2KCl + 4HNO3 🔥→ 2KNO3 + Cl2↑ + 2NO2↑ + 2H2O
Last updated:
- Reaction of potassium chloride and nitric acid
- 2KClPotassium chloride + 4HNO3Nitric acid2KNO3Potassium nitrate + ↑ + 2NO2↑Nitrogen dioxide + 2H2OWater🔥⟶
The reaction of potassium chloride and nitric acid yields potassium nitrate, , nitrogen dioxide, and water (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 potassium chloride and nitric acid
- 2KClPotassium chloride + 4HNO3Nitric acid2KNO3Potassium nitrate + ↑ + 2NO2↑Nitrogen dioxide + 2H2OWater🔥⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium chloride and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KCl | Potassium chloride | 2 | Reducing | Hardly oxidizable |
| HNO3 | Nitric acid | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO3 | Potassium nitrate | 2 | – | – |
| 1 | Oxidized | – | ||
| NO2 | Nitrogen dioxide | 2 | Reduced | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium chloride and nitric acid◆
ΔrG −20.24 kJ/mol K 3.51 × 103 pK −3.55
| 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 | 75.33 | −20.24 | 321.53 | −90.39 |
per 1 mol of | 37.66 | −10.12 | 160.76 | −45.20 |
per 1 mol of | 18.83 | −5.060 | 80.382 | −22.60 |
per 1 mol of | 37.66 | −10.12 | 160.76 | −45.20 |
| 75.33 | −20.24 | 321.53 | −90.39 | |
per 1 mol of | 37.66 | −10.12 | 160.76 | −45.20 |
per 1 mol of | 37.66 | −10.12 | 160.76 | −45.20 |
Changes in aqueous solution (1)
- Reaction of potassium chloride and nitric acid◆
ΔrG 113.28 kJ/mol K 0.14 × 10−19 pK 19.85
| 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 | 243.72 | 113.28 | 437.2 | 704.7 |
per 1 mol of | 121.86 | 56.640 | 218.6 | 352.4 |
per 1 mol of | 60.930 | 28.320 | 109.3 | 176.2 |
per 1 mol of | 121.86 | 56.640 | 218.6 | 352.4 |
| 243.72 | 113.28 | 437.2 | 704.7 | |
per 1 mol of | 121.86 | 56.640 | 218.6 | 352.4 |
per 1 mol of | 121.86 | 56.640 | 218.6 | 352.4 |
Changes in aqueous solution (2)
- Reaction of potassium chloride and nitric acid◆
ΔrG 120.22 kJ/mol K 0.87 × 10−21 pK 21.06
| 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 | 220.3 | 120.22 | 335 | – |
per 1 mol of | 110.2 | 60.110 | 168 | – |
per 1 mol of | 55.08 | 30.055 | 83.8 | – |
per 1 mol of | 110.2 | 60.110 | 168 | – |
| 220.3 | 120.22 | 335 | – | |
per 1 mol of | 110.2 | 60.110 | 168 | – |
per 1 mol of | 110.2 | 60.110 | 168 | – |
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 |
|---|---|---|---|---|
| KCl (cr) | -436.747[1] | -409.14[1] | 82.59[1] | 51.30[1] |
| KCl (g) | -214.14[1] | -233.0[1] | 239.10[1] | 36.48[1] |
| KCl (ai) | -419.53[1] | -414.49[1] | 159.0[1] | -114.6[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| KNO3 (cr) | -494.63[1] | -394.86[1] | 133.05[1] | 96.40[1] |
| KNO3 (ai) | -459.74[1] | -394.53[1] | 248.9[1] | -64.9[1] |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[1] |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -436.747 kJ · mol−1
- ^ ΔfG°, -409.14 kJ · mol−1
- ^ S°, 82.59 J · K−1 · mol−1
- ^ Cp°, 51.30 J · K−1 · mol−1
- ^ ΔfH°, -214.14 kJ · mol−1
- ^ ΔfG°, -233.0 kJ · mol−1
- ^ S°, 239.10 J · K−1 · mol−1
- ^ Cp°, 36.48 J · K−1 · mol−1
- ^ ΔfH°, -419.53 kJ · mol−1
- ^ ΔfG°, -414.49 kJ · mol−1
- ^ S°, 159.0 J · K−1 · mol−1
- ^ Cp°, -114.6 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°, -494.63 kJ · mol−1
- ^ ΔfG°, -394.86 kJ · mol−1
- ^ S°, 133.05 J · K−1 · mol−1
- ^ Cp°, 96.40 J · K−1 · mol−1
- ^ ΔfH°, -459.74 kJ · mol−1
- ^ ΔfG°, -394.53 kJ · mol−1
- ^ S°, 248.9 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, 33.18 kJ · mol−1
- ^ ΔfG°, 51.31 kJ · mol−1
- ^ S°, 240.06 J · K−1 · mol−1
- ^ Cp°, 37.20 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1