5NaCl + 11AgNO3 + 11H+ 🔥→ 5NaNO3 + 5HClO3 + 3N2↑ + 11Ag+ + 3H2O
Last updated:
- Reaction of sodium chloride and silver(I) nitrate under acidic condition
- 5NaClSodium chloride + 11AgNO3Silver(I) nitrate + 11H+Hydrogen ion5NaNO3Sodium nitrate + 5HClO3Chloric acid + 3↑ + 11Ag+Silver(I) ion + 3H2OWater🔥⟶
The reaction of sodium chloride, silver(I) nitrate, and hydrogen ion yields sodium nitrate, chloric acid, , 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
- 5NaClSodium chloride + 11AgNO3Silver(I) nitrate + 11H+Hydrogen ion5NaNO3Sodium nitrate + 5HClO3Chloric acid + 3↑ + 11Ag+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 | 5 | Reducing | Hardly oxidizable |
| AgNO3 | Silver(I) nitrate | 11 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 11 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO3 | Sodium nitrate | 5 | – | – |
| HClO3 | Chloric acid | 5 | Oxidized | – |
| 3 | Reduced | – | ||
| Ag+ | Silver(I) ion | 11 | – | – |
| H2O | Water | 3 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 572.72 kJ/mol K 0.46 × 10−100 pK 100.34
| 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 | 702.78 | 572.72 | 433.8 | – |
per 1 mol of | 140.56 | 114.54 | 86.76 | – |
per 1 mol of | 63.889 | 52.065 | 39.44 | – |
per 1 mol of Hydrogen ion | 63.889 | 52.065 | 39.44 | – |
per 1 mol of | 140.56 | 114.54 | 86.76 | – |
per 1 mol of | 140.56 | 114.54 | 86.76 | – |
| 234.26 | 190.91 | 144.6 | – | |
per 1 mol of Silver(I) ion | 63.889 | 52.065 | 39.44 | – |
per 1 mol of | 234.26 | 190.91 | 144.6 | – |
Changes in standard condition (2)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 554.35 kJ/mol K 0.76 × 10−97 pK 97.12
| 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 | – | 554.35 | – | – |
per 1 mol of | – | 110.87 | – | – |
per 1 mol of | – | 50.395 | – | – |
per 1 mol of Hydrogen ion | – | 50.395 | – | – |
per 1 mol of | – | 110.87 | – | – |
per 1 mol of | – | 110.87 | – | – |
| – | 184.78 | – | – | |
per 1 mol of Silver(I) ion | – | 50.395 | – | – |
per 1 mol of | – | 184.78 | – | – |
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 |
|---|---|---|---|---|
| NaNO3 (cr) | -467.85[1] | -367.00[1] | 116.52[1] | 92.88[1] |
| NaNO3 (ai) | -447.48[1] | -373.15[1] | 205.4[1] | -40.2[1] |
| HClO3 (ai) | -103.97[1] | -7.95[1] | 162.3[1] | – |
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[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] |
* (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°, -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°, -467.85 kJ · mol−1
- ^ ΔfG°, -367.00 kJ · mol−1
- ^ S°, 116.52 J · K−1 · mol−1
- ^ Cp°, 92.88 J · K−1 · mol−1
- ^ ΔfH°, -447.48 kJ · mol−1
- ^ ΔfG°, -373.15 kJ · mol−1
- ^ S°, 205.4 J · K−1 · mol−1
- ^ Cp°, -40.2 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 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