13HCl + 8AgNO3 🔥→ 5HClO4 + 4N2 + 8AgCl + 4H2O
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- Reaction of hydrogen chloride and silver(I) nitrate
The reaction of hydrogen chloride and silver(I) nitrate yields perchloric acid, , silver(I) chloride, 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 | 13 | Reducing | Hardly oxidizable |
| AgNO3 | Silver(I) nitrate | 8 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO4 | Perchloric acid | 5 | Oxidized | – |
| 4 | Reduced | – | ||
| AgCl | Silver(I) chloride | 8 | – | – |
| H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and silver(I) nitrate
| 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 | −167.65 | – | – | – |
per 1 mol of | −12.896 | – | – | – |
per 1 mol of | −20.956 | – | – | – |
per 1 mol of | −33.530 | – | – | – |
| −41.913 | – | – | – | |
per 1 mol of | −20.956 | – | – | – |
per 1 mol of | −41.913 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 555.17 kJ/mol K 0.55 × 10−97 pK 97.26
| 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 | 704.86 | 555.17 | 502.4 | – |
per 1 mol of | 54.220 | 42.705 | 38.65 | – |
per 1 mol of | 88.108 | 69.396 | 62.80 | – |
per 1 mol of | 140.97 | 111.03 | 100.5 | – |
| 176.22 | 138.79 | 125.6 | – | |
per 1 mol of | 88.108 | 69.396 | 62.80 | – |
per 1 mol of | 176.22 | 138.79 | 125.6 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 405.7 kJ/mol K 0.84 × 10−71 pK 71.08
| 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 | 615.1 | 405.7 | 700.0 | – |
per 1 mol of | 47.32 | 31.21 | 53.85 | – |
per 1 mol of | 76.89 | 50.71 | 87.50 | – |
per 1 mol of | 123.0 | 81.14 | 140.0 | – |
| 153.8 | 101.4 | 175.0 | – | |
per 1 mol of | 76.89 | 50.71 | 87.50 | – |
per 1 mol of | 153.8 | 101.4 | 175.0 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 541.81 kJ/mol K 0.12 × 10−94 pK 94.92
| 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 | – | 541.81 | – | – |
per 1 mol of | – | 41.678 | – | – |
per 1 mol of | – | 67.726 | – | – |
per 1 mol of | – | 108.36 | – | – |
| – | 135.45 | – | – | |
per 1 mol of | – | 67.726 | – | – |
per 1 mol of | – | 135.45 | – | – |
Changes in aqueous solution (4)
- Reaction of hydrogen chloride and silver(I) nitrate◆
ΔrG 392.4 kJ/mol K 0.18 × 10−68 pK 68.75
| 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 | – | 392.4 | – | – |
per 1 mol of | – | 30.18 | – | – |
per 1 mol of | – | 49.05 | – | – |
per 1 mol of | – | 78.48 | – | – |
| – | 98.10 | – | – | |
per 1 mol of | – | 49.05 | – | – |
per 1 mol of | – | 98.10 | – | – |
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 |
|---|---|---|---|---|
| HClO4 (l) | -40.58[1] | – | – | – |
| HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
| HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
| HClO4 (l) 2 hydrate | -677.98[1] | – | – | – |
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
| AgCl (cr) | -127.068[1] | -109.789[1] | 96.2[1] | 50.79[1] |
| AgCl (g) | – | – | 245.92[1] | 35.86[1] |
| AgCl (ai) | -61.580[1] | -54.120[1] | 129.3[1] | -114.6[1] |
| AgCl (ao) | -72.8[1] | -72.8[1] | 154.0[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] |
* (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution
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°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · 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°, -127.068 kJ · mol−1
- ^ ΔfG°, -109.789 kJ · mol−1
- ^ S°, 96.2 J · K−1 · mol−1
- ^ Cp°, 50.79 J · K−1 · mol−1
- ^ S°, 245.92 J · K−1 · mol−1
- ^ Cp°, 35.86 J · K−1 · mol−1
- ^ ΔfH°, -61.580 kJ · mol−1
- ^ ΔfG°, -54.120 kJ · mol−1
- ^ S°, 129.3 J · K−1 · mol−1
- ^ Cp°, -114.6 J · K−1 · mol−1
- ^ ΔfH°, -72.8 kJ · mol−1
- ^ ΔfG°, -72.8 kJ · mol−1
- ^ S°, 154.0 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