Na3[Fe(CN)6] + 21HNO3 → 3NaHCO3 + Fe(NO3)3 + 3NH4NO3 + 9N2O3↑ + 3H2CO3
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The reaction of sodium hexacyanidoferrate(III) and nitric acid yields sodium hydrogencarbonate, iron(III) nitrate, ammonium nitrate, dinitrogen trioxide, and carbonic acid (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 | 21 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHCO3 | Sodium hydrogencarbonate | 3 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 1 | – | – |
| NH4NO3 | Ammonium nitrate | 3 | – | – |
| N2O3 | Dinitrogen trioxide | 9 | Redoxed product | – |
| H2CO3 | Carbonic acid | 3 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1677.4 kJ/mol K 7.38 × 10293 pK −293.87
| 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 | −1319.0 | −1677.4 | 1204.4 | – |
per 1 mol of | −1319.0 | −1677.4 | 1204.4 | – |
per 1 mol of | −62.810 | −79.876 | 57.352 | – |
per 1 mol of | −439.67 | −559.13 | 401.47 | – |
per 1 mol of | −1319.0 | −1677.4 | 1204.4 | – |
per 1 mol of | −439.67 | −559.13 | 401.47 | – |
per 1 mol of | −146.56 | −186.38 | 133.82 | – |
per 1 mol of | −439.67 | −559.13 | 401.47 | – |
Changes in aqueous solution (2)
- 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 | −1323.2 | – | – | – |
per 1 mol of | −1323.2 | – | – | – |
per 1 mol of | −63.010 | – | – | – |
per 1 mol of | −441.07 | – | – | – |
per 1 mol of | −1323.2 | – | – | – |
per 1 mol of | −441.07 | – | – | – |
per 1 mol of | −147.02 | – | – | – |
per 1 mol of | −441.07 | – | – | – |
Changes in aqueous solution (3)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −1680.5 kJ/mol K 2.58 × 10294 pK −294.41
| 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 | −1354.3 | −1680.5 | 1095.2 | – |
per 1 mol of | −1354.3 | −1680.5 | 1095.2 | – |
per 1 mol of | −64.490 | −80.024 | 52.152 | – |
per 1 mol of | −451.43 | −560.17 | 365.07 | – |
per 1 mol of | −1354.3 | −1680.5 | 1095.2 | – |
per 1 mol of | −451.43 | −560.17 | 365.07 | – |
per 1 mol of | −150.48 | −186.72 | 121.69 | – |
per 1 mol of | −451.43 | −560.17 | 365.07 | – |
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 | −1358.5 | – | – | – |
per 1 mol of | −1358.5 | – | – | – |
per 1 mol of | −64.690 | – | – | – |
per 1 mol of | −452.83 | – | – | – |
per 1 mol of | −1358.5 | – | – | – |
per 1 mol of | −452.83 | – | – | – |
per 1 mol of | −150.94 | – | – | – |
per 1 mol of | −452.83 | – | – | – |
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] | – | – | – |
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
| N2O3 (l) | 50.29[1] | – | – | – |
| N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[1] |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):Aqueous solution, (l):Liquid, (g):Gas
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°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 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°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1