9H2 + Zn(NO3)2 → Zn + 2NH3 + 6H2O
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- Reaction of and zinc nitrate
The reaction of and zinc 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 zinc 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 zinc nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 9 | Reducing | Reducing | ||
| Zn(NO3)2 | Zinc nitrate | 1 | Oxidizing | Oxidizing |
Products
Thermodynamic changes
Changes in standard condition
- Reaction of and zinc 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 | −1323.5 | – | – | – |
| −147.06 | – | – | – | |
per 1 mol of | −1323.5 | – | – | – |
| −1323.5 | – | – | – | |
per 1 mol of | −661.75 | – | – | – |
per 1 mol of | −220.58 | – | – | – |
Changes in aqueous solution (1)
- Reaction of and zinc nitrate◆
ΔrG −1244.5 kJ/mol K 1.06 × 10218 pK −218.03
| 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 | −1200.8 | −1244.5 | −4528 | – |
| −133.42 | −138.28 | −503.1 | – | |
per 1 mol of | −1200.8 | −1244.5 | −4528 | – |
| −1200.8 | −1244.5 | −4528 | – | |
per 1 mol of | −600.40 | −622.25 | −2264 | – |
per 1 mol of | −200.13 | −207.42 | −754.7 | – |
Changes in aqueous solution (2)
- Reaction of and zinc nitrate◆
ΔrG −1264.6 kJ/mol K 3.53 × 10221 pK −221.55
| 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 | −1269.2 | −1264.6 | −4690 | – |
| −141.02 | −140.51 | −521.1 | – | |
per 1 mol of | −1269.2 | −1264.6 | −4690 | – |
| −1269.2 | −1264.6 | −4690 | – | |
per 1 mol of | −634.60 | −632.30 | −2345 | – |
per 1 mol of | −211.53 | −210.77 | −781.7 | – |
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] | – |
| Zn(NO3)2 (cr) | -483.7[1] | – | – | – |
| Zn(NO3)2 (ai) | -568.61[1] | -369.57[1] | 180.7[1] | -126[1] |
| Zn(NO3)2 (cr) 1 hydrate | -805.0[1] | – | – | – |
| Zn(NO3)2 (cr) 2 hydrate | -1110.27[1] | – | – | – |
| Zn(NO3)2 (cr) 4 hydrate | -1699.12[1] | – | – | – |
| Zn(NO3)2 (cr) 6 hydrate | -2306.64[1] | -1772.71[1] | 456.9[1] | 323.0[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) | 0[1] | 0[1] | 41.63[1] | 25.40[1] |
| (g) | 130.729[1] | 95.145[1] | 160.984[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°, -483.7 kJ · mol−1
- ^ ΔfH°, -568.61 kJ · mol−1
- ^ ΔfG°, -369.57 kJ · mol−1
- ^ S°, 180.7 J · K−1 · mol−1
- ^ Cp°, -126. J · K−1 · mol−1
- ^ ΔfH°, -805.0 kJ · mol−1
- ^ ΔfH°, -1110.27 kJ · mol−1
- ^ ΔfH°, -1699.12 kJ · mol−1
- ^ ΔfH°, -2306.64 kJ · mol−1
- ^ ΔfG°, -1772.71 kJ · mol−1
- ^ S°, 456.9 J · K−1 · mol−1
- ^ Cp°, 323.0 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.63 J · K−1 · mol−1
- ^ Cp°, 25.40 J · K−1 · mol−1
- ^ ΔfH°, 130.729 kJ · mol−1
- ^ ΔfG°, 95.145 kJ · mol−1
- ^ S°, 160.984 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