5NaClO + H4SiO4 → 3NaCl + Na2SiO3 + 2ClO2↑ + 2H2O
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- Reaction of sodium hypochlorite and silicic acid
- 5NaClOSodium hypochlorite + H4SiO4Silicic acid3NaClSodium chloride + Na2SiO3Sodium metasilicate + 2ClO2↑Chlorine dioxide + 2H2OWater⟶
The reaction of sodium hypochlorite and silicic acid yields sodium chloride, sodium metasilicate, chlorine dioxide, 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 sodium hypochlorite and silicic acid
- 5NaClOSodium hypochlorite + H4SiO4Silicic acid3NaClSodium chloride + Na2SiO3Sodium metasilicate + 2ClO2↑Chlorine dioxide + 2H2OWater⟶
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 sodium hypochlorite and silicic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaClO | Sodium hypochlorite | 5 | – | Self redoxing |
| H4SiO4 | Silicic acid | 1 | – | Acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaCl | Sodium chloride | 3 | Reduced | – |
| Na2SiO3 | Sodium metasilicate | 1 | – | – |
| ClO2 | Chlorine dioxide | 2 | Oxidized | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium hypochlorite and silicic 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 | 30.4 | – | – | – |
per 1 mol of | 6.08 | – | – | – |
per 1 mol of Silicic acid | 30.4 | – | – | – |
per 1 mol of | 10.1 | – | – | – |
per 1 mol of | 30.4 | – | – | – |
per 1 mol of | 15.2 | – | – | – |
per 1 mol of | 15.2 | – | – | – |
Changes in standard condition (2)
- Reaction of sodium hypochlorite and silicic 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 | −24.8 | – | – | – |
per 1 mol of | −4.96 | – | – | – |
per 1 mol of Silicic acid | −24.8 | – | – | – |
per 1 mol of | −8.27 | – | – | – |
per 1 mol of | −24.8 | – | – | – |
per 1 mol of | −12.4 | – | – | – |
per 1 mol of | −12.4 | – | – | – |
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 |
|---|---|---|---|---|
| NaClO (ai) | -347.3[1] | -298.7[1] | 100[1] | – |
| H4SiO4 (cr) | -1481.1[1] | -1332.9[1] | 192[1] | – |
| H4SiO4 (ao) | -1468.6[1] | -1316.6[1] | 180[1] | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (ao):Un-ionized aqueous solution
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 |
|---|---|---|---|---|
| NaCl (cr) | -411.153[1] | -384.138[1] | 72.13[1] | 50.50[1] |
| NaCl (g) | -176.65[1] | -196.66[1] | 229.81[1] | 35.77[1] |
| NaCl (ai) | -407.27[1] | -393.133[1] | 115.5[1] | -90.0[1] |
| Na2SiO3 (cr) | -1554.90[1] | -1462.80[1] | 113.85[1] | – |
| Na2SiO3 (vit) | -1540.1[1] | – | – | – |
| Na2SiO3 (aq) | -1586.2[1] | – | – | – |
| Na2SiO3 (cr) 5 hydrate | -3048.5[1] | – | – | – |
| Na2SiO3 (cr) 9 hydrate | -4228.8[1] | – | – | – |
| ClO2 (g) | 102.5[1] | 120.5[1] | 256.84[1] | 41.97[1] |
| ClO2 (ao) | 74.9[1] | 120.1[1] | 164.8[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, (vit):Vitreous liquid, (aq):Aqueous solution, (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°, -347.3 kJ · mol−1
- ^ ΔfG°, -298.7 kJ · mol−1
- ^ S°, 100. J · K−1 · mol−1
- ^ ΔfH°, -1481.1 kJ · mol−1
- ^ ΔfG°, -1332.9 kJ · mol−1
- ^ S°, 192. J · K−1 · mol−1
- ^ ΔfH°, -1468.6 kJ · mol−1
- ^ ΔfG°, -1316.6 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ ΔfH°, -411.153 kJ · mol−1
- ^ ΔfG°, -384.138 kJ · mol−1
- ^ S°, 72.13 J · K−1 · mol−1
- ^ Cp°, 50.50 J · K−1 · mol−1
- ^ ΔfH°, -176.65 kJ · mol−1
- ^ ΔfG°, -196.66 kJ · mol−1
- ^ S°, 229.81 J · K−1 · mol−1
- ^ Cp°, 35.77 J · K−1 · mol−1
- ^ ΔfH°, -407.27 kJ · mol−1
- ^ ΔfG°, -393.133 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ Cp°, -90.0 J · K−1 · mol−1
- ^ ΔfH°, -1554.90 kJ · mol−1
- ^ ΔfG°, -1462.80 kJ · mol−1
- ^ S°, 113.85 J · K−1 · mol−1
- ^ ΔfH°, -1540.1 kJ · mol−1
- ^ ΔfH°, -1586.2 kJ · mol−1
- ^ ΔfH°, -3048.5 kJ · mol−1
- ^ ΔfH°, -4228.8 kJ · mol−1
- ^ ΔfH°, 102.5 kJ · mol−1
- ^ ΔfG°, 120.5 kJ · mol−1
- ^ S°, 256.84 J · K−1 · mol−1
- ^ Cp°, 41.97 J · K−1 · mol−1
- ^ ΔfH°, 74.9 kJ · mol−1
- ^ ΔfG°, 120.1 kJ · mol−1
- ^ S°, 164.8 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