4KClO + 2H2SeO4 → 2K2SeO4 + 2Cl2↑ + O2↑ + 2H2O
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- Reaction of potassium hypochlorite and selenic acid
The reaction of potassium hypochlorite and selenic acid yields potassium selenate, , , and water (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 selenic 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 selenic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO | Potassium hypochlorite | 4 | Oxidizing | Self redoxing |
| H2SeO4 | Selenic acid | 2 | – | Acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2SeO4 | Potassium selenate | 2 | – | – |
| 2 | Reduced | – | ||
| 1 | – | – | ||
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hypochlorite and selenic acid
| 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 | −281.3 | – | – | – |
per 1 mol of | −70.33 | – | – | – |
per 1 mol of | −140.7 | – | – | – |
per 1 mol of | −140.7 | – | – | – |
| −140.7 | – | – | – | |
| −281.3 | – | – | – | |
per 1 mol of | −140.7 | – | – | – |
Changes in aqueous solution (2)
- Reaction of potassium hypochlorite and selenic acid
| 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 | −293.0 | – | – | – |
per 1 mol of | −73.25 | – | – | – |
per 1 mol of | −146.5 | – | – | – |
per 1 mol of | −146.5 | – | – | – |
| −146.5 | – | – | – | |
| −293.0 | – | – | – | |
per 1 mol of | −146.5 | – | – | – |
Changes in aqueous solution (3)
- Reaction of potassium hypochlorite and selenic acid
| 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 | −328.1 | – | – | – |
per 1 mol of | −82.03 | – | – | – |
per 1 mol of | −164.1 | – | – | – |
per 1 mol of | −164.1 | – | – | – |
| −164.1 | – | – | – | |
| −328.1 | – | – | – | |
per 1 mol of | −164.1 | – | – | – |
Changes in aqueous solution (4)
- Reaction of potassium hypochlorite and selenic acid
| 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 | −339.8 | – | – | – |
per 1 mol of | −84.95 | – | – | – |
per 1 mol of | −169.9 | – | – | – |
per 1 mol of | −169.9 | – | – | – |
| −169.9 | – | – | – | |
| −339.8 | – | – | – | |
per 1 mol of | −169.9 | – | – | – |
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] | – |
| H2SeO4 (cr) | -530.1[1] | – | – | – |
| H2SeO4 (cr) 1 hydrate | -840.6[1] | – | – | – |
| H2SeO4 (l) 1 hydrate | -820.5[1] | – | – | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| K2SeO4 (cr) | -1110.02[1] | -1002.8[1] | 222[1] | – |
| K2SeO4 (ai) | -1103.7[1] | -1007.9[1] | 259.0[1] | – |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| (g) | 0[1] | 0[1] | 205.138[1] | 29.355[1] |
| (ao) | -11.7[1] | 16.4[1] | 110.9[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, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -530.1 kJ · mol−1
- ^ ΔfH°, -840.6 kJ · mol−1
- ^ ΔfH°, -820.5 kJ · mol−1
- ^ ΔfH°, -1110.02 kJ · mol−1
- ^ ΔfG°, -1002.8 kJ · mol−1
- ^ S°, 222. J · K−1 · mol−1
- ^ ΔfH°, -1103.7 kJ · mol−1
- ^ ΔfG°, -1007.9 kJ · mol−1
- ^ S°, 259.0 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 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