3NaClO + 2AgOH 🔥→ NaClO3 + Na2O + 2AgCl + H2O
Last updated:
- Reaction of sodium hypochlorite and silver(I) hydroxide
- 3NaClOSodium hypochlorite + 2AgOHSilver(I) hydroxideNaClO3Sodium chlorate + Na2OSodium oxide + 2AgClSilver(I) chloride + H2OWater🔥⟶
The reaction of sodium hypochlorite and silver(I) hydroxide yields sodium chlorate, sodium oxide, silver(I) chloride, 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 silver(I) hydroxide
- 3NaClOSodium hypochlorite + 2AgOHSilver(I) hydroxideNaClO3Sodium chlorate + Na2OSodium oxide + 2AgClSilver(I) chloride + H2OWater🔥⟶
General equation
- Reaction of self redoxing species and base
- Self-redoxing speciesSelf redox agent + BaseNon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of sodium hypochlorite and silver(I) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaClO | Sodium hypochlorite | 3 | – | Self redoxing |
| AgOH | Silver(I) hydroxide | 2 | – | Base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaClO3 | Sodium chlorate | 1 | Oxidized | – |
| Na2O | Sodium oxide | 1 | – | – |
| AgCl | Silver(I) chloride | 2 | Reduced | – |
| H2O | Water | 1 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium hypochlorite and silver(I) hydroxide◆
ΔrG 65.7 kJ/mol K 0.31 × 10−11 pK 11.51
| 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 | 123.4 | 65.7 | 201 | – |
per 1 mol of | 41.13 | 21.9 | 67.0 | – |
per 1 mol of Silver(I) hydroxide | 61.70 | 32.9 | 101 | – |
per 1 mol of | 123.4 | 65.7 | 201 | – |
per 1 mol of | 123.4 | 65.7 | 201 | – |
per 1 mol of | 61.70 | 32.9 | 101 | – |
per 1 mol of | 123.4 | 65.7 | 201 | – |
Changes in aqueous solution (2)
- Reaction of sodium hypochlorite and silver(I) hydroxide◆
ΔrG 28.3 kJ/mol K 0.11 × 10−4 pK 4.96
| 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 | 101.0 | 28.3 | 250 | – |
per 1 mol of | 33.67 | 9.43 | 83.3 | – |
per 1 mol of Silver(I) hydroxide | 50.50 | 14.2 | 125 | – |
per 1 mol of | 101.0 | 28.3 | 250 | – |
per 1 mol of | 101.0 | 28.3 | 250 | – |
per 1 mol of | 50.50 | 14.2 | 125 | – |
per 1 mol of | 101.0 | 28.3 | 250 | – |
Changes in aqueous solution (3)
- Reaction of sodium hypochlorite and silver(I) hydroxide◆
ΔrG 89.4 kJ/mol K 0.22 × 10−15 pK 15.66
| 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 | – | 89.4 | – | – |
per 1 mol of | – | 29.8 | – | – |
per 1 mol of Silver(I) hydroxide | – | 44.7 | – | – |
per 1 mol of | – | 89.4 | – | – |
per 1 mol of | – | 89.4 | – | – |
per 1 mol of | – | 44.7 | – | – |
per 1 mol of | – | 89.4 | – | – |
Changes in aqueous solution (4)
- Reaction of sodium hypochlorite and silver(I) hydroxide◆
ΔrG 52.1 kJ/mol K 0.75 × 10−9 pK 9.13
| 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 | – | 52.1 | – | – |
per 1 mol of | – | 17.4 | – | – |
per 1 mol of Silver(I) hydroxide | – | 26.1 | – | – |
per 1 mol of | – | 52.1 | – | – |
per 1 mol of | – | 52.1 | – | – |
per 1 mol of | – | 26.1 | – | – |
per 1 mol of | – | 52.1 | – | – |
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] | – |
| AgOH (ai) | -124.415[1] | -80.137[1] | 61.92[1] | -126.8[1] |
| AgOH (ao) | – | -92.0[1] | – | – |
* (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| NaClO3 (cr) | -365.774[1] | -262.259[1] | 123.4[1] | – |
| NaClO3 (ai) | -344.09[1] | -269.84[1] | 221.3[1] | – |
| Na2O (cr) | -414.22[1] | -375.46[1] | 75.06[1] | 69.12[1] |
| Na2O (g) | -35.6[1] | -52.3[1] | 261.2[1] | 55.2[1] |
| AgCl (cr) | -127.068[1] | -109.789[1] | 96.2[1] | 50.79[1] |
| AgCl (g) | – | – | 245.92[1] | 35.86[1] |
| AgCl (ai) | -61.580[1] | -54.120[1] | 129.3[1] | -114.6[1] |
| AgCl (ao) | -72.8[1] | -72.8[1] | 154.0[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°, -347.3 kJ · mol−1
- ^ ΔfG°, -298.7 kJ · mol−1
- ^ S°, 100. J · K−1 · mol−1
- ^ ΔfH°, -124.415 kJ · mol−1
- ^ ΔfG°, -80.137 kJ · mol−1
- ^ S°, 61.92 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfG°, -92.0 kJ · mol−1
- ^ ΔfH°, -365.774 kJ · mol−1
- ^ ΔfG°, -262.259 kJ · mol−1
- ^ S°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, -344.09 kJ · mol−1
- ^ ΔfG°, -269.84 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ ΔfH°, -414.22 kJ · mol−1
- ^ ΔfG°, -375.46 kJ · mol−1
- ^ S°, 75.06 J · K−1 · mol−1
- ^ Cp°, 69.12 J · K−1 · mol−1
- ^ ΔfH°, -35.6 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 261.2 J · K−1 · mol−1
- ^ Cp°, 55.2 J · K−1 · mol−1
- ^ ΔfH°, -127.068 kJ · mol−1
- ^ ΔfG°, -109.789 kJ · mol−1
- ^ S°, 96.2 J · K−1 · mol−1
- ^ Cp°, 50.79 J · K−1 · mol−1
- ^ S°, 245.92 J · K−1 · mol−1
- ^ Cp°, 35.86 J · K−1 · mol−1
- ^ ΔfH°, -61.580 kJ · mol−1
- ^ ΔfG°, -54.120 kJ · mol−1
- ^ S°, 129.3 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1
- ^ ΔfH°, -72.8 kJ · mol−1
- ^ ΔfG°, -72.8 kJ · mol−1
- ^ S°, 154.0 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