Mn(NO3)2 + H2O 💧⚡→ Mn(OH)2 + 2NO↑ + O3↑
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- Electrolysis of aqueous manganese(II) nitrate with water as non-redox agent
Electrolysis of aqueous manganese(II) nitrate yields manganese(II) hydroxide, nitrogen monoxide, 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 manganese(II) nitrate with water as non-redox agent
General equation
- Electrolysis of aqueous solution with water as non redox agent
- Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous manganese(II) nitrate with water as non-redox agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(NO3)2 | Manganese(II) nitrate | 1 | Self redox agent | Very soluble in water |
| H2O | Water | 1 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(OH)2 | Manganese(II) hydroxide | 1 | – | – |
| NO | Nitrogen monoxide | 2 | Reduced | – |
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Electrolysis of aqueous manganese(II) nitrate with water as non-redox agent
| 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 | 489.9 | – | – | – |
per 1 mol of | 489.9 | – | – | – |
per 1 mol of | 489.9 | – | – | – |
per 1 mol of | 489.9 | – | – | – |
per 1 mol of | 244.9 | – | – | – |
| 489.9 | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous manganese(II) nitrate with water as non-redox agent◆
ΔrG 409.3 kJ/mol K 0.20 × 10−71 pK 71.71
| 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 | 549.1 | 409.3 | 472 | – |
per 1 mol of | 549.1 | 409.3 | 472 | – |
per 1 mol of | 549.1 | 409.3 | 472 | – |
per 1 mol of | 549.1 | 409.3 | 472 | – |
per 1 mol of | 274.6 | 204.7 | 236 | – |
| 549.1 | 409.3 | 472 | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous manganese(II) nitrate with water as non-redox agent◆
ΔrG 420.2 kJ/mol K 0.24 × 10−73 pK 73.62
| 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 | 532.3 | 420.2 | 379 | – |
per 1 mol of | 532.3 | 420.2 | 379 | – |
per 1 mol of | 532.3 | 420.2 | 379 | – |
per 1 mol of | 532.3 | 420.2 | 379 | – |
per 1 mol of | 266.1 | 210.1 | 190 | – |
| 532.3 | 420.2 | 379 | – |
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 |
|---|---|---|---|---|
| Mn(NO3)2 (cr) | -576.26[1] | – | – | – |
| Mn(NO3)2 (ai) | -635.5[1] | -450.9[1] | 218[1] | -121[1] |
| Mn(NO3)2 (vit) 6 hydrate | -2371.9[1] | – | – | – |
| Mn(NO3)2 (l) 6 hydrate | -2331.62[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, (vit):Vitreous liquid, (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 |
|---|---|---|---|---|
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[1] | – |
* (am):Amorphous solid, (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°, -576.26 kJ · mol−1
- ^ ΔfH°, -635.5 kJ · mol−1
- ^ ΔfG°, -450.9 kJ · mol−1
- ^ S°, 218. J · K−1 · mol−1
- ^ Cp°, -121. J · K−1 · mol−1
- ^ ΔfH°, -2371.9 kJ · mol−1
- ^ ΔfH°, -2331.62 kJ · 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°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1