4HCl + 2AgNO3 🔥→ 2Cl2 + 2Ag + N2O4 + 2H2O
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- Reaction of hydrogen chloride and silver(I) nitrate
The reaction of hydrogen chloride and silver(I) nitrate yields , , dinitrogen tetraoxide, 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 hydrogen chloride and silver(I) nitrate
General equation
- Reaction of hardly oxidizable species and oxidizing species
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen chloride and silver(I) nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCl | Hydrogen chloride | 4 | Reducing | Hardly oxidizable |
| AgNO3 | Silver(I) nitrate | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Oxidized | – | ||
| 2 | Reduced | – | ||
| N2O4 | Dinitrogen tetraoxide | 1 | Reduced | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 71.30 kJ/mol K 0.32 × 10−12 pK 12.49
| 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 | 26.85 | 71.30 | −149.2 | 109.2 |
per 1 mol of | 6.713 | 17.82 | −37.30 | 27.30 |
per 1 mol of | 13.43 | 35.65 | −74.60 | 54.60 |
| 13.43 | 35.65 | −74.60 | 54.60 | |
| 13.43 | 35.65 | −74.60 | 54.60 | |
per 1 mol of | 26.85 | 71.30 | −149.2 | 109.2 |
per 1 mol of | 13.43 | 35.65 | −74.60 | 54.60 |
Changes in aqueous solution (1)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 216.51 kJ/mol K 0.12 × 10−37 pK 37.93
| 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 | 281.08 | 216.51 | 215.9 | 1087.2 |
per 1 mol of | 70.270 | 54.127 | 53.98 | 271.80 |
per 1 mol of | 140.54 | 108.25 | 108.0 | 543.60 |
| 140.54 | 108.25 | 108.0 | 543.60 | |
| 140.54 | 108.25 | 108.0 | 543.60 | |
per 1 mol of | 281.08 | 216.51 | 215.9 | 1087.2 |
per 1 mol of | 140.54 | 108.25 | 108.0 | 543.60 |
Changes in aqueous solution (2)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 230.39 kJ/mol K 0.43 × 10−40 pK 40.36
| 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 | 234.3 | 230.39 | 12 | – |
per 1 mol of | 58.58 | 57.597 | 3.0 | – |
per 1 mol of | 117.2 | 115.19 | 6.0 | – |
| 117.2 | 115.19 | 6.0 | – | |
| 117.2 | 115.19 | 6.0 | – | |
per 1 mol of | 234.3 | 230.39 | 12 | – |
per 1 mol of | 117.2 | 115.19 | 6.0 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 213.17 kJ/mol K 0.45 × 10−37 pK 37.35
| 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 | – | 213.17 | – | – |
per 1 mol of | – | 53.292 | – | – |
per 1 mol of | – | 106.58 | – | – |
| – | 106.58 | – | – | |
| – | 106.58 | – | – | |
per 1 mol of | – | 213.17 | – | – |
per 1 mol of | – | 106.58 | – | – |
Changes in aqueous solution (4)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 227.05 kJ/mol K 0.17 × 10−39 pK 39.78
| 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 | – | 227.05 | – | – |
per 1 mol of | – | 56.763 | – | – |
per 1 mol of | – | 113.53 | – | – |
| – | 113.53 | – | – | |
| – | 113.53 | – | – | |
per 1 mol of | – | 227.05 | – | – |
per 1 mol of | – | 113.53 | – | – |
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 |
|---|---|---|---|---|
| HCl (g) | -92.307[1] | -95.299[1] | 186.908[1] | 29.12[1] |
| HCl (ai) | -167.159[1] | -131.228[1] | 56.5[1] | -136.4[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] | – | – |
* (g):Gas, (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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| (cr) | 0[1] | 0[1] | 42.55[1] | 25.351[1] |
| (g) | 284.55[1] | 245.65[1] | 172.997[1] | 20.786[1] |
| N2O4 (l) | -19.50[1] | 97.54[1] | 209.2[1] | 142.7[1] |
| N2O4 (g) | 9.16[1] | 97.89[1] | 304.29[1] | 77.28[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, (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°, -92.307 kJ · mol−1
- ^ ΔfG°, -95.299 kJ · mol−1
- ^ S°, 186.908 J · K−1 · mol−1
- ^ Cp°, 29.12 J · K−1 · mol−1
- ^ ΔfH°, -167.159 kJ · mol−1
- ^ ΔfG°, -131.228 kJ · mol−1
- ^ S°, 56.5 J · K−1 · mol−1
- ^ Cp°, -136.4 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°, 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 42.55 J · K−1 · mol−1
- ^ Cp°, 25.351 J · K−1 · mol−1
- ^ ΔfH°, 284.55 kJ · mol−1
- ^ ΔfG°, 245.65 kJ · mol−1
- ^ S°, 172.997 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -19.50 kJ · mol−1
- ^ ΔfG°, 97.54 kJ · mol−1
- ^ S°, 209.2 J · K−1 · mol−1
- ^ Cp°, 142.7 J · K−1 · mol−1
- ^ ΔfH°, 9.16 kJ · mol−1
- ^ ΔfG°, 97.89 kJ · mol−1
- ^ S°, 304.29 J · K−1 · mol−1
- ^ Cp°, 77.28 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