8KClO + 3H2[PtCl6] → 2KClO4 + 3K2[PtCl6] + 6HCl↑
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The reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid yields potassium perchlorate, potassium hexachloridoplatinate(IV), 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 | 8 | Oxidizing | Self redoxing |
| H2[PtCl6] | Hexachloridoplatinic(IV) acid | 3 | – | Acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO4 | Potassium perchlorate | 2 | – | – |
| K2[PtCl6] | Potassium hexachloridoplatinate(IV) | 3 | Reduced | – |
| HCl | Hydrogen chloride | 6 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid◆
ΔrG −294.9 kJ/mol K 4.62 × 1051 pK −51.66
| 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 | 44.1 | −294.9 | 1137 | – |
per 1 mol of | 5.51 | −36.86 | 142.1 | – |
per 1 mol of | 14.7 | −98.30 | 379.0 | – |
per 1 mol of | 22.1 | −147.4 | 568.5 | – |
per 1 mol of | 14.7 | −98.30 | 379.0 | – |
per 1 mol of | 7.35 | −49.15 | 189.5 | – |
Changes in aqueous solution (2)
- Reaction of potassium hypochlorite and hexachloridoplatinic(IV) acid◆
ΔrG −510.4 kJ/mol K 2.62 × 1089 pK −89.42
| 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 | −405.0 | −510.4 | 355 | – |
per 1 mol of | −50.63 | −63.80 | 44.4 | – |
per 1 mol of | −135.0 | −170.1 | 118 | – |
per 1 mol of | −202.5 | −255.2 | 178 | – |
per 1 mol of | −135.0 | −170.1 | 118 | – |
per 1 mol of | −67.50 | −85.07 | 59.2 | – |
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 |
|---|---|---|---|---|
| KClO4 (cr) | -432.75[1] | -303.09[1] | 151.0[1] | 112.38[1] |
| KClO4 (ai) | -381.71[1] | -291.79[1] | 284.5[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] | – |
| 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, (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°, -432.75 kJ · mol−1
- ^ ΔfG°, -303.09 kJ · mol−1
- ^ S°, 151.0 J · K−1 · mol−1
- ^ Cp°, 112.38 J · K−1 · mol−1
- ^ ΔfH°, -381.71 kJ · mol−1
- ^ ΔfG°, -291.79 kJ · mol−1
- ^ S°, 284.5 J · K−1 · 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°, -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