Mn(OH)2 🔥→ Mn + H2O2
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- Decomposition of manganese(II) hydroxide
Decomposition of manganese(II) hydroxide yields and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Decomposition of manganese(II) hydroxide
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of manganese(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(OH)2 | Manganese(II) hydroxide | 1 | Self redox agent | Thermally decomposable |
Products
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of manganese(II) hydroxide◆
ΔrG 494.7 kJ/mol K 0.21 × 10−86 pK 86.67
| 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 | 507.6 | 494.7 | 42.4 | – |
per 1 mol of | 507.6 | 494.7 | 42.4 | – |
| 507.6 | 494.7 | 42.4 | – | |
| 507.6 | 494.7 | 42.4 | – |
Changes in standard condition (2)
- Decomposition of manganese(II) hydroxide
| 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 | – | – | 44.8 | – |
per 1 mol of | – | – | 44.8 | – |
| – | – | 44.8 | – | |
| – | – | 44.8 | – |
Changes in standard condition (3)
- Decomposition of manganese(II) hydroxide◆
ΔrG 496.1 kJ/mol K 0.12 × 10−86 pK 86.91
| 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 | 509.2 | 496.1 | 42.8 | – |
per 1 mol of | 509.2 | 496.1 | 42.8 | – |
| 509.2 | 496.1 | 42.8 | – | |
| 509.2 | 496.1 | 42.8 | – |
Changes in aqueous solution
- Decomposition of manganese(II) hydroxide◆
ΔrG 481.0 kJ/mol K 0.54 × 10−84 pK 84.27
| 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 | 504.2 | 481.0 | 76.7 | – |
per 1 mol of | 504.2 | 481.0 | 76.7 | – |
| 504.2 | 481.0 | 76.7 | – | |
| 504.2 | 481.0 | 76.7 | – |
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(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
* (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 |
|---|---|---|---|---|
| (cr) α | 0[1] | 0[1] | 32.01[1] | 26.32[1] |
| (cr) β | – | – | 34.39[1] | 26.53[1] |
| (cr) γ | 1.55[1] | 1.42[1] | 32.43[1] | 27.57[1] |
| (g) | 280.7[1] | 238.5[1] | 173.70[1] | 20.79[1] |
| (l) | -187.78[1] | -120.35[1] | 109.6[1] | 89.1[1] |
| (g) | -136.31[1] | -105.57[1] | 232.7[1] | 43.1[1] |
| (ao) | -191.17[1] | -134.03[1] | 143.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (l):Liquid, (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°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 32.01 J · K−1 · mol−1
- ^ Cp°, 26.32 J · K−1 · mol−1
- ^ S°, 34.39 J · K−1 · mol−1
- ^ Cp°, 26.53 J · K−1 · mol−1
- ^ ΔfH°, 1.55 kJ · mol−1
- ^ ΔfG°, 1.42 kJ · mol−1
- ^ S°, 32.43 J · K−1 · mol−1
- ^ Cp°, 27.57 J · K−1 · mol−1
- ^ ΔfH°, 280.7 kJ · mol−1
- ^ ΔfG°, 238.5 kJ · mol−1
- ^ S°, 173.70 J · K−1 · mol−1
- ^ Cp°, 20.79 J · K−1 · mol−1
- ^ ΔfH°, -187.78 kJ · mol−1
- ^ ΔfG°, -120.35 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ Cp°, 89.1 J · K−1 · mol−1
- ^ ΔfH°, -136.31 kJ · mol−1
- ^ ΔfG°, -105.57 kJ · mol−1
- ^ S°, 232.7 J · K−1 · mol−1
- ^ Cp°, 43.1 J · K−1 · mol−1
- ^ ΔfH°, -191.17 kJ · mol−1
- ^ ΔfG°, -134.03 kJ · mol−1
- ^ S°, 143.9 J · K−1 · mol−1