10KI + SrSO4 🔥→ K2S + 4K2O + 4I2 + SrI2
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- Reaction of potassium iodide and strontium sulfate
The reaction of potassium iodide and strontium sulfate yields potassium sulfide, potassium oxide, , and strontium iodide (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 | 10 | Reducing | Oxidizable |
| SrSO4 | Strontium sulfate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2S | Potassium sulfide | 1 | Reduced | – |
| K2O | Potassium oxide | 4 | – | – |
| 4 | Oxidized | – | ||
| SrI2 | Strontium iodide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- 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 | 2347.3 | – | – | – |
per 1 mol of | 234.73 | – | – | – |
per 1 mol of | 2347.3 | – | – | – |
per 1 mol of | 2347.3 | – | – | – |
per 1 mol of | 586.83 | – | – | – |
| 586.83 | – | – | – | |
per 1 mol of | 2347.3 | – | – | – |
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 | 2344.0 | – | – | – |
per 1 mol of | 234.40 | – | – | – |
per 1 mol of | 2344.0 | – | – | – |
per 1 mol of | 2344.0 | – | – | – |
per 1 mol of | 586.00 | – | – | – |
| 586.00 | – | – | – | |
per 1 mol of | 2344.0 | – | – | – |
Changes in aqueous solution (1)
- Reaction of potassium iodide and strontium sulfate◆
ΔrG 2323.3 kJ/mol K 0.95 × 10−407 pK 407.02
| 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 | 2045.5 | 2323.3 | −949 | – |
per 1 mol of | 204.55 | 232.33 | −94.9 | – |
per 1 mol of | 2045.5 | 2323.3 | −949 | – |
per 1 mol of | 2045.5 | 2323.3 | −949 | – |
per 1 mol of | 511.38 | 580.83 | −237 | – |
| 511.38 | 580.83 | −237 | – | |
per 1 mol of | 2045.5 | 2323.3 | −949 | – |
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 | 2042.2 | – | – | – |
per 1 mol of | 204.22 | – | – | – |
per 1 mol of | 2042.2 | – | – | – |
per 1 mol of | 2042.2 | – | – | – |
per 1 mol of | 510.55 | – | – | – |
| 510.55 | – | – | – | |
per 1 mol of | 2042.2 | – | – | – |
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 |
|---|---|---|---|---|
| K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
| K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
| K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
| K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[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] | – |
| SrI2 (cr) | -558.1[1] | – | – | 81.6[1] |
| SrI2 (g) | -272[1] | – | – | – |
| SrI2 (ai) | -656.18[1] | -662.62[1] | 190.0[1] | – |
| SrI2 (cr) 1 hydrate | -886.6[1] | – | – | 119.2[1] |
| SrI2 (cr) 2 hydrate | -1182.4[1] | – | – | 163.6[1] |
| SrI2 (cr) 6 hydrate | -2388.6[1] | – | – | 355.2[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · 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°, -558.1 kJ · mol−1
- ^ Cp°, 81.6 J · K−1 · mol−1
- ^ ΔfH°, -272. kJ · mol−1
- ^ ΔfH°, -656.18 kJ · mol−1
- ^ ΔfG°, -662.62 kJ · mol−1
- ^ S°, 190.0 J · K−1 · mol−1
- ^ ΔfH°, -886.6 kJ · mol−1
- ^ Cp°, 119.2 J · K−1 · mol−1
- ^ ΔfH°, -1182.4 kJ · mol−1
- ^ Cp°, 163.6 J · K−1 · mol−1
- ^ ΔfH°, -2388.6 kJ · mol−1
- ^ Cp°, 355.2 J · K−1 · 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