12Na4[Fe(CN)6] + 16HNO3 → 11Na3[Fe(CN)6] + 11NaNO3 + 2Na2CO3 + Fe(NO3)3 + 4NH4CN
Last updated:
The reaction of sodium hexacyanidoferrate(II) and nitric acid yields sodium hexacyanidoferrate(III), sodium nitrate, sodium carbonate, iron(III) nitrate, and ammonium cyanide (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) | 12 | Reducing | Reducing |
| HNO3 | Nitric acid | 16 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na3[Fe(CN)6] | Sodium hexacyanidoferrate(III) | 11 | Redoxed product | – |
| NaNO3 | Sodium nitrate | 11 | – | – |
| Na2CO3 | Sodium carbonate | 2 | Oxidized | – |
| Fe(NO3)3 | Iron(III) nitrate | 1 | Oxidized | – |
| NH4CN | Ammonium cyanide | 4 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid◆
ΔrG −784.3 kJ/mol K 2.53 × 10137 pK −137.40 - 12Na4[Fe(CN)6]Ionized aqueous solution + 16HNO3Ionized aqueous solution11Na3[Fe(CN)6]Ionized aqueous solution + 11NaNO3Ionized aqueous solution + 2Na2CO3Ionized aqueous solution + Fe(NO3)3Ionized aqueous solution + 4NH4CNIonized 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 | −202.6 | −784.3 | 1940.9 | – |
per 1 mol of | −16.88 | −65.36 | 161.74 | – |
per 1 mol of | −12.66 | −49.02 | 121.31 | – |
per 1 mol of | −18.42 | −71.30 | 176.45 | – |
per 1 mol of | −18.42 | −71.30 | 176.45 | – |
per 1 mol of | −101.3 | −392.1 | 970.45 | – |
per 1 mol of | −202.6 | −784.3 | 1940.9 | – |
per 1 mol of | −50.65 | −196.1 | 485.23 | – |
Changes in aqueous solution (2)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 12Na4[Fe(CN)6]Ionized aqueous solution + 16HNO3Ionized aqueous solution11Na3[Fe(CN)6]Ionized aqueous solution + 11NaNO3Ionized aqueous solution + 2Na2CO3Ionized aqueous solution + Fe(NO3)3Ionized aqueous solution + 4NH4CNAqueous 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 | −145.8 | – | – | – |
per 1 mol of | −12.15 | – | – | – |
per 1 mol of | −9.113 | – | – | – |
per 1 mol of | −13.25 | – | – | – |
per 1 mol of | −13.25 | – | – | – |
per 1 mol of | −72.90 | – | – | – |
per 1 mol of | −145.8 | – | – | – |
per 1 mol of | −36.45 | – | – | – |
Changes in aqueous solution (3)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 12Na4[Fe(CN)6]Ionized aqueous solution + 16HNO3Ionized aqueous solution11Na3[Fe(CN)6]Ionized aqueous solution + 11NaNO3Ionized aqueous solution + 2Na2CO3Ionized aqueous solution + Fe(NO3)3Aqueous solution + 4NH4CNIonized 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 | −206.8 | – | – | – |
per 1 mol of | −17.23 | – | – | – |
per 1 mol of | −12.93 | – | – | – |
per 1 mol of | −18.80 | – | – | – |
per 1 mol of | −18.80 | – | – | – |
per 1 mol of | −103.4 | – | – | – |
per 1 mol of | −206.8 | – | – | – |
per 1 mol of | −51.70 | – | – | – |
Changes in aqueous solution (4)
- Reaction of sodium hexacyanidoferrate(II) and nitric acid
- 12Na4[Fe(CN)6]Ionized aqueous solution + 16HNO3Ionized aqueous solution11Na3[Fe(CN)6]Ionized aqueous solution + 11NaNO3Ionized aqueous solution + 2Na2CO3Ionized aqueous solution + Fe(NO3)3Aqueous solution + 4NH4CNAqueous 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 | −150.0 | – | – | – |
per 1 mol of | −12.50 | – | – | – |
per 1 mol of | −9.375 | – | – | – |
per 1 mol of | −13.64 | – | – | – |
per 1 mol of | −13.64 | – | – | – |
per 1 mol of | −75.00 | – | – | – |
per 1 mol of | −150.0 | – | – | – |
per 1 mol of | −37.50 | – | – | – |
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 |
|---|---|---|---|---|
| Na3[Fe(CN)6] (ai) | -158.6[1] | -56.4[1] | 447.3[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] |
| Na2CO3 (cr) | -1130.68[1] | -1044.44[1] | 134.98[1] | 112.30[1] |
| Na2CO3 (ai) | -1157.38[1] | -1051.64[1] | 61.1[1] | – |
| Na2CO3 (cr) 1 hydrate | -1431.26[1] | -1285.31[1] | 168.11[1] | 145.60[1] |
| Na2CO3 (cr) 7 hydrate | -3199.96[1] | -2714.2[1] | 422.2[1] | – |
| Na2CO3 (cr) 10 hydrate | -4081.32[1] | -3427.66[1] | 562.7[1] | 550.32[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] | – | – | – |
| NH4CN (cr) | 0.42[1] | – | – | 134[1] |
| NH4CN (ai) | 18.0[1] | 93.0[1] | 207.5[1] | – |
| NH4CN (aq) | 32.2[1] | – | – | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (aq):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°, -158.6 kJ · mol−1
- ^ ΔfG°, -56.4 kJ · mol−1
- ^ S°, 447.3 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°, -1130.68 kJ · mol−1
- ^ ΔfG°, -1044.44 kJ · mol−1
- ^ S°, 134.98 J · K−1 · mol−1
- ^ Cp°, 112.30 J · K−1 · mol−1
- ^ ΔfH°, -1157.38 kJ · mol−1
- ^ ΔfG°, -1051.64 kJ · mol−1
- ^ S°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -1431.26 kJ · mol−1
- ^ ΔfG°, -1285.31 kJ · mol−1
- ^ S°, 168.11 J · K−1 · mol−1
- ^ Cp°, 145.60 J · K−1 · mol−1
- ^ ΔfH°, -3199.96 kJ · mol−1
- ^ ΔfG°, -2714.2 kJ · mol−1
- ^ S°, 422.2 J · K−1 · mol−1
- ^ ΔfH°, -4081.32 kJ · mol−1
- ^ ΔfG°, -3427.66 kJ · mol−1
- ^ S°, 562.7 J · K−1 · mol−1
- ^ Cp°, 550.32 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°, 0.42 kJ · mol−1
- ^ Cp°, 134. J · K−1 · mol−1
- ^ ΔfH°, 18.0 kJ · mol−1
- ^ ΔfG°, 93.0 kJ · mol−1
- ^ S°, 207.5 J · K−1 · mol−1
- ^ ΔfH°, 32.2 kJ · mol−1