NH4F + 2HNO3 🔥→ 3HNO2 + HF↑ + H2↑
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- Reaction of ammonium fluoride and nitric acid
The reaction of ammonium fluoride and nitric acid yields nitrous acid, hydrogen fluoride, 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 ammonium fluoride 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 fluoride and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4F | Ammonium fluoride | 1 | Reducing | Reducing |
| HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HNO2 | Nitrous acid | 3 | Redoxed product | – |
| HF | Hydrogen fluoride | 1 | – | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 155.6 kJ/mol K 0.55 × 10−27 pK 27.26
| 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 | 251.2 | 155.6 | 318.9 | – |
per 1 mol of | 251.2 | 155.6 | 318.9 | – |
per 1 mol of | 125.6 | 77.80 | 159.4 | – |
per 1 mol of | 83.73 | 51.87 | 106.3 | – |
per 1 mol of | 251.2 | 155.6 | 318.9 | – |
| 251.2 | 155.6 | 318.9 | – |
Changes in standard condition (2)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 173.2 kJ/mol K 0.45 × 10−30 pK 30.34
| 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 | 247.0 | 173.2 | 765 | – |
per 1 mol of | 247.0 | 173.2 | 765 | – |
per 1 mol of | 123.5 | 86.60 | 383 | – |
per 1 mol of | 82.33 | 57.73 | 255 | – |
per 1 mol of | 247.0 | 173.2 | 765 | – |
| 247.0 | 173.2 | 765 | – |
Changes in standard condition (3)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 132.0 kJ/mol K 0.75 × 10−23 pK 23.13
| 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 | 202.2 | 132.0 | 233.8 | – |
per 1 mol of | 202.2 | 132.0 | 233.8 | – |
per 1 mol of | 101.1 | 66.00 | 116.9 | – |
per 1 mol of | 67.40 | 44.00 | 77.93 | – |
per 1 mol of | 202.2 | 132.0 | 233.8 | – |
| 202.2 | 132.0 | 233.8 | – |
Changes in standard condition (4)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 149.6 kJ/mol K 0.62 × 10−26 pK 26.21
| 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 | 198.0 | 149.6 | 680 | – |
per 1 mol of | 198.0 | 149.6 | 680 | – |
per 1 mol of | 99.00 | 74.80 | 340 | – |
per 1 mol of | 66.00 | 49.87 | 227 | – |
per 1 mol of | 198.0 | 149.6 | 680 | – |
| 198.0 | 149.6 | 680 | – |
Changes in standard condition (5)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 150.0 kJ/mol K 0.53 × 10−26 pK 26.28
| 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 | 189.6 | 150.0 | 131.3 | – |
per 1 mol of | 189.6 | 150.0 | 131.3 | – |
per 1 mol of | 94.80 | 75.00 | 65.65 | – |
per 1 mol of | 63.20 | 50.00 | 43.77 | – |
per 1 mol of | 189.6 | 150.0 | 131.3 | – |
| 189.6 | 150.0 | 131.3 | – |
Changes in standard condition (6)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 167.6 kJ/mol K 0.43 × 10−29 pK 29.36
| 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 | 185.4 | 167.6 | 578 | – |
per 1 mol of | 185.4 | 167.6 | 578 | – |
per 1 mol of | 92.70 | 83.80 | 289 | – |
per 1 mol of | 61.80 | 55.87 | 193 | – |
per 1 mol of | 185.4 | 167.6 | 578 | – |
| 185.4 | 167.6 | 578 | – |
Changes in standard condition (7)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 132.0 kJ/mol K 0.75 × 10−23 pK 23.13
| 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 | 202.2 | 132.0 | 233.8 | – |
per 1 mol of | 202.2 | 132.0 | 233.8 | – |
per 1 mol of | 101.1 | 66.00 | 116.9 | – |
per 1 mol of | 67.40 | 44.00 | 77.93 | – |
per 1 mol of | 202.2 | 132.0 | 233.8 | – |
| 202.2 | 132.0 | 233.8 | – |
Changes in standard condition (8)
- Reaction of ammonium fluoride and nitric acid◆
ΔrG 149.6 kJ/mol K 0.62 × 10−26 pK 26.21
| 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 | 198.0 | 149.6 | 680 | – |
per 1 mol of | 198.0 | 149.6 | 680 | – |
per 1 mol of | 99.00 | 74.80 | 340 | – |
per 1 mol of | 66.00 | 49.87 | 227 | – |
per 1 mol of | 198.0 | 149.6 | 680 | – |
| 198.0 | 149.6 | 680 | – |
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 |
|---|---|---|---|---|
| NH4F (cr) | -463.96[1] | -348.68[1] | 71.96[1] | 65.27[1] |
| NH4F (ai) | -465.14[1] | -358.09[1] | 99.6[1] | -26.8[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 |
|---|---|---|---|---|
| HNO2 (g) cis | -77.99[1] | -42.94[1] | 248.76[1] | 44.77[1] |
| HNO2 (g) trans | -80.12[1] | -45.24[1] | 249.22[1] | 46.07[1] |
| HNO2 (g) | -79.5[1] | -46.0[1] | 254.1[1] | 45.6[1] |
| HNO2 (ao) | -119.2[1] | -50.6[1] | 135.6[1] | – |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[1] | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid, (ai):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°, -463.96 kJ · mol−1
- ^ ΔfG°, -348.68 kJ · mol−1
- ^ S°, 71.96 J · K−1 · mol−1
- ^ Cp°, 65.27 J · K−1 · mol−1
- ^ ΔfH°, -465.14 kJ · mol−1
- ^ ΔfG°, -358.09 kJ · mol−1
- ^ S°, 99.6 J · K−1 · mol−1
- ^ Cp°, -26.8 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°, -77.99 kJ · mol−1
- ^ ΔfG°, -42.94 kJ · mol−1
- ^ S°, 248.76 J · K−1 · mol−1
- ^ Cp°, 44.77 J · K−1 · mol−1
- ^ ΔfH°, -80.12 kJ · mol−1
- ^ ΔfG°, -45.24 kJ · mol−1
- ^ S°, 249.22 J · K−1 · mol−1
- ^ Cp°, 46.07 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -46.0 kJ · mol−1
- ^ S°, 254.1 J · K−1 · mol−1
- ^ Cp°, 45.6 J · K−1 · mol−1
- ^ ΔfH°, -119.2 kJ · mol−1
- ^ ΔfG°, -50.6 kJ · mol−1
- ^ S°, 135.6 J · K−1 · mol−1
- ^ ΔfH°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 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