KI + 3F2 + 3H2O → KIO3 + 6HF
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- Reaction of potassium iodide and under neutral condition
The reaction of potassium iodide, , and water yields potassium iodate and hydrogen fluoride. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium iodide and under neutral condition
General equation
- Reaction of oxidizable species and oxidizing species under neutral condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium iodide and under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 1 | Reducing | Oxidizable |
| 3 | Oxidizing | Oxidizing | ||
| H2O | Water | 3 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 1 | Oxidized | – |
| HF | Hydrogen fluoride | 6 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium iodide and under neutral condition◆
ΔrG −1021.3 kJ/mol K 8.39 × 10178 pK −178.92
| 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 | −942.6 | −1021.3 | 269.74 | −91.43 |
per 1 mol of | −942.6 | −1021.3 | 269.74 | −91.43 |
| −314.2 | −340.43 | 89.913 | −30.48 | |
per 1 mol of | −314.2 | −340.43 | 89.913 | −30.48 |
per 1 mol of | −942.6 | −1021.3 | 269.74 | −91.43 |
per 1 mol of | −157.1 | −170.22 | 44.957 | −15.24 |
Changes in aqueous solution (1)
- Reaction of potassium iodide and under neutral condition◆
ΔrG −1004.2 kJ/mol K 8.48 × 10175 pK −175.93
| 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 | −935.1 | −1004.2 | 231.7 | – |
per 1 mol of | −935.1 | −1004.2 | 231.7 | – |
| −311.7 | −334.73 | 77.23 | – | |
per 1 mol of | −311.7 | −334.73 | 77.23 | – |
per 1 mol of | −935.1 | −1004.2 | 231.7 | – |
per 1 mol of | −155.8 | −167.37 | 38.62 | – |
Changes in aqueous solution (2)
- Reaction of potassium iodide and under neutral condition◆
ΔrG −1145.9 kJ/mol K 5.66 × 10200 pK −200.75
| 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 | −1229.0 | −1145.9 | −278.8 | – |
per 1 mol of | −1229.0 | −1145.9 | −278.8 | – |
| −409.67 | −381.97 | −92.93 | – | |
per 1 mol of | −409.67 | −381.97 | −92.93 | – |
per 1 mol of | −1229.0 | −1145.9 | −278.8 | – |
per 1 mol of | −204.83 | −190.98 | −46.47 | – |
Changes in aqueous solution (3)
- Reaction of potassium iodide and under neutral condition◆
ΔrG −1145.9 kJ/mol K 5.66 × 10200 pK −200.75
| 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 | −1229.0 | −1145.9 | −278.8 | – |
per 1 mol of | −1229.0 | −1145.9 | −278.8 | – |
| −409.67 | −381.97 | −92.93 | – | |
per 1 mol of | −409.67 | −381.97 | −92.93 | – |
per 1 mol of | −1229.0 | −1145.9 | −278.8 | – |
per 1 mol of | −204.83 | −190.98 | −46.47 | – |
Changes in aqueous solution (4)
- Reaction of potassium iodide and under neutral condition◆
ΔrG −1037.7 kJ/mol K 6.27 × 10181 pK −181.80
| 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 | −1304.3 | −1037.7 | −893.8 | – |
per 1 mol of | −1304.3 | −1037.7 | −893.8 | – |
| −434.77 | −345.90 | −297.9 | – | |
per 1 mol of | −434.77 | −345.90 | −297.9 | – |
per 1 mol of | −1304.3 | −1037.7 | −893.8 | – |
per 1 mol of | −217.38 | −172.95 | −149.0 | – |
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] |
| (g) | 0[1] | 0[1] | 202.78[1] | 31.30[1] |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid
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] | – |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 202.78 J · K−1 · mol−1
- ^ Cp°, 31.30 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · 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°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1