3SrS + 8KMnO4 → 3SrSO4 + 8MnO2 + 4K2O
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The reaction of strontium sulfide and potassium permanganate yields strontium sulfate, manganese(IV) 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 strontium 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 strontium sulfide and potassium permanganate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SrS | Strontium sulfide | 3 | Reducing | Reducing |
KMnO4 | Potassium permanganate | 8 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SrSO4 | Strontium sulfate | 3 | Oxidized | – |
MnO2 | Manganese(IV) oxide | 8 | Reduced | – |
K2O | Potassium oxide | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of strontium sulfide and potassium permanganate◆
ΔrG −1728.0 kJ/mol K 5.40 × 10302 pK −302.73
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 | −1850.7 | −1728.0 | −426 | – |
per 1 mol of | −616.90 | −576.00 | −142 | – |
per 1 mol of | −231.34 | −216.00 | −53.3 | – |
per 1 mol of | −616.90 | −576.00 | −142 | – |
per 1 mol of | −231.34 | −216.00 | −53.3 | – |
per 1 mol of | −462.68 | −432.00 | −107 | – |
Changes in standard condition (2)
- Reaction of strontium sulfide and potassium permanganate
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 | −1710.5 | – | – | – |
per 1 mol of | −570.17 | – | – | – |
per 1 mol of | −213.81 | – | – | – |
per 1 mol of | −570.17 | – | – | – |
per 1 mol of | −213.81 | – | – | – |
per 1 mol of | −427.63 | – | – | – |
Changes in standard condition (3)
- Reaction of strontium sulfide and potassium permanganate
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 | −1840.8 | – | – | – |
per 1 mol of | −613.60 | – | – | – |
per 1 mol of | −230.10 | – | – | – |
per 1 mol of | −613.60 | – | – | – |
per 1 mol of | −230.10 | – | – | – |
per 1 mol of | −460.20 | – | – | – |
Changes in standard condition (4)
- Reaction of strontium sulfide and potassium permanganate
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 | −1700.6 | – | – | – |
per 1 mol of | −566.87 | – | – | – |
per 1 mol of | −212.57 | – | – | – |
per 1 mol of | −566.87 | – | – | – |
per 1 mol of | −212.57 | – | – | – |
per 1 mol of | −425.15 | – | – | – |
Changes in aqueous solution (1)
- Reaction of strontium sulfide and potassium permanganate◆
ΔrG −1784.8 kJ/mol K 4.82 × 10312 pK −312.68
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 | −2197.9 | −1784.8 | −1402 | – |
per 1 mol of | −732.63 | −594.93 | −467.3 | – |
per 1 mol of | −274.74 | −223.10 | −175.3 | – |
per 1 mol of | −732.63 | −594.93 | −467.3 | – |
per 1 mol of | −274.74 | −223.10 | −175.3 | – |
per 1 mol of | −549.48 | −446.20 | −350.5 | – |
Changes in aqueous solution (2)
- Reaction of strontium sulfide and potassium permanganate
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 | −2188.0 | – | – | – |
per 1 mol of | −729.33 | – | – | – |
per 1 mol of | −273.50 | – | – | – |
per 1 mol of | −729.33 | – | – | – |
per 1 mol of | −273.50 | – | – | – |
per 1 mol of | −547.00 | – | – | – |
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 |
---|---|---|---|---|
SrS (cr) | -472.4[1] | -467.8[1] | 68.2[1] | 48.70[1] |
SrS (g) | 109[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, (g):Gas, (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 |
---|---|---|---|---|
SrSO4 (cr) | -1453.1[1] | -1340.9[1] | 117[1] | – |
SrSO4 (cr) precipitated | -1449.8[1] | – | – | – |
SrSO4 (ai) | -1455.07[1] | -1304.00[1] | -12.6[1] | – |
MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
MnO2 (am) precipitated | -502.5[1] | – | – | – |
K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous 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°, -472.4 kJ · mol−1
- ^ ΔfG°, -467.8 kJ · mol−1
- ^ S°, 68.2 J · K−1 · mol−1
- ^ Cp°, 48.70 J · K−1 · mol−1
- ^ ΔfH°, 109. kJ · 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°, -1453.1 kJ · mol−1
- ^ ΔfG°, -1340.9 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -1449.8 kJ · mol−1
- ^ ΔfH°, -1455.07 kJ · mol−1
- ^ ΔfG°, -1304.00 kJ · mol−1
- ^ S°, -12.6 J · K−1 · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 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