6KI + 4SrSO4 🔥→ 3K2SO4 + 3I2 + S + 4SrO
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- Reaction of potassium iodide and strontium sulfate
The reaction of potassium iodide and strontium sulfate yields potassium sulfate, , , and strontium 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 potassium iodide and strontium sulfate
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium iodide and strontium sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 6 | Reducing | Oxidizable |
| SrSO4 | Strontium sulfate | 4 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SO4 | Potassium sulfate | 3 | – | – |
| 3 | Oxidized | – | ||
| 1 | Reduced | – | ||
| SrO | Strontium oxide | 4 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of potassium iodide and strontium sulfate◆
ΔrG 1101.2 kJ/mol K 0.12 × 10−192 pK 192.92
| 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 | 1098.4 | 1101.2 | 19 | – |
per 1 mol of | 183.07 | 183.53 | 3.2 | – |
per 1 mol of | 274.60 | 275.30 | 4.8 | – |
per 1 mol of | 366.13 | 367.07 | 6.3 | – |
| 366.13 | 367.07 | 6.3 | – | |
| 1098.4 | 1101.2 | 19 | – | |
per 1 mol of | 274.60 | 275.30 | 4.8 | – |
Changes in standard condition (2)
- Reaction of potassium iodide and strontium sulfate
| 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 | 1098.8 | – | – | – |
per 1 mol of | 183.13 | – | – | – |
per 1 mol of | 274.70 | – | – | – |
per 1 mol of | 366.27 | – | – | – |
| 366.27 | – | – | – | |
| 1098.8 | – | – | – | |
per 1 mol of | 274.70 | – | – | – |
Changes in standard condition (3)
- Reaction of potassium iodide and strontium sulfate
| 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 | 1085.2 | – | – | – |
per 1 mol of | 180.87 | – | – | – |
per 1 mol of | 271.30 | – | – | – |
per 1 mol of | 361.73 | – | – | – |
| 361.73 | – | – | – | |
| 1085.2 | – | – | – | |
per 1 mol of | 271.30 | – | – | – |
Changes in standard condition (4)
- Reaction of potassium iodide and strontium sulfate
| 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 | 1085.6 | – | – | – |
per 1 mol of | 180.93 | – | – | – |
per 1 mol of | 271.40 | – | – | – |
per 1 mol of | 361.87 | – | – | – |
| 361.87 | – | – | – | |
| 1085.6 | – | – | – | |
per 1 mol of | 271.40 | – | – | – |
Changes in aqueous solution (1)
- Reaction of potassium iodide and strontium sulfate◆
ΔrG 1241.1 kJ/mol K 0.37 × 10−217 pK 217.43
| 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 | 1115.6 | 1241.1 | −415 | – |
per 1 mol of | 185.93 | 206.85 | −69.2 | – |
per 1 mol of | 278.90 | 310.27 | −104 | – |
per 1 mol of | 371.87 | 413.70 | −138 | – |
| 371.87 | 413.70 | −138 | – | |
| 1115.6 | 1241.1 | −415 | – | |
per 1 mol of | 278.90 | 310.27 | −104 | – |
Changes in aqueous solution (2)
- Reaction of potassium iodide and strontium sulfate
| 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 | 1102.4 | – | – | – |
per 1 mol of | 183.73 | – | – | – |
per 1 mol of | 275.60 | – | – | – |
per 1 mol of | 367.47 | – | – | – |
| 367.47 | – | – | – | |
| 1102.4 | – | – | – | |
per 1 mol of | 275.60 | – | – | – |
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 |
|---|---|---|---|---|
| KI (cr) | -327.900[1] | -324.892[1] | 106.32[1] | 52.93[1] |
| KI (g) | -125.5[1] | -166.1[1] | 258.3[1] | 37.11[1] |
| KI (ai) | -307.57[1] | -334.85[1] | 213.8[1] | -120.5[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] | – |
* (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 |
|---|---|---|---|---|
| K2SO4 (cr) | -1437.79[1] | -1321.37[1] | 175.56[1] | 131.46[1] |
| K2SO4 (g) | -1096[1] | -1033[1] | 364[1] | 108.8[1] |
| K2SO4 (ai) | -1414.02[1] | -1311.07[1] | 225.1[1] | -251[1] |
| (cr) | 0[1] | 0[1] | 116.135[1] | 54.438[1] |
| (g) | 62.438[1] | 19.327[1] | 260.69[1] | 36.90[1] |
| (ao) | 22.6[1] | 16.40[1] | 137.2[1] | – |
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| SrO (cr) | -592.0[1] | -561.9[1] | 54.4[1] | 45.02[1] |
| SrO (g) | -8[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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°, -327.900 kJ · mol−1
- ^ ΔfG°, -324.892 kJ · mol−1
- ^ S°, 106.32 J · K−1 · mol−1
- ^ Cp°, 52.93 J · K−1 · mol−1
- ^ ΔfH°, -125.5 kJ · mol−1
- ^ ΔfG°, -166.1 kJ · mol−1
- ^ S°, 258.3 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -307.57 kJ · mol−1
- ^ ΔfG°, -334.85 kJ · mol−1
- ^ S°, 213.8 J · K−1 · mol−1
- ^ Cp°, -120.5 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°, -1437.79 kJ · mol−1
- ^ ΔfG°, -1321.37 kJ · mol−1
- ^ S°, 175.56 J · K−1 · mol−1
- ^ Cp°, 131.46 J · K−1 · mol−1
- ^ ΔfH°, -1096. kJ · mol−1
- ^ ΔfG°, -1033. kJ · mol−1
- ^ S°, 364. J · K−1 · mol−1
- ^ Cp°, 108.8 J · K−1 · mol−1
- ^ ΔfH°, -1414.02 kJ · mol−1
- ^ ΔfG°, -1311.07 kJ · mol−1
- ^ S°, 225.1 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 116.135 J · K−1 · mol−1
- ^ Cp°, 54.438 J · K−1 · mol−1
- ^ ΔfH°, 62.438 kJ · mol−1
- ^ ΔfG°, 19.327 kJ · mol−1
- ^ S°, 260.69 J · K−1 · mol−1
- ^ Cp°, 36.90 J · K−1 · mol−1
- ^ ΔfH°, 22.6 kJ · mol−1
- ^ ΔfG°, 16.40 kJ · mol−1
- ^ S°, 137.2 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -592.0 kJ · mol−1
- ^ ΔfG°, -561.9 kJ · mol−1
- ^ S°, 54.4 J · K−1 · mol−1
- ^ Cp°, 45.02 J · K−1 · mol−1
- ^ ΔfH°, -8. kJ · mol−1