2Na4[Fe(CN)6] + 14HNO3 🔥→ 8NaNO3 + 2Fe(NO3)3 + 12HCN + H2↑
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The reaction of sodium hexacyanidoferrate(II) and nitric acid yields sodium nitrate, iron(III) nitrate, hydrogen cyanide, and (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) | 2 | Reducing | Reducing |
| HNO3 | Nitric acid | 14 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO3 | Sodium nitrate | 8 | – | – |
| Fe(NO3)3 | Iron(III) nitrate | 2 | Oxidized | – |
| HCN | Hydrogen cyanide | 12 | – | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG 37.2 kJ/mol K 0.30 × 10−6 pK 6.52 - 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 12HCNUn-ionized aqueous solution + ↑Gas🔥⟶
| 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 | 277.0 | 37.2 | 805.5 | – |
per 1 mol of | 138.5 | 18.6 | 402.8 | – |
per 1 mol of | 19.79 | 2.66 | 57.54 | – |
per 1 mol of | 34.63 | 4.65 | 100.7 | – |
per 1 mol of | 138.5 | 18.6 | 402.8 | – |
per 1 mol of | 23.08 | 3.10 | 67.13 | – |
| 277.0 | 37.2 | 805.5 | – |
Changes in aqueous solution (2)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG 54.8 kJ/mol K 0.25 × 10−9 pK 9.60 - 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 12HCNUn-ionized aqueous solution + ↑Un-ionized aqueous solution🔥⟶
| 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 | 272.8 | 54.8 | 1252 | – |
per 1 mol of | 136.4 | 27.4 | 626.0 | – |
per 1 mol of | 19.49 | 3.91 | 89.43 | – |
per 1 mol of | 34.10 | 6.85 | 156.5 | – |
per 1 mol of | 136.4 | 27.4 | 626.0 | – |
per 1 mol of | 22.73 | 4.57 | 104.3 | – |
| 272.8 | 54.8 | 1252 | – |
Changes in aqueous solution (3)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 12HCNUn-ionized aqueous solution + ↑Gas🔥⟶
| 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 | 268.6 | – | – | – |
per 1 mol of | 134.3 | – | – | – |
per 1 mol of | 19.19 | – | – | – |
per 1 mol of | 33.58 | – | – | – |
per 1 mol of | 134.3 | – | – | – |
per 1 mol of | 22.38 | – | – | – |
| 268.6 | – | – | – |
Changes in aqueous solution (4)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 12HCNUn-ionized aqueous solution + ↑Un-ionized aqueous solution🔥⟶
| 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 | 264.4 | – | – | – |
per 1 mol of | 132.2 | – | – | – |
per 1 mol of | 18.89 | – | – | – |
per 1 mol of | 33.05 | – | – | – |
per 1 mol of | 132.2 | – | – | – |
per 1 mol of | 22.03 | – | – | – |
| 264.4 | – | – | – |
Changes in aqueous solution (5)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG 669.6 kJ/mol K 0.49 × 10−117 pK 117.31 - 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 12HCNIonized aqueous solution + ↑Gas🔥⟶
| 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 | 799.0 | 669.6 | 438.3 | – |
per 1 mol of | 399.5 | 334.8 | 219.2 | – |
per 1 mol of | 57.07 | 47.83 | 31.31 | – |
per 1 mol of | 99.88 | 83.70 | 54.79 | – |
per 1 mol of | 399.5 | 334.8 | 219.2 | – |
per 1 mol of | 66.58 | 55.80 | 36.52 | – |
| 799.0 | 669.6 | 438.3 | – |
Changes in aqueous solution (6)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG 687.2 kJ/mol K 0.41 × 10−120 pK 120.39 - 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 12HCNIonized aqueous solution + ↑Un-ionized aqueous solution🔥⟶
| 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 | 794.8 | 687.2 | 885 | – |
per 1 mol of | 397.4 | 343.6 | 443 | – |
per 1 mol of | 56.77 | 49.09 | 63.2 | – |
per 1 mol of | 99.35 | 85.90 | 111 | – |
per 1 mol of | 397.4 | 343.6 | 443 | – |
per 1 mol of | 66.23 | 57.27 | 73.8 | – |
| 794.8 | 687.2 | 885 | – |
Changes in aqueous solution (7)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 12HCNIonized aqueous solution + ↑Gas🔥⟶
| 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 | 790.6 | – | – | – |
per 1 mol of | 395.3 | – | – | – |
per 1 mol of | 56.47 | – | – | – |
per 1 mol of | 98.83 | – | – | – |
per 1 mol of | 395.3 | – | – | – |
per 1 mol of | 65.88 | – | – | – |
| 790.6 | – | – | – |
Changes in aqueous solution (8)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 2Na4[Fe(CN)6]Ionized aqueous solution + 14HNO3Ionized aqueous solution8NaNO3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 12HCNIonized aqueous solution + ↑Un-ionized aqueous solution🔥⟶
| 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 | 786.4 | – | – | – |
per 1 mol of | 393.2 | – | – | – |
per 1 mol of | 56.17 | – | – | – |
per 1 mol of | 98.30 | – | – | – |
per 1 mol of | 393.2 | – | – | – |
per 1 mol of | 65.53 | – | – | – |
| 786.4 | – | – | – |
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 |
|---|---|---|---|---|
| NaNO3 (cr) | -467.85[1] | -367.00[1] | 116.52[1] | 92.88[1] |
| NaNO3 (ai) | -447.48[1] | -373.15[1] | 205.4[1] | -40.2[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] | – | – | – |
| HCN (l) | 108.87[1] | 124.97[1] | 112.84[1] | 70.63[1] |
| HCN (g) | 135.1[1] | 124.7[1] | 201.78[1] | 35.86[1] |
| HCN (ai) | 150.6[1] | 172.4[1] | 94.1[1] | – |
| HCN (ao) | 107.1[1] | 119.7[1] | 124.7[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution
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°, -467.85 kJ · mol−1
- ^ ΔfG°, -367.00 kJ · mol−1
- ^ S°, 116.52 J · K−1 · mol−1
- ^ Cp°, 92.88 J · K−1 · mol−1
- ^ ΔfH°, -447.48 kJ · mol−1
- ^ ΔfG°, -373.15 kJ · mol−1
- ^ S°, 205.4 J · K−1 · mol−1
- ^ Cp°, -40.2 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°, 108.87 kJ · mol−1
- ^ ΔfG°, 124.97 kJ · mol−1
- ^ S°, 112.84 J · K−1 · mol−1
- ^ Cp°, 70.63 J · K−1 · mol−1
- ^ ΔfH°, 135.1 kJ · mol−1
- ^ ΔfG°, 124.7 kJ · mol−1
- ^ S°, 201.78 J · K−1 · mol−1
- ^ Cp°, 35.86 J · K−1 · mol−1
- ^ ΔfH°, 150.6 kJ · mol−1
- ^ ΔfG°, 172.4 kJ · mol−1
- ^ S°, 94.1 J · K−1 · mol−1
- ^ ΔfH°, 107.1 kJ · mol−1
- ^ ΔfG°, 119.7 kJ · mol−1
- ^ S°, 124.7 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1