7KI + 3Na2SeO4 🔥→ KIO3 + 3K2SeO3 + 6NaI
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The reaction of potassium iodide and sodium selenate yields potassium iodate, potassium selenite, and sodium 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 sodium selenate
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 sodium selenate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
KI | Potassium iodide | 7 | Reducing | Oxidizable |
Na2SeO4 | Sodium selenate | 3 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
KIO3 | Potassium iodate | 1 | Oxidized | – |
K2SeO3 | Potassium selenite | 3 | Reduced | – |
NaI | Sodium iodide | 6 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium iodide and sodium selenate
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 | 328.3 | – | – | – |
per 1 mol of | 46.90 | – | – | – |
per 1 mol of | 109.4 | – | – | – |
per 1 mol of | 328.3 | – | – | – |
per 1 mol of | 109.4 | – | – | – |
per 1 mol of | 54.72 | – | – | – |
Changes in aqueous solution
- Reaction of potassium iodide and sodium selenate◆
ΔrG 138.6 kJ/mol K 0.52 × 10−24 pK 24.28
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 | 104.6 | 138.6 | −115.9 | – |
per 1 mol of | 14.94 | 19.80 | −16.56 | – |
per 1 mol of | 34.87 | 46.20 | −38.63 | – |
per 1 mol of | 104.6 | 138.6 | −115.9 | – |
per 1 mol of | 34.87 | 46.20 | −38.63 | – |
per 1 mol of | 17.43 | 23.10 | −19.32 | – |
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] |
Na2SeO4 (cr) | -1069.0[1] | – | – | – |
Na2SeO4 (ai) | -1079.5[1] | -965.2[1] | 172.0[1] | – |
Na2SeO4 (cr) 10 hydrate | -4006.6[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 |
---|---|---|---|---|
KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[1] | – |
K2SeO3 (cr) | -982.0[1] | – | – | – |
K2SeO3 (ai) | -1013.8[1] | -936.3[1] | 218.0[1] | – |
NaI (cr) | -287.78[1] | -286.06[1] | 98.53[1] | 52.09[1] |
NaI (g) | -79.5[1] | -121.0[1] | 248.978[1] | 36.65[1] |
NaI (ai) | -295.31[1] | -313.47[1] | 170.3[1] | -95.8[1] |
NaI (cr) 1 hydrate | -883.096[1] | -771.10[1] | 196.2[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -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°, -1069.0 kJ · mol−1
- ^ ΔfH°, -1079.5 kJ · mol−1
- ^ ΔfG°, -965.2 kJ · mol−1
- ^ S°, 172.0 J · K−1 · mol−1
- ^ ΔfH°, -4006.6 kJ · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 J · K−1 · mol−1
- ^ ΔfH°, -982.0 kJ · mol−1
- ^ ΔfH°, -1013.8 kJ · mol−1
- ^ ΔfG°, -936.3 kJ · mol−1
- ^ S°, 218.0 J · K−1 · mol−1
- ^ ΔfH°, -287.78 kJ · mol−1
- ^ ΔfG°, -286.06 kJ · mol−1
- ^ S°, 98.53 J · K−1 · mol−1
- ^ Cp°, 52.09 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -121.0 kJ · mol−1
- ^ S°, 248.978 J · K−1 · mol−1
- ^ Cp°, 36.65 J · K−1 · mol−1
- ^ ΔfH°, -295.31 kJ · mol−1
- ^ ΔfG°, -313.47 kJ · mol−1
- ^ S°, 170.3 J · K−1 · mol−1
- ^ Cp°, -95.8 J · K−1 · mol−1
- ^ ΔfH°, -883.096 kJ · mol−1
- ^ ΔfG°, -771.10 kJ · mol−1
- ^ S°, 196.2 J · K−1 · mol−1