2MnSiO3 🔥→ 2Mn + 2Si + 3O2↑
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- Decomposition of manganese(II) metasilicate
Decomposition of manganese(II) metasilicate 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) metasilicate
General equation
- Thermal decomposition with redox
- Thermally decomposable substanceSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
- Thermal decomposition of oxoacid salt with redox
- Oxoacid saltSelf redox agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Decomposition of manganese(II) metasilicate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnSiO3 | Manganese(II) metasilicate | 2 | Self redox agent | Thermally decomposable Oxoacid salt |
Products
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of manganese(II) metasilicate◆
ΔrG 2481.0 kJ/mol K 0.22 × 10−434 pK 434.65
| 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 | 2641.8 | 2481.0 | 538.9 | 7.83 |
per 1 mol of | 1320.9 | 1240.5 | 269.4 | 3.92 |
| 1320.9 | 1240.5 | 269.4 | 3.92 | |
| 1320.9 | 1240.5 | 269.4 | 3.92 | |
| 880.60 | 827.00 | 179.6 | 2.61 |
Changes in standard condition (2)
- Decomposition of manganese(II) metasilicate
| 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 | 2650.2 | – | – | – |
per 1 mol of | 1325.1 | – | – | – |
| 1325.1 | – | – | – | |
| 1325.1 | – | – | – | |
| 883.40 | – | – | – |
Changes in standard condition (3)
- Decomposition of manganese(II) metasilicate
| 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 | – | – | 543.7 | 8.25 |
per 1 mol of | – | – | 271.9 | 4.13 |
| – | – | 271.9 | 4.13 | |
| – | – | 271.9 | 4.13 | |
| – | – | 181.2 | 2.75 |
Changes in standard condition (4)
- Decomposition of manganese(II) metasilicate
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
| – | – | – | – | |
| – | – | – | – |
Changes in standard condition (5)
- Decomposition of manganese(II) metasilicate◆
ΔrG 2483.8 kJ/mol K 0.72 × 10−435 pK 435.14
| 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 | 2644.9 | 2483.8 | 539.7 | 10.33 |
per 1 mol of | 1322.5 | 1241.9 | 269.9 | 5.165 |
| 1322.5 | 1241.9 | 269.9 | 5.165 | |
| 1322.5 | 1241.9 | 269.9 | 5.165 | |
| 881.63 | 827.93 | 179.9 | 3.443 |
Changes in standard condition (6)
- Decomposition of manganese(II) metasilicate
| 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 | 2653.3 | – | – | – |
per 1 mol of | 1326.7 | – | – | – |
| 1326.7 | – | – | – | |
| 1326.7 | – | – | – | |
| 884.43 | – | – | – |
Changes in aqueous solution (1)
- Decomposition of manganese(II) metasilicate◆
ΔrG 2481.0 kJ/mol K 0.22 × 10−434 pK 434.65
| 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 | 2641.8 | 2481.0 | 538.9 | 7.83 |
per 1 mol of | 1320.9 | 1240.5 | 269.4 | 3.92 |
| 1320.9 | 1240.5 | 269.4 | 3.92 | |
| 1320.9 | 1240.5 | 269.4 | 3.92 | |
| 880.60 | 827.00 | 179.6 | 2.61 |
Changes in aqueous solution (2)
- Decomposition of manganese(II) metasilicate◆
ΔrG 2530.2 kJ/mol K 0.53 × 10−443 pK 443.27
| 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 | 2606.7 | 2530.2 | 256.2 | – |
per 1 mol of | 1303.3 | 1265.1 | 128.1 | – |
| 1303.3 | 1265.1 | 128.1 | – | |
| 1303.3 | 1265.1 | 128.1 | – | |
| 868.90 | 843.40 | 85.40 | – |
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 |
|---|---|---|---|---|
| MnSiO3 (cr) | -1320.9[1] | -1240.5[1] | 89.1[1] | 86.44[1] |
| MnSiO3 (vit) | -1285.3[1] | – | – | – |
* (cr):Crystalline solid, (vit):Vitreous 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 |
|---|---|---|---|---|
| (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] |
| (cr) | 0[1] | 0[1] | 18.83[1] | 20.00[1] |
| (am) | 4.2[1] | – | – | – |
| (g) | 455.6[1] | 411.3[1] | 167.97[1] | 22.251[1] |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[1] | – |
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid, (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°, -1320.9 kJ · mol−1
- ^ ΔfG°, -1240.5 kJ · mol−1
- ^ S°, 89.1 J · K−1 · mol−1
- ^ Cp°, 86.44 J · K−1 · mol−1
- ^ ΔfH°, -1285.3 kJ · 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 18.83 J · K−1 · mol−1
- ^ Cp°, 20.00 J · K−1 · mol−1
- ^ ΔfH°, 4.2 kJ · mol−1
- ^ ΔfH°, 455.6 kJ · mol−1
- ^ ΔfG°, 411.3 kJ · mol−1
- ^ S°, 167.97 J · K−1 · mol−1
- ^ Cp°, 22.251 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1