4C + 3Mn(OH)2 → Mn(CH3COO)2 + 2MnO
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The reaction of and manganese(II) hydroxide yields manganese(II) acetate and manganese(II) oxide. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and manganese(II) hydroxide
General equation
- Reaction of self redoxing species and base
- Self-redoxing speciesSelf redox agent + BaseNon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and manganese(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 4 | – | Self redoxing | ||
| Mn(OH)2 | Manganese(II) hydroxide | 3 | – | Base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(CH3COO)2 | Manganese(II) acetate | 1 | Redoxed product | – |
| MnO | Manganese(II) oxide | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and manganese(II) hydroxide
- 4Crystalline solidgraphite + 3Mn(OH)2Amorphous solidprecipitatedMn(CH3COO)2Crystalline solid + 2MnOCrystalline solid⟶
| 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 | 167.7 | – | – | – |
| 41.92 | – | – | – | |
per 1 mol of | 55.90 | – | – | – |
per 1 mol of | 167.7 | – | – | – |
per 1 mol of | 83.85 | – | – | – |
Changes in standard condition (2)
- Reaction of and manganese(II) hydroxide
- 4Crystalline soliddiamond + 3Mn(OH)2Amorphous solidprecipitatedMn(CH3COO)2Crystalline solid + 2MnOCrystalline solid⟶
| 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 | 160.1 | – | – | – |
| 40.02 | – | – | – | |
per 1 mol of | 53.37 | – | – | – |
per 1 mol of | 160.1 | – | – | – |
per 1 mol of | 80.05 | – | – | – |
Changes in aqueous solution
- Reaction of and manganese(II) hydroxide
- 4Crystalline solidgraphite + 3Mn(OH)2Amorphous solidprecipitatedMn(CH3COO)2Aqueous solution + 2MnOCrystalline solid⟶
| 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 | 116.7 | – | – | – |
| 29.18 | – | – | – | |
per 1 mol of | 38.90 | – | – | – |
per 1 mol of | 116.7 | – | – | – |
per 1 mol of | 58.35 | – | – | – |
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) graphite | 0[1] | 0[1] | 5.740[1] | 8.527[1] |
| (cr) diamond | 1.895[1] | 2.900[1] | 2.377[1] | 6.113[1] |
| (g) | 716.682[1] | 671.257[1] | 158.096[1] | 20.838[1] |
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid
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(CH3COO)2 (cr) | -1148.1[1] | – | – | – |
| Mn(CH3COO)2 (aq) | -1199.1[1] | – | – | – |
| Mn(CH3COO)2 (cr) 4 hydrate | -2338.0[1] | – | – | – |
| MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
| MnO (g) | 124.22[1] | – | – | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (g):Gas
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°, 5.740 J · K−1 · mol−1
- ^ Cp°, 8.527 J · K−1 · mol−1
- ^ ΔfH°, 1.895 kJ · mol−1
- ^ ΔfG°, 2.900 kJ · mol−1
- ^ S°, 2.377 J · K−1 · mol−1
- ^ Cp°, 6.113 J · K−1 · mol−1
- ^ ΔfH°, 716.682 kJ · mol−1
- ^ ΔfG°, 671.257 kJ · mol−1
- ^ S°, 158.096 J · K−1 · mol−1
- ^ Cp°, 20.838 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°, -1148.1 kJ · mol−1
- ^ ΔfH°, -1199.1 kJ · mol−1
- ^ ΔfH°, -2338.0 kJ · mol−1
- ^ ΔfH°, -385.22 kJ · mol−1
- ^ ΔfG°, -362.90 kJ · mol−1
- ^ S°, 59.71 J · K−1 · mol−1
- ^ Cp°, 45.44 J · K−1 · mol−1
- ^ ΔfH°, 124.22 kJ · mol−1