7Na3[Fe(CN)6] + 99HNO3 → 21NaHCO3 + 7Fe(NO3)3 + 108NO↑ + 12NH4HCO3 + 9H2CO3
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The reaction of sodium hexacyanidoferrate(III) and nitric acid yields sodium hydrogencarbonate, iron(III) nitrate, nitrogen monoxide, ammonium hydrogencarbonate, 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) | 7 | Reducing | Reducing |
| HNO3 | Nitric acid | 99 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHCO3 | Sodium hydrogencarbonate | 21 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 7 | Oxidized | – |
| NO | Nitrogen monoxide | 108 | Redoxed product | – |
| NH4HCO3 | Ammonium hydrogencarbonate | 12 | Oxidized | – |
| H2CO3 | Carbonic acid | 9 | Oxidized | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −13034.6 kJ/mol K 3.66 × 102283 pK −2283.56
| 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 | −9074.2 | −13034.6 | 13297.3 | – |
per 1 mol of | −1296.3 | −1862.09 | 1899.61 | – |
per 1 mol of | −91.659 | −131.663 | 134.316 | – |
per 1 mol of | −432.10 | −620.695 | 633.205 | – |
per 1 mol of | −1296.3 | −1862.09 | 1899.61 | – |
per 1 mol of | −84.020 | −120.691 | 123.123 | – |
per 1 mol of | −756.18 | −1086.22 | 1108.11 | – |
per 1 mol of | −1008.2 | −1448.29 | 1477.48 | – |
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 | −9040.6 | – | – | – |
per 1 mol of | −1291.5 | – | – | – |
per 1 mol of | −91.319 | – | – | – |
per 1 mol of | −430.50 | – | – | – |
per 1 mol of | −1291.5 | – | – | – |
per 1 mol of | −83.709 | – | – | – |
per 1 mol of | −753.38 | – | – | – |
per 1 mol of | −1004.5 | – | – | – |
Changes in aqueous solution (3)
- 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 | −9103.6 | – | – | – |
per 1 mol of | −1300.5 | – | – | – |
per 1 mol of | −91.956 | – | – | – |
per 1 mol of | −433.50 | – | – | – |
per 1 mol of | −1300.5 | – | – | – |
per 1 mol of | −84.293 | – | – | – |
per 1 mol of | −758.63 | – | – | – |
per 1 mol of | −1011.5 | – | – | – |
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 | −9070.0 | – | – | – |
per 1 mol of | −1295.7 | – | – | – |
per 1 mol of | −91.616 | – | – | – |
per 1 mol of | −431.90 | – | – | – |
per 1 mol of | −1295.7 | – | – | – |
per 1 mol of | −83.981 | – | – | – |
per 1 mol of | −755.83 | – | – | – |
per 1 mol of | −1007.8 | – | – | – |
Changes in aqueous solution (5)
- Reaction of sodium hexacyanidoferrate(III) and nitric acid◆
ΔrG −13056.4 kJ/mol K 2.41 × 102287 pK −2287.38
| 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 | −9321.8 | −13056.4 | 12532.9 | – |
per 1 mol of | −1331.7 | −1865.20 | 1790.41 | – |
per 1 mol of | −94.160 | −131.883 | 126.595 | – |
per 1 mol of | −443.90 | −621.733 | 596.805 | – |
per 1 mol of | −1331.7 | −1865.20 | 1790.41 | – |
per 1 mol of | −86.313 | −120.893 | 116.045 | – |
per 1 mol of | −776.82 | −1088.03 | 1044.41 | – |
per 1 mol of | −1035.8 | −1450.71 | 1392.54 | – |
Changes in aqueous solution (6)
- 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 | −9288.2 | – | – | – |
per 1 mol of | −1326.9 | – | – | – |
per 1 mol of | −93.820 | – | – | – |
per 1 mol of | −442.30 | – | – | – |
per 1 mol of | −1326.9 | – | – | – |
per 1 mol of | −86.002 | – | – | – |
per 1 mol of | −774.02 | – | – | – |
per 1 mol of | −1032.0 | – | – | – |
Changes in aqueous solution (7)
- 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 | −9351.2 | – | – | – |
per 1 mol of | −1335.9 | – | – | – |
per 1 mol of | −94.457 | – | – | – |
per 1 mol of | −445.30 | – | – | – |
per 1 mol of | −1335.9 | – | – | – |
per 1 mol of | −86.585 | – | – | – |
per 1 mol of | −779.27 | – | – | – |
per 1 mol of | −1039.0 | – | – | – |
Changes in aqueous solution (8)
- 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 | −9317.6 | – | – | – |
per 1 mol of | −1331.1 | – | – | – |
per 1 mol of | −94.117 | – | – | – |
per 1 mol of | −443.70 | – | – | – |
per 1 mol of | −1331.1 | – | – | – |
per 1 mol of | −86.274 | – | – | – |
per 1 mol of | −776.47 | – | – | – |
per 1 mol of | −1035.3 | – | – | – |
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] | – | – | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| NH4HCO3 (cr) | -849.4[1] | -665.9[1] | 120.9[1] | – |
| NH4HCO3 (ai) | -824.50[1] | -666.07[1] | 204.6[1] | – |
| NH4HCO3 (aq) | -821.7[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, (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°, 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°, -849.4 kJ · mol−1
- ^ ΔfG°, -665.9 kJ · mol−1
- ^ S°, 120.9 J · K−1 · mol−1
- ^ ΔfH°, -824.50 kJ · mol−1
- ^ ΔfG°, -666.07 kJ · mol−1
- ^ S°, 204.6 J · K−1 · mol−1
- ^ ΔfH°, -821.7 kJ · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1