NaCl + 6AgNO3 + 7H+ 🔥→ Na+ + HClO3 + 6NO2↑ + 6Ag+ + 3H2O
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- Reaction of sodium chloride and silver(I) nitrate under acidic condition
- NaClSodium chloride + 6AgNO3Silver(I) nitrate + 7H+Hydrogen ionNa+Sodium ion + HClO3Chloric acid + 6NO2↑Nitrogen dioxide + 6Ag+Silver(I) ion + 3H2OWater🔥⟶
The reaction of sodium chloride, silver(I) nitrate, and hydrogen ion yields sodium ion, chloric acid, nitrogen dioxide, silver(I) ion, 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 chloride and silver(I) nitrate under acidic condition
- NaClSodium chloride + 6AgNO3Silver(I) nitrate + 7H+Hydrogen ionNa+Sodium ion + HClO3Chloric acid + 6NO2↑Nitrogen dioxide + 6Ag+Silver(I) ion + 3H2OWater🔥⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species under acidic condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of sodium chloride and silver(I) nitrate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaCl | Sodium chloride | 1 | Reducing | Hardly oxidizable |
| AgNO3 | Silver(I) nitrate | 6 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 7 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na+ | Sodium ion | 1 | – | – |
| HClO3 | Chloric acid | 1 | Oxidized | – |
| NO2 | Nitrogen dioxide | 6 | Reduced | – |
| Ag+ | Silver(I) ion | 6 | – | – |
| H2O | Water | 3 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 387.35 kJ/mol K 0.14 × 10−67 pK 67.86
| 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 | 649.04 | 387.35 | 876.8 | – |
per 1 mol of | 649.04 | 387.35 | 876.8 | – |
per 1 mol of | 108.17 | 64.558 | 146.1 | – |
per 1 mol of Hydrogen ion | 92.720 | 55.336 | 125.3 | – |
per 1 mol of Sodium ion | 649.04 | 387.35 | 876.8 | – |
per 1 mol of | 649.04 | 387.35 | 876.8 | – |
per 1 mol of | 108.17 | 64.558 | 146.1 | – |
per 1 mol of Silver(I) ion | 108.17 | 64.558 | 146.1 | – |
per 1 mol of | 216.35 | 129.12 | 292.3 | – |
Changes in standard condition (2)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 377.33 kJ/mol K 0.78 × 10−66 pK 66.11
| 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 | – | 377.33 | – | – |
per 1 mol of | – | 377.33 | – | – |
per 1 mol of | – | 62.888 | – | – |
per 1 mol of Hydrogen ion | – | 53.904 | – | – |
per 1 mol of Sodium ion | – | 377.33 | – | – |
per 1 mol of | – | 377.33 | – | – |
per 1 mol of | – | 62.888 | – | – |
per 1 mol of Silver(I) ion | – | 62.888 | – | – |
per 1 mol of | – | 125.78 | – | – |
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 |
|---|---|---|---|---|
| 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] |
| AgNO3 (cr) | -124.39[1] | -33.41[1] | 140.92[1] | 93.05[1] |
| AgNO3 (ai) | -101.80[1] | -34.16[1] | 219.2[1] | -64.9[1] |
| AgNO3 (ao) | – | -32.49[1] | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| Na+ (g) | 609.358[1] | – | – | – |
| Na+ (ao) | -240.12[1] | -261.905[1] | 59.0[1] | 46.4[1] |
| HClO3 (ai) | -103.97[1] | -7.95[1] | 162.3[1] | – |
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[1] |
| Ag+ (g) | 1021.73[1] | – | – | – |
| Ag+ (ao) | 105.579[1] | 77.107[1] | 72.68[1] | 21.8[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] |
* (g):Gas, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution, (cr):Crystalline solid, (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°, -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°, -124.39 kJ · mol−1
- ^ ΔfG°, -33.41 kJ · mol−1
- ^ S°, 140.92 J · K−1 · mol−1
- ^ Cp°, 93.05 J · K−1 · mol−1
- ^ ΔfH°, -101.80 kJ · mol−1
- ^ ΔfG°, -34.16 kJ · mol−1
- ^ S°, 219.2 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfG°, -32.49 kJ · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, 609.358 kJ · mol−1
- ^ ΔfH°, -240.12 kJ · mol−1
- ^ ΔfG°, -261.905 kJ · mol−1
- ^ S°, 59.0 J · K−1 · mol−1
- ^ Cp°, 46.4 J · K−1 · mol−1
- ^ ΔfH°, -103.97 kJ · mol−1
- ^ ΔfG°, -7.95 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1
- ^ ΔfH°, 33.18 kJ · mol−1
- ^ ΔfG°, 51.31 kJ · mol−1
- ^ S°, 240.06 J · K−1 · mol−1
- ^ Cp°, 37.20 J · K−1 · mol−1
- ^ ΔfH°, 1021.73 kJ · mol−1
- ^ ΔfH°, 105.579 kJ · mol−1
- ^ ΔfG°, 77.107 kJ · mol−1
- ^ S°, 72.68 J · K−1 · mol−1
- ^ Cp°, 21.8 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