2HCl + 5AgNO3 🔥→ 2ClO2 + 5Ag + 5NO2 + H2O
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- Reaction of hydrogen chloride and silver(I) nitrate
The reaction of hydrogen chloride and silver(I) nitrate yields chlorine dioxide, , nitrogen dioxide, 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 | 2 | Reducing | Hardly oxidizable |
| AgNO3 | Silver(I) nitrate | 5 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ClO2 | Chlorine dioxide | 2 | Oxidized | – |
| 5 | Reduced | – | ||
| NO2 | Nitrogen dioxide | 5 | Reduced | – |
| H2O | Water | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 618.1 kJ/mol K 0.52 × 10−108 pK 108.29
| 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 | 891.6 | 618.1 | 918.22 | −51.50 |
per 1 mol of | 445.8 | 309.1 | 459.11 | −25.75 |
per 1 mol of | 178.3 | 123.6 | 183.64 | −10.30 |
per 1 mol of | 445.8 | 309.1 | 459.11 | −25.75 |
| 178.3 | 123.6 | 183.64 | −10.30 | |
per 1 mol of | 178.3 | 123.6 | 183.64 | −10.30 |
per 1 mol of | 891.6 | 618.1 | 918.22 | −51.50 |
Changes in aqueous solution (1)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 693.7 kJ/mol K 0.29 × 10−121 pK 121.53
| 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 | 928.4 | 693.7 | 787.6 | 1069.3 |
per 1 mol of | 464.2 | 346.9 | 393.8 | 534.65 |
per 1 mol of | 185.7 | 138.7 | 157.5 | 213.86 |
per 1 mol of | 464.2 | 346.9 | 393.8 | 534.65 |
| 185.7 | 138.7 | 157.5 | 213.86 | |
per 1 mol of | 185.7 | 138.7 | 157.5 | 213.86 |
per 1 mol of | 928.4 | 693.7 | 787.6 | 1069.3 |
Changes in aqueous solution (2)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 692.9 kJ/mol K 0.41 × 10−121 pK 121.39
| 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 | 873.2 | 692.9 | 603.6 | – |
per 1 mol of | 436.6 | 346.4 | 301.8 | – |
per 1 mol of | 174.6 | 138.6 | 120.7 | – |
per 1 mol of | 436.6 | 346.4 | 301.8 | – |
| 174.6 | 138.6 | 120.7 | – | |
per 1 mol of | 174.6 | 138.6 | 120.7 | – |
per 1 mol of | 873.2 | 692.9 | 603.6 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 685.3 kJ/mol K 0.87 × 10−120 pK 120.06
| 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 | – | 685.3 | – | – |
per 1 mol of | – | 342.6 | – | – |
per 1 mol of | – | 137.1 | – | – |
per 1 mol of | – | 342.6 | – | – |
| – | 137.1 | – | – | |
per 1 mol of | – | 137.1 | – | – |
per 1 mol of | – | 685.3 | – | – |
Changes in aqueous solution (4)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 684.5 kJ/mol K 0.12 × 10−119 pK 119.92
| 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 | – | 684.5 | – | – |
per 1 mol of | – | 342.3 | – | – |
per 1 mol of | – | 136.9 | – | – |
per 1 mol of | – | 342.3 | – | – |
| – | 136.9 | – | – | |
per 1 mol of | – | 136.9 | – | – |
per 1 mol of | – | 684.5 | – | – |
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 |
|---|---|---|---|---|
| ClO2 (g) | 102.5[1] | 120.5[1] | 256.84[1] | 41.97[1] |
| ClO2 (ao) | 74.9[1] | 120.1[1] | 164.8[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] |
| NO2 (g) | 33.18[1] | 51.31[1] | 240.06[1] | 37.20[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°, 102.5 kJ · mol−1
- ^ ΔfG°, 120.5 kJ · mol−1
- ^ S°, 256.84 J · K−1 · mol−1
- ^ Cp°, 41.97 J · K−1 · mol−1
- ^ ΔfH°, 74.9 kJ · mol−1
- ^ ΔfG°, 120.1 kJ · mol−1
- ^ S°, 164.8 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°, 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°, -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