KNO2 + H2O 💧⚡→ KNO3 + H2↑
Last updated:
- Electrolysis of aqueous potassium nitrite with water as oxidizing agent
Electrolysis of aqueous potassium nitrite yields potassium nitrate and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous potassium nitrite with water as oxidizing agent
General equation
- Electrolysis of aqueous solution with water as oxidizing agent
- Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous potassium nitrite with water as oxidizing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO2 | Potassium nitrite | 1 | Reducing | Very soluble in water |
| H2O | Water | 1 | Oxidizing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO3 | Potassium nitrate | 1 | Oxidized | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous potassium nitrite with water as oxidizing agent◆
ΔrG 148.82 kJ/mol K 0.85 × 10−26 pK 26.07
| 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 | 161.02 | 148.82 | 41.73 | −57.47 |
per 1 mol of | 161.02 | 148.82 | 41.73 | −57.47 |
per 1 mol of | 161.02 | 148.82 | 41.73 | −57.47 |
per 1 mol of | 161.02 | 148.82 | 41.73 | −57.47 |
| 161.02 | 148.82 | 41.73 | −57.47 |
Changes in aqueous solution (1)
- Electrolysis of aqueous potassium nitrite with water as oxidizing agent◆
ΔrG 158.0 kJ/mol K 0.21 × 10−27 pK 27.68
| 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 | 183.0 | 158.0 | 84.2 | – |
per 1 mol of | 183.0 | 158.0 | 84.2 | – |
per 1 mol of | 183.0 | 158.0 | 84.2 | – |
per 1 mol of | 183.0 | 158.0 | 84.2 | – |
| 183.0 | 158.0 | 84.2 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous potassium nitrite with water as oxidizing agent◆
ΔrG 175.6 kJ/mol K 0.17 × 10−30 pK 30.76
| 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 | 178.8 | 175.6 | 530 | – |
per 1 mol of | 178.8 | 175.6 | 530 | – |
per 1 mol of | 178.8 | 175.6 | 530 | – |
per 1 mol of | 178.8 | 175.6 | 530 | – |
| 178.8 | 175.6 | 530 | – |
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 |
|---|---|---|---|---|
| KNO2 (cr) rhombic | -369.82[1] | -306.55[1] | 152.09[1] | 107.40[1] |
| KNO2 (ai) | -356.9[1] | -315.4[1] | 225.5[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, (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 |
|---|---|---|---|---|
| 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] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -369.82 kJ · mol−1
- ^ ΔfG°, -306.55 kJ · mol−1
- ^ S°, 152.09 J · K−1 · mol−1
- ^ Cp°, 107.40 J · K−1 · mol−1
- ^ ΔfH°, -356.9 kJ · mol−1
- ^ ΔfG°, -315.4 kJ · mol−1
- ^ S°, 225.5 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
- ^ 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°, 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