16KI + Mg3(AsO4)2 🔥→ 8K2O + 5I2 + 2As + 3MgI2
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- Reaction of potassium iodide and magnesium arsenate
The reaction of potassium iodide and magnesium arsenate yields potassium oxide, , , and magnesium 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 magnesium arsenate
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 magnesium arsenate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 16 | Reducing | Oxidizable |
| Mg3(AsO4)2 | Magnesium arsenate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 8 | – | – |
| 5 | Oxidized | – | ||
| 2 | Reduced | – | ||
| MgI2 | Magnesium iodide | 3 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of potassium iodide and magnesium arsenate
- 16KICrystalline solid + Mg3(AsO4)2Crystalline solid8K2OCrystalline solid + 5Crystalline solid + 2Crystalline solidα, gray, metallic + 3MgI2Crystalline solid🔥⟶
| 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 | 4355.2 | – | – | – |
per 1 mol of | 272.20 | – | – | – |
per 1 mol of | 4355.2 | – | – | – |
per 1 mol of | 544.40 | – | – | – |
| 871.04 | – | – | – | |
| 2177.6 | – | – | – | |
per 1 mol of | 1451.7 | – | – | – |
Changes in standard condition (2)
- Reaction of potassium iodide and magnesium arsenate
- 16KICrystalline solid + Mg3(AsO4)2Crystalline solid8K2OCrystalline solid + 5Crystalline solid + 2Crystalline solidγ, yellow, cubic + 3MgI2Crystalline solid🔥⟶
| 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 | 4384.4 | – | – | – |
per 1 mol of | 274.02 | – | – | – |
per 1 mol of | 4384.4 | – | – | – |
per 1 mol of | 548.05 | – | – | – |
| 876.88 | – | – | – | |
| 2192.2 | – | – | – | |
per 1 mol of | 1461.5 | – | – | – |
Changes in standard condition (3)
- Reaction of potassium iodide and magnesium arsenate
- 16KICrystalline solid + Mg3(AsO4)2Crystalline solid8K2OCrystalline solid + 5Crystalline solid + 2Amorphous solidβ + 3MgI2Crystalline solid🔥⟶
| 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 | 4363.6 | – | – | – |
per 1 mol of | 272.73 | – | – | – |
per 1 mol of | 4363.6 | – | – | – |
per 1 mol of | 545.45 | – | – | – |
| 872.72 | – | – | – | |
| 2181.8 | – | – | – | |
per 1 mol of | 1454.5 | – | – | – |
Changes in aqueous solution
- Reaction of potassium iodide and magnesium arsenate
- 16KIIonized aqueous solution + Mg3(AsO4)2Crystalline solid8K2OCrystalline solid + 5Un-ionized aqueous solution + 2Crystalline solidα, gray, metallic + 3MgI2Ionized aqueous solution🔥⟶
| 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 | 3503.3 | – | – | – |
per 1 mol of | 218.96 | – | – | – |
per 1 mol of | 3503.3 | – | – | – |
per 1 mol of | 437.91 | – | – | – |
| 700.66 | – | – | – | |
| 1751.7 | – | – | – | |
per 1 mol of | 1167.8 | – | – | – |
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] |
| Mg3(AsO4)2 (cr) | -3092.8[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 |
|---|---|---|---|---|
| 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] | – |
| (cr) α, gray, metallic | 0[1] | 0[1] | 35.1[1] | 24.64[1] |
| (cr) γ, yellow, cubic | 14.6[1] | – | – | – |
| (am) β | 4.2[1] | – | – | – |
| (g) | 302.5[1] | 261.0[1] | 174.21[1] | 20.786[1] |
| MgI2 (cr) | -364.0[1] | -358.2[1] | 129.7[1] | – |
| MgI2 (g) | -172[1] | – | – | – |
| MgI2 (ai) | -577.22[1] | -558.1[1] | 84.5[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (am):Amorphous solid, (ai):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°, -3092.8 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 35.1 J · K−1 · mol−1
- ^ Cp°, 24.64 J · K−1 · mol−1
- ^ ΔfH°, 14.6 kJ · mol−1
- ^ ΔfH°, 4.2 kJ · mol−1
- ^ ΔfH°, 302.5 kJ · mol−1
- ^ ΔfG°, 261.0 kJ · mol−1
- ^ S°, 174.21 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -364.0 kJ · mol−1
- ^ ΔfG°, -358.2 kJ · mol−1
- ^ S°, 129.7 J · K−1 · mol−1
- ^ ΔfH°, -172. kJ · mol−1
- ^ ΔfH°, -577.22 kJ · mol−1
- ^ ΔfG°, -558.1 kJ · mol−1
- ^ S°, 84.5 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