HCl + KIO3 🔥→ KClO3 + HI
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The reaction of hydrogen chloride and potassium iodate yields potassium chlorate and hydrogen 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 hydrogen chloride and potassium iodate
General equation
- Reaction of hardly oxidizable species and oxidizing species
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen chloride and potassium iodate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCl | Hydrogen chloride | 1 | Reducing | Hardly oxidizable |
| KIO3 | Potassium iodate | 1 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO3 | Potassium chlorate | 1 | Oxidized | – |
| HI | Hydrogen iodide | 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and potassium iodate◆
ΔrG 219.10 kJ/mol K 0.41 × 10−38 pK 38.38
| 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 | 222.43 | 219.10 | 11.3 | −6.19 |
per 1 mol of | 222.43 | 219.10 | 11.3 | −6.19 |
per 1 mol of | 222.43 | 219.10 | 11.3 | −6.19 |
per 1 mol of | 222.43 | 219.10 | 11.3 | −6.19 |
per 1 mol of | 222.43 | 219.10 | 11.3 | −6.19 |
Changes in aqueous solution (1)
- Reaction of hydrogen chloride and potassium iodate◆
ΔrG 252.9 kJ/mol K 0.49 × 10−44 pK 44.31
| 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 | 310.9 | 252.9 | 194.0 | – |
per 1 mol of | 310.9 | 252.9 | 194.0 | – |
per 1 mol of | 310.9 | 252.9 | 194.0 | – |
per 1 mol of | 310.9 | 252.9 | 194.0 | – |
per 1 mol of | 310.9 | 252.9 | 194.0 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen chloride and potassium iodate◆
ΔrG 199.6 kJ/mol K 0.11 × 10−34 pK 34.97
| 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 | 229.2 | 199.6 | 98.7 | – |
per 1 mol of | 229.2 | 199.6 | 98.7 | – |
per 1 mol of | 229.2 | 199.6 | 98.7 | – |
per 1 mol of | 229.2 | 199.6 | 98.7 | – |
per 1 mol of | 229.2 | 199.6 | 98.7 | – |
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 |
|---|---|---|---|---|
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[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] | – |
* (g):Gas, (ai):Ionized aqueous solution, (cr):Crystalline solid
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 |
|---|---|---|---|---|
| KClO3 (cr) | -397.73[1] | -296.25[1] | 143.1[1] | 100.25[1] |
| KClO3 (ai) | -356.35[1] | -291.22[1] | 264.8[1] | – |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[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°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 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°, -397.73 kJ · mol−1
- ^ ΔfG°, -296.25 kJ · mol−1
- ^ S°, 143.1 J · K−1 · mol−1
- ^ Cp°, 100.25 J · K−1 · mol−1
- ^ ΔfH°, -356.35 kJ · mol−1
- ^ ΔfG°, -291.22 kJ · mol−1
- ^ S°, 264.8 J · K−1 · mol−1
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1