7Cu + Mn(NO3)2 + 3H2O → 7CuO + N2H4 + Mn(OH)2
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- Reaction of and manganese(II) nitrate under neutral condition
The reaction of , manganese(II) nitrate, and water yields copper(II) oxide, hydrazine, and manganese(II) hydroxide (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 and manganese(II) nitrate under neutral condition
General equation
- Reaction of oxidizable species and oxidizing species under neutral condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and manganese(II) nitrate under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 7 | Reducing | Oxidizable | ||
| Mn(NO3)2 | Manganese(II) nitrate | 1 | Oxidizing | Oxidizing |
| H2O | Water | 3 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuO | Copper(II) oxide | 7 | Oxidized | – |
| N2H4 | Hydrazine | 1 | Reduced | – |
| Mn(OH)2 | Manganese(II) hydroxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and manganese(II) nitrate under neutral condition
| 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 | −312.1 | – | – | – |
| −44.59 | – | – | – | |
per 1 mol of | −312.1 | – | – | – |
per 1 mol of | −104.0 | – | – | – |
per 1 mol of | −44.59 | – | – | – |
per 1 mol of | −312.1 | – | – | – |
per 1 mol of | −312.1 | – | – | – |
Changes in aqueous solution
- Reaction of and manganese(II) nitrate under neutral condition◆
ΔrG −232.5 kJ/mol K 5.40 × 1040 pK −40.73
| 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 | −269.2 | −232.5 | −124 | – |
| −38.46 | −33.21 | −17.7 | – | |
per 1 mol of | −269.2 | −232.5 | −124 | – |
per 1 mol of | −89.73 | −77.50 | −41.3 | – |
per 1 mol of | −38.46 | −33.21 | −17.7 | – |
per 1 mol of | −269.2 | −232.5 | −124 | – |
per 1 mol of | −269.2 | −232.5 | −124 | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 33.150[1] | 24.435[1] |
| (g) | 338.32[1] | 298.58[1] | 166.38[1] | 20.786[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, (g):Gas, (ai):Ionized aqueous solution, (vit):Vitreous liquid, (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 |
|---|---|---|---|---|
| CuO (cr) | -157.3[1] | -129.7[1] | 42.63[1] | 42.30[1] |
| N2H4 (l) | 50.63[1] | 149.34[1] | 121.21[1] | 98.87[1] |
| N2H4 (g) | 95.40[1] | 159.35[1] | 238.47[1] | 49.58[1] |
| N2H4 (ao) | 34.31[1] | 128.1[1] | 138[1] | – |
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (am):Amorphous solid
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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 33.150 J · K−1 · mol−1
- ^ Cp°, 24.435 J · K−1 · mol−1
- ^ ΔfH°, 338.32 kJ · mol−1
- ^ ΔfG°, 298.58 kJ · mol−1
- ^ S°, 166.38 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ 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°, -157.3 kJ · mol−1
- ^ ΔfG°, -129.7 kJ · mol−1
- ^ S°, 42.63 J · K−1 · mol−1
- ^ Cp°, 42.30 J · K−1 · mol−1
- ^ ΔfH°, 50.63 kJ · mol−1
- ^ ΔfG°, 149.34 kJ · mol−1
- ^ S°, 121.21 J · K−1 · mol−1
- ^ Cp°, 98.87 J · K−1 · mol−1
- ^ ΔfH°, 95.40 kJ · mol−1
- ^ ΔfG°, 159.35 kJ · mol−1
- ^ S°, 238.47 J · K−1 · mol−1
- ^ Cp°, 49.58 J · K−1 · mol−1
- ^ ΔfH°, 34.31 kJ · mol−1
- ^ ΔfG°, 128.1 kJ · mol−1
- ^ S°, 138. 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