2NaCl + AgNO3 + 2H+ 🔥→ NaNO2 + Na+ + Cl2↑ + Ag+ + H2O
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- Reaction of sodium chloride and silver(I) nitrate under acidic condition
- 2NaClSodium chloride + AgNO3Silver(I) nitrate + 2H+Hydrogen ionNaNO2Sodium nitrite + Na+Sodium ion + ↑ + Ag+Silver(I) ion + H2OWater🔥⟶
The reaction of sodium chloride, silver(I) nitrate, and hydrogen ion yields sodium nitrite, sodium ion, , 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
- 2NaClSodium chloride + AgNO3Silver(I) nitrate + 2H+Hydrogen ionNaNO2Sodium nitrite + Na+Sodium ion + ↑ + Ag+Silver(I) ion + H2OWater🔥⟶
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 | 2 | Reducing | Hardly oxidizable |
| AgNO3 | Silver(I) nitrate | 1 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 2 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaNO2 | Sodium nitrite | 1 | Reduced | – |
| Na+ | Sodium ion | 1 | – | – |
| 1 | Oxidized | – | ||
| Ag+ | Silver(I) ion | 1 | – | – |
| H2O | Water | 1 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 104.4 kJ/mol K 0.51 × 10−18 pK 18.29
| 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 | 151.2 | 104.4 | 156.5 | 371.3 |
per 1 mol of | 75.60 | 52.20 | 78.25 | 185.7 |
per 1 mol of | 151.2 | 104.4 | 156.5 | 371.3 |
per 1 mol of Hydrogen ion | 75.60 | 52.20 | 78.25 | 185.7 |
per 1 mol of | 151.2 | 104.4 | 156.5 | 371.3 |
per 1 mol of Sodium ion | 151.2 | 104.4 | 156.5 | 371.3 |
| 151.2 | 104.4 | 156.5 | 371.3 | |
per 1 mol of Silver(I) ion | 151.2 | 104.4 | 156.5 | 371.3 |
per 1 mol of | 151.2 | 104.4 | 156.5 | 371.3 |
Changes in standard condition (2)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 111.3 kJ/mol K 0.32 × 10−19 pK 19.50
| 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 | 127.8 | 111.3 | 54 | – |
per 1 mol of | 63.90 | 55.65 | 27 | – |
per 1 mol of | 127.8 | 111.3 | 54 | – |
per 1 mol of Hydrogen ion | 63.90 | 55.65 | 27 | – |
per 1 mol of | 127.8 | 111.3 | 54 | – |
per 1 mol of Sodium ion | 127.8 | 111.3 | 54 | – |
| 127.8 | 111.3 | 54 | – | |
per 1 mol of Silver(I) ion | 127.8 | 111.3 | 54 | – |
per 1 mol of | 127.8 | 111.3 | 54 | – |
Changes in standard condition (3)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 102.7 kJ/mol K 0.10 × 10−17 pK 17.99
| 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 | – | 102.7 | – | – |
per 1 mol of | – | 51.35 | – | – |
per 1 mol of | – | 102.7 | – | – |
per 1 mol of Hydrogen ion | – | 51.35 | – | – |
per 1 mol of | – | 102.7 | – | – |
per 1 mol of Sodium ion | – | 102.7 | – | – |
| – | 102.7 | – | – | |
per 1 mol of Silver(I) ion | – | 102.7 | – | – |
per 1 mol of | – | 102.7 | – | – |
Changes in standard condition (4)
- Reaction of sodium chloride and silver(I) nitrate under acidic condition◆
ΔrG 109.7 kJ/mol K 0.60 × 10−19 pK 19.22
| 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 | – | 109.7 | – | – |
per 1 mol of | – | 54.85 | – | – |
per 1 mol of | – | 109.7 | – | – |
per 1 mol of Hydrogen ion | – | 54.85 | – | – |
per 1 mol of | – | 109.7 | – | – |
per 1 mol of Sodium ion | – | 109.7 | – | – |
| – | 109.7 | – | – | |
per 1 mol of Silver(I) ion | – | 109.7 | – | – |
per 1 mol of | – | 109.7 | – | – |
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 |
|---|---|---|---|---|
| NaNO2 (cr) | -358.65[1] | -284.55[1] | 103.8[1] | – |
| NaNO2 (ai) | -344.8[1] | -294.1[1] | 182.0[1] | -51.0[1] |
| Na+ (g) | 609.358[1] | – | – | – |
| Na+ (ao) | -240.12[1] | -261.905[1] | 59.0[1] | 46.4[1] |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[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°, -358.65 kJ · mol−1
- ^ ΔfG°, -284.55 kJ · mol−1
- ^ S°, 103.8 J · K−1 · mol−1
- ^ ΔfH°, -344.8 kJ · mol−1
- ^ ΔfG°, -294.1 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ Cp°, -51.0 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°, 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°, 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