |
per 1 mol of | −1287.08 | −1399.12 | 376.24 | – |
Changes in aqueous solution (2)
- 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 | −23463.3 | – | – | – |
per 1 mol of | −2932.91 | – | – | – |
per 1 mol of | −239.421 | – | – | – |
per 1 mol of | −733.228 | – | – | – |
per 1 mol of | −2932.91 | – | – | – |
per 1 mol of | −384.644 | – | – | – |
per 1 mol of | −1466.46 | – | – | – |
per 1 mol of | −1380.19 | – | – | – |
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 | −21913.9 | – | – | – |
per 1 mol of | −2739.24 | – | – | – |
per 1 mol of | −223.611 | – | – | – |
per 1 mol of | −684.809 | – | – | – |
per 1 mol of | −2739.24 | – | – | – |
per 1 mol of | −359.244 | – | – | – |
per 1 mol of | −1369.62 | – | – | – |
per 1 mol of | −1289.05 | – | – | – |
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 | −23496.9 | – | – | – |
per 1 mol of | −2937.11 | – | – | – |
per 1 mol of | −239.764 | – | – | – |
per 1 mol of | −734.278 | – | – | – |
per 1 mol of | −2937.11 | – | – | – |
per 1 mol of | −385.195 | – | – | – |
per 1 mol of | −1468.56 | – | – | – |
per 1 mol of | −1382.17 | – | – | – |
Changes in aqueous solution (5)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −23818.3 kJ/mol K 6.10 × 104172 pK −4172.79
| 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 | −22257.6 | −23818.3 | 5231.3 | – |
per 1 mol of | −2782.20 | −2977.29 | 653.91 | – |
per 1 mol of | −227.118 | −243.044 | 53.381 | – |
per 1 mol of | −695.550 | −744.322 | 163.48 | – |
per 1 mol of | −2782.20 | −2977.29 | 653.91 | – |
per 1 mol of | −364.879 | −390.464 | 85.759 | – |
per 1 mol of | −1391.10 | −1488.64 | 326.96 | – |
per 1 mol of | −1309.27 | −1401.08 | 307.72 | – |
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 | −23840.5 | – | – | – |
per 1 mol of | −2980.06 | – | – | – |
per 1 mol of | −243.270 | – | – | – |
per 1 mol of | −745.016 | – | – | – |
per 1 mol of | −2980.06 | – | – | – |
per 1 mol of | −390.828 | – | – | – |
per 1 mol of | −1490.03 | – | – | – |
per 1 mol of | −1402.38 | – | – | – |
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 | −22291.2 | – | – | – |
per 1 mol of | −2786.40 | – | – | – |
per 1 mol of | −227.461 | – | – | – |
per 1 mol of | −696.600 | – | – | – |
per 1 mol of | −2786.40 | – | – | – |
per 1 mol of | −365.430 | – | – | – |
per 1 mol of | −1393.20 | – | – | – |
per 1 mol of | −1311.25 | – | – | – |
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 | −23874.1 | – | – | – |
per 1 mol of | −2984.26 | – | – | – |
per 1 mol of | −243.613 | – | – | – |
per 1 mol of | −746.066 | – | – | – |
per 1 mol of | −2984.26 | – | – | – |
per 1 mol of | −391.379 | – | – | – |
per 1 mol of | −1492.13 | – | – | – |
per 1 mol of | −1404.36 | – | – | – |
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] | – | – | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[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°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 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