4HCl + Cd(NO3)2 🔥→ Cl2 + N2O4 + CdCl2 + 2H2O
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- Reaction of hydrogen chloride and cadmium nitrate
The reaction of hydrogen chloride and cadmium nitrate yields , dinitrogen tetraoxide, cadmium 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 cadmium 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 cadmium nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCl | Hydrogen chloride | 4 | Reducing | Hardly oxidizable |
| Cd(NO3)2 | Cadmium nitrate | 1 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Oxidized | – | ||
| N2O4 | Dinitrogen tetraoxide | 1 | Reduced | – |
| CdCl2 | Cadmium chloride | 1 | – | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and cadmium 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 | −157.12 | – | – | – |
per 1 mol of | −39.280 | – | – | – |
per 1 mol of | −157.12 | – | – | – |
| −157.12 | – | – | – | |
per 1 mol of | −157.12 | – | – | – |
per 1 mol of | −157.12 | – | – | – |
per 1 mol of | −78.560 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen chloride and cadmium nitrate◆
ΔrG 108.24 kJ/mol K 0.11 × 10−18 pK 18.96
| 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 | 157.90 | 108.24 | 166.1 | – |
per 1 mol of | 39.475 | 27.060 | 41.52 | – |
per 1 mol of | 157.90 | 108.24 | 166.1 | – |
| 157.90 | 108.24 | 166.1 | – | |
per 1 mol of | 157.90 | 108.24 | 166.1 | – |
per 1 mol of | 157.90 | 108.24 | 166.1 | – |
per 1 mol of | 78.950 | 54.120 | 83.05 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen chloride and cadmium nitrate◆
ΔrG 89.01 kJ/mol K 0.25 × 10−15 pK 15.59
| 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 | 163.1 | 89.01 | 248.2 | – |
per 1 mol of | 40.77 | 22.25 | 62.05 | – |
per 1 mol of | 163.1 | 89.01 | 248.2 | – |
| 163.1 | 89.01 | 248.2 | – | |
per 1 mol of | 163.1 | 89.01 | 248.2 | – |
per 1 mol of | 163.1 | 89.01 | 248.2 | – |
per 1 mol of | 81.55 | 44.51 | 124.1 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen chloride and cadmium nitrate◆
ΔrG 115.18 kJ/mol K 0.66 × 10−20 pK 20.18
| 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 | 134.5 | 115.18 | 64 | – |
per 1 mol of | 33.63 | 28.795 | 16 | – |
per 1 mol of | 134.5 | 115.18 | 64 | – |
| 134.5 | 115.18 | 64 | – | |
per 1 mol of | 134.5 | 115.18 | 64 | – |
per 1 mol of | 134.5 | 115.18 | 64 | – |
per 1 mol of | 67.25 | 57.590 | 32 | – |
Changes in aqueous solution (4)
- Reaction of hydrogen chloride and cadmium nitrate◆
ΔrG 95.95 kJ/mol K 0.15 × 10−16 pK 16.81
| 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 | 139.7 | 95.95 | 146 | – |
per 1 mol of | 34.92 | 23.99 | 36.5 | – |
per 1 mol of | 139.7 | 95.95 | 146 | – |
| 139.7 | 95.95 | 146 | – | |
per 1 mol of | 139.7 | 95.95 | 146 | – |
per 1 mol of | 139.7 | 95.95 | 146 | – |
per 1 mol of | 69.85 | 47.98 | 73.0 | – |
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] |
| Cd(NO3)2 (cr) | -456.31[1] | – | – | – |
| Cd(NO3)2 (ai) | -490.62[1] | -300.11[1] | 219.7[1] | – |
| Cd(NO3)2 (cr) 2 hydrate | -1055.62[1] | – | – | – |
| Cd(NO3)2 (cr) 4 hydrate | -1648.96[1] | – | – | – |
* (g):Gas, (ai):Ionized aqueous solution, (cr):Crystalline solid
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] | – |
| 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] |
| CdCl2 (cr) | -391.50[1] | -343.93[1] | 115.27[1] | 74.68[1] |
| CdCl2 (ai) | -410.20[1] | -340.068[1] | 39.7[1] | – |
| CdCl2 (ao) | -405.0[1] | -359.29[1] | 121.8[1] | – |
| CdCl2 (cr) 1 hydrate | -688.44[1] | -586.975[1] | 167.8[1] | – |
| CdCl2 (cr) 2.5 hydrate | -1131.94[1] | -943.939[1] | 227.2[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, (l):Liquid, (cr):Crystalline solid, (ai):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°, -456.31 kJ · mol−1
- ^ ΔfH°, -490.62 kJ · mol−1
- ^ ΔfG°, -300.11 kJ · mol−1
- ^ S°, 219.7 J · K−1 · mol−1
- ^ ΔfH°, -1055.62 kJ · mol−1
- ^ ΔfH°, -1648.96 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°, -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°, -391.50 kJ · mol−1
- ^ ΔfG°, -343.93 kJ · mol−1
- ^ S°, 115.27 J · K−1 · mol−1
- ^ Cp°, 74.68 J · K−1 · mol−1
- ^ ΔfH°, -410.20 kJ · mol−1
- ^ ΔfG°, -340.068 kJ · mol−1
- ^ S°, 39.7 J · K−1 · mol−1
- ^ ΔfH°, -405.0 kJ · mol−1
- ^ ΔfG°, -359.29 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -688.44 kJ · mol−1
- ^ ΔfG°, -586.975 kJ · mol−1
- ^ S°, 167.8 J · K−1 · mol−1
- ^ ΔfH°, -1131.94 kJ · mol−1
- ^ ΔfG°, -943.939 kJ · mol−1
- ^ S°, 227.2 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