9H2 + Cd(NO3)2 → Cd + 2NH3 + 6H2O
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- Reaction of and cadmium nitrate
The reaction of and cadmium nitrate yields , ammonia, 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 and cadmium nitrate
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and cadmium nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 9 | Reducing | Reducing | ||
| Cd(NO3)2 | Cadmium nitrate | 1 | Oxidizing | Oxidizing |
Products
Thermodynamic changes
Changes in standard condition (1)
- Reaction of 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 | −1350.89 | – | – | – |
| −150.099 | – | – | – | |
per 1 mol of | −1350.89 | – | – | – |
| −1350.89 | – | – | – | |
per 1 mol of | −675.445 | – | – | – |
per 1 mol of | −225.148 | – | – | – |
Changes in standard condition (2)
- Reaction of 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 | −1351.48 | – | – | – |
| −150.164 | – | – | – | |
per 1 mol of | −1351.48 | – | – | – |
| −1351.48 | – | – | – | |
per 1 mol of | −675.740 | – | – | – |
per 1 mol of | −225.247 | – | – | – |
Changes in aqueous solution (1)
- Reaction of and cadmium nitrate◆
ΔrG −1314.0 kJ/mol K 1.60 × 10230 pK −230.20
| 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 | −1278.8 | −1314.0 | −4557 | – |
| −142.09 | −146.00 | −506.3 | – | |
per 1 mol of | −1278.8 | −1314.0 | −4557 | – |
| −1278.8 | −1314.0 | −4557 | – | |
per 1 mol of | −639.40 | −657.00 | −2279 | – |
per 1 mol of | −213.13 | −219.00 | −759.5 | – |
Changes in aqueous solution (2)
- Reaction of and cadmium nitrate◆
ΔrG −1334.1 kJ/mol K 5.30 × 10233 pK −233.72
| 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 | −1347.1 | −1334.1 | −4719 | – |
| −149.68 | −148.23 | −524.3 | – | |
per 1 mol of | −1347.1 | −1334.1 | −4719 | – |
| −1347.1 | −1334.1 | −4719 | – | |
per 1 mol of | −673.55 | −667.05 | −2360 | – |
per 1 mol of | −224.52 | −222.35 | −786.5 | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[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, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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 |
|---|---|---|---|---|
| (cr) γ | 0[1] | 0[1] | 51.76[1] | 25.98[1] |
| (cr) α | -0.59[1] | -0.59[1] | 51.76[1] | – |
| (g) | 112.01[1] | 77.41[1] | 167.746[1] | 20.786[1] |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[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, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 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°, 51.76 J · K−1 · mol−1
- ^ Cp°, 25.98 J · K−1 · mol−1
- ^ ΔfH°, -0.59 kJ · mol−1
- ^ ΔfG°, -0.59 kJ · mol−1
- ^ S°, 51.76 J · K−1 · mol−1
- ^ ΔfH°, 112.01 kJ · mol−1
- ^ ΔfG°, 77.41 kJ · mol−1
- ^ S°, 167.746 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 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