5MgS + 6KMnO4 → 5MgSO3 + 6MnO + 3K2O
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The reaction of magnesium sulfide and potassium permanganate yields magnesium sulfite, manganese(II) oxide, and potassium oxide (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 magnesium sulfide and potassium permanganate
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of magnesium sulfide and potassium permanganate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgS | Magnesium sulfide | 5 | Reducing | Reducing |
KMnO4 | Potassium permanganate | 6 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
MgSO3 | Magnesium sulfite | 5 | Oxidized | – |
MnO | Manganese(II) oxide | 6 | Reduced | – |
K2O | Potassium oxide | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of magnesium sulfide and potassium permanganate◆
ΔrG −1628.1 kJ/mol K 1.70 × 10285 pK −285.23
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 | −1684.1 | −1628.1 | −201.9 | – |
per 1 mol of | −336.82 | −325.62 | −40.38 | – |
per 1 mol of | −280.68 | −271.35 | −33.65 | – |
per 1 mol of | −336.82 | −325.62 | −40.38 | – |
per 1 mol of | −280.68 | −271.35 | −33.65 | – |
per 1 mol of | −561.37 | −542.70 | −67.30 | – |
Changes in aqueous solution
- Reaction of magnesium sulfide and potassium permanganate◆
ΔrG −1670.7 kJ/mol K 4.94 × 10292 pK −292.69
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 | −1944.5 | −1670.7 | −933.8 | – |
per 1 mol of | −388.90 | −334.14 | −186.8 | – |
per 1 mol of | −324.08 | −278.45 | −155.6 | – |
per 1 mol of | −388.90 | −334.14 | −186.8 | – |
per 1 mol of | −324.08 | −278.45 | −155.6 | – |
per 1 mol of | −648.17 | −556.90 | −311.3 | – |
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 |
---|---|---|---|---|
MgS (cr) | -346.0[1] | -341.8[1] | 50.33[1] | 45.56[1] |
KMnO4 (cr) | -837.2[1] | -737.6[1] | 171.71[1] | 117.57[1] |
KMnO4 (ai) | -793.8[1] | -730.5[1] | 293.7[1] | -60.2[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution
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 |
---|---|---|---|---|
MgSO3 (cr) | -1008.3[1] | -923.8[1] | 87.9[1] | – |
MgSO3 (cr) 3 hydrate | -1931.8[1] | -1674.7[1] | 209.2[1] | – |
MgSO3 (cr) 6 hydrate | -2817.5[1] | -2385.4[1] | 322.2[1] | – |
MnO (cr) | -385.22[1] | -362.90[1] | 59.71[1] | 45.44[1] |
MnO (g) | 124.22[1] | – | – | – |
K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (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°, -346.0 kJ · mol−1
- ^ ΔfG°, -341.8 kJ · mol−1
- ^ S°, 50.33 J · K−1 · mol−1
- ^ Cp°, 45.56 J · K−1 · mol−1
- ^ ΔfH°, -837.2 kJ · mol−1
- ^ ΔfG°, -737.6 kJ · mol−1
- ^ S°, 171.71 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -793.8 kJ · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ S°, 293.7 J · K−1 · mol−1
- ^ Cp°, -60.2 J · K−1 · mol−1
- ^ ΔfH°, -1008.3 kJ · mol−1
- ^ ΔfG°, -923.8 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -1931.8 kJ · mol−1
- ^ ΔfG°, -1674.7 kJ · mol−1
- ^ S°, 209.2 J · K−1 · mol−1
- ^ ΔfH°, -2817.5 kJ · mol−1
- ^ ΔfG°, -2385.4 kJ · mol−1
- ^ S°, 322.2 J · K−1 · 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
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280