8CH3COONH4 + 7HNO3 → 12NH4HCO3 + 3HCN + CO↑
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The reaction of ammonium acetate and nitric acid yields ammonium hydrogencarbonate, hydrogen cyanide, and carbon monoxide (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 ammonium acetate 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 ammonium acetate and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COONH4 | Ammonium acetate | 8 | Reducing | Reducing |
| HNO3 | Nitric acid | 7 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4HCO3 | Ammonium hydrogencarbonate | 12 | Redoxed product | – |
| HCN | Hydrogen cyanide | 3 | Redoxed product | – |
| CO | Carbon monoxide | 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium acetate 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 | −3828.9 | – | – | – |
per 1 mol of | −478.61 | – | – | – |
per 1 mol of | −546.99 | – | – | – |
per 1 mol of | −319.07 | – | – | – |
per 1 mol of | −1276.3 | – | – | – |
per 1 mol of | −3828.9 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium acetate and nitric acid◆
ΔrG −3403.3 kJ/mol K 1.71 × 10596 pK −596.23
| 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 | −3283.5 | −3403.3 | 402.2 | – |
per 1 mol of | −410.44 | −425.41 | 50.27 | – |
per 1 mol of | −469.07 | −486.19 | 57.46 | – |
per 1 mol of | −273.63 | −283.61 | 33.52 | – |
per 1 mol of | −1094.5 | −1134.4 | 134.1 | – |
per 1 mol of | −3283.5 | −3403.3 | 402.2 | – |
Changes in aqueous solution (2)
- Reaction of ammonium acetate and nitric acid◆
ΔrG −3386.0 kJ/mol K 1.59 × 10593 pK −593.20
| 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 | −3294.0 | −3386.0 | 309.1 | – |
per 1 mol of | −411.75 | −423.25 | 38.64 | – |
per 1 mol of | −470.57 | −483.71 | 44.16 | – |
per 1 mol of | −274.50 | −282.17 | 25.76 | – |
per 1 mol of | −1098.0 | −1128.7 | 103.0 | – |
per 1 mol of | −3294.0 | −3386.0 | 309.1 | – |
Changes in aqueous solution (3)
- Reaction of ammonium acetate 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 | −3249.9 | – | – | – |
per 1 mol of | −406.24 | – | – | – |
per 1 mol of | −464.27 | – | – | – |
per 1 mol of | −270.82 | – | – | – |
per 1 mol of | −1083.3 | – | – | – |
per 1 mol of | −3249.9 | – | – | – |
Changes in aqueous solution (4)
- Reaction of ammonium acetate 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 | −3260.4 | – | – | – |
per 1 mol of | −407.55 | – | – | – |
per 1 mol of | −465.77 | – | – | – |
per 1 mol of | −271.70 | – | – | – |
per 1 mol of | −1086.8 | – | – | – |
per 1 mol of | −3260.4 | – | – | – |
Changes in aqueous solution (5)
- Reaction of ammonium acetate and nitric acid◆
ΔrG −3245.2 kJ/mol K 3.42 × 10568 pK −568.53
| 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 | −3153.0 | −3245.2 | 310.4 | – |
per 1 mol of | −394.13 | −405.65 | 38.80 | – |
per 1 mol of | −450.43 | −463.60 | 44.34 | – |
per 1 mol of | −262.75 | −270.43 | 25.87 | – |
per 1 mol of | −1051.0 | −1081.7 | 103.5 | – |
per 1 mol of | −3153.0 | −3245.2 | 310.4 | – |
Changes in aqueous solution (6)
- Reaction of ammonium acetate and nitric acid◆
ΔrG −3227.9 kJ/mol K 3.19 × 10565 pK −565.50
| 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 | −3163.5 | −3227.9 | 217.3 | – |
per 1 mol of | −395.44 | −403.49 | 27.16 | – |
per 1 mol of | −451.93 | −461.13 | 31.04 | – |
per 1 mol of | −263.63 | −268.99 | 18.11 | – |
per 1 mol of | −1054.5 | −1076.0 | 72.43 | – |
per 1 mol of | −3163.5 | −3227.9 | 217.3 | – |
Changes in aqueous solution (7)
- Reaction of ammonium acetate 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 | −3119.4 | – | – | – |
per 1 mol of | −389.93 | – | – | – |
per 1 mol of | −445.63 | – | – | – |
per 1 mol of | −259.95 | – | – | – |
per 1 mol of | −1039.8 | – | – | – |
per 1 mol of | −3119.4 | – | – | – |
Changes in aqueous solution (8)
- Reaction of ammonium acetate 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 | −3129.9 | – | – | – |
per 1 mol of | −391.24 | – | – | – |
per 1 mol of | −447.13 | – | – | – |
per 1 mol of | −260.82 | – | – | – |
per 1 mol of | −1043.3 | – | – | – |
per 1 mol of | −3129.9 | – | – | – |
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 |
|---|---|---|---|---|
| CH3COONH4 (cr) | -616.14[1] | – | – | – |
| CH3COONH4 (ai) | -618.52[1] | -448.61[1] | 200.0[1] | 73.6[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] |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| 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] | – | – | – |
| 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] | – |
| CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
| CO (ao) | -120.96[1] | -119.90[1] | 104.6[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°, -616.14 kJ · mol−1
- ^ ΔfH°, -618.52 kJ · mol−1
- ^ ΔfG°, -448.61 kJ · mol−1
- ^ S°, 200.0 J · K−1 · mol−1
- ^ Cp°, 73.6 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°, -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°, 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°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 J · K−1 · mol−1