8KI + SrSO4 🔥→ K2S + 3K2O + 4I2 + SrO
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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 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 | 8 | 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 | 3 | – | – |
4 | Oxidized | – | ||
SrO | Strontium oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of potassium iodide and strontium sulfate◆
ΔrG 2047.8 kJ/mol K 0.17 × 10−358 pK 358.76
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 | 2019.1 | 2047.8 | −61 | – |
per 1 mol of | 252.39 | 255.97 | −7.6 | – |
per 1 mol of | 2019.1 | 2047.8 | −61 | – |
per 1 mol of | 2019.1 | 2047.8 | −61 | – |
per 1 mol of | 673.03 | 682.60 | −20 | – |
504.77 | 511.95 | −15 | – | |
per 1 mol of | 2019.1 | 2047.8 | −61 | – |
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 | 2015.8 | – | – | – |
per 1 mol of | 251.97 | – | – | – |
per 1 mol of | 2015.8 | – | – | – |
per 1 mol of | 2015.8 | – | – | – |
per 1 mol of | 671.93 | – | – | – |
503.95 | – | – | – | |
per 1 mol of | 2015.8 | – | – | – |
Changes in aqueous solution (1)
- Reaction of potassium iodide and strontium sulfate◆
ΔrG 2076.4 kJ/mol K 0.17 × 10−363 pK 363.77
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 | 1856.1 | 2076.4 | −752 | – |
per 1 mol of | 232.01 | 259.55 | −94.0 | – |
per 1 mol of | 1856.1 | 2076.4 | −752 | – |
per 1 mol of | 1856.1 | 2076.4 | −752 | – |
per 1 mol of | 618.70 | 692.13 | −251 | – |
464.02 | 519.10 | −188 | – | |
per 1 mol of | 1856.1 | 2076.4 | −752 | – |
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 | 1852.8 | – | – | – |
per 1 mol of | 231.60 | – | – | – |
per 1 mol of | 1852.8 | – | – | – |
per 1 mol of | 1852.8 | – | – | – |
per 1 mol of | 617.60 | – | – | – |
463.20 | – | – | – | |
per 1 mol of | 1852.8 | – | – | – |
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] | – |
SrO (cr) | -592.0[1] | -561.9[1] | 54.4[1] | 45.02[1] |
SrO (g) | -8[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°, -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
- 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