2KClO + H2[PtCl6] → K2[PtCl6] + HClO2 + HCl↑
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The reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid yields potassium hexachloridoplatinate(IV), chlorous acid, and hydrogen chloride (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 hypochlorite and hexachloridoplatinic(IV) acid
General equation
- Reaction of self redoxing species and acid
- Self-redoxing speciesSelf redox agent + AcidNon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO | Potassium hypochlorite | 2 | – | Self redoxing |
| H2[PtCl6] | Hexachloridoplatinic(IV) acid | 1 | – | Acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2[PtCl6] | Potassium hexachloridoplatinate(IV) | 1 | Reduced | – |
| HClO2 | Chlorous acid | 1 | Oxidized | – |
| HCl | Hydrogen chloride | 1 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid◆
ΔrG −15.9 kJ/mol K 6.10 × 102 pK −2.79
| 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 | 70.0 | −15.9 | 288 | – |
per 1 mol of | 35.0 | −7.95 | 144 | – |
per 1 mol of | 70.0 | −15.9 | 288 | – |
per 1 mol of | 70.0 | −15.9 | 288 | – |
per 1 mol of | 70.0 | −15.9 | 288 | – |
per 1 mol of | 70.0 | −15.9 | 288 | – |
Changes in aqueous solution (2)
- Reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid◆
ΔrG −51.8 kJ/mol K 1.19 × 109 pK −9.07
| 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 | −4.9 | −51.8 | 158 | – |
per 1 mol of | −2.5 | −25.9 | 79.0 | – |
per 1 mol of | −4.9 | −51.8 | 158 | – |
per 1 mol of | −4.9 | −51.8 | 158 | – |
per 1 mol of | −4.9 | −51.8 | 158 | – |
per 1 mol of | −4.9 | −51.8 | 158 | – |
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 |
|---|---|---|---|---|
| KClO (ai) | -359.4[1] | -320.0[1] | 146[1] | – |
| H2[PtCl6] (ai) | -668.2[1] | -482.7[1] | 219.7[1] | – |
| H2[PtCl6] (cr) 6 hydrate | -2371.1[1] | – | – | – |
* (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 |
|---|---|---|---|---|
| K2[PtCl6] (cr) | -1229.3[1] | -1078.5[1] | 333.9[1] | 205.60[1] |
| K2[PtCl6] (ai) | -1172.8[1] | -1049.2[1] | 424.7[1] | – |
| HClO2 (ao) | -51.9[1] | 5.9[1] | 188.3[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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°, -359.4 kJ · mol−1
- ^ ΔfG°, -320.0 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1
- ^ ΔfH°, -668.2 kJ · mol−1
- ^ ΔfG°, -482.7 kJ · mol−1
- ^ S°, 219.7 J · K−1 · mol−1
- ^ ΔfH°, -2371.1 kJ · mol−1
- ^ ΔfH°, -1229.3 kJ · mol−1
- ^ ΔfG°, -1078.5 kJ · mol−1
- ^ S°, 333.9 J · K−1 · mol−1
- ^ Cp°, 205.60 J · K−1 · mol−1
- ^ ΔfH°, -1172.8 kJ · mol−1
- ^ ΔfG°, -1049.2 kJ · mol−1
- ^ S°, 424.7 J · K−1 · mol−1
- ^ ΔfH°, -51.9 kJ · mol−1
- ^ ΔfG°, 5.9 kJ · mol−1
- ^ S°, 188.3 J · K−1 · mol−1
- ^ 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