9ZnI2 + 2HNO3 + 18H+ → 9Zn2+ + 8I2 + 2NH4I + 6H2O
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- Reaction of zinc iodide and nitric acid under acidic condition
- 9ZnI2Zinc iodide + 2HNO3Nitric acid + 18H+Hydrogen ion9Zn2+Zinc ion + 8 + 2NH4IAmmonium iodide + 6H2OWater⟶
The reaction of zinc iodide, nitric acid, and hydrogen ion yields zinc ion, , ammonium iodide, 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 zinc iodide and nitric acid under acidic condition
- 9ZnI2Zinc iodide + 2HNO3Nitric acid + 18H+Hydrogen ion9Zn2+Zinc ion + 8 + 2NH4IAmmonium iodide + 6H2OWater⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of zinc iodide and nitric acid under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnI2 | Zinc iodide | 9 | Reducing | Oxidizable |
| HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 18 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn2+ | Zinc ion | 9 | – | – |
| 8 | Oxidized | – | ||
| NH4I | Ammonium iodide | 2 | Reduced | – |
| H2O | Water | 6 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of zinc iodide and nitric acid under acidic condition◆
ΔrG −402.57 kJ/mol K 3.37 × 1070 pK −70.53
| 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 | −501.5 | −402.57 | −329.7 | – |
per 1 mol of | −55.72 | −44.730 | −36.63 | – |
per 1 mol of | −250.8 | −201.28 | −164.8 | – |
per 1 mol of Hydrogen ion | −27.86 | −22.365 | −18.32 | – |
per 1 mol of Zinc ion | −55.72 | −44.730 | −36.63 | – |
| −62.69 | −50.321 | −41.21 | – | |
per 1 mol of | −250.8 | −201.28 | −164.8 | – |
per 1 mol of | −83.58 | −67.095 | −54.95 | – |
Changes in standard condition (2)
- Reaction of zinc iodide and nitric acid under acidic condition◆
ΔrG −489.0 kJ/mol K 4.67 × 1085 pK −85.67
| 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 | – | −489.0 | – | – |
per 1 mol of | – | −54.33 | – | – |
per 1 mol of | – | −244.5 | – | – |
per 1 mol of Hydrogen ion | – | −27.17 | – | – |
per 1 mol of Zinc ion | – | −54.33 | – | – |
| – | −61.13 | – | – | |
per 1 mol of | – | −244.5 | – | – |
per 1 mol of | – | −81.50 | – | – |
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 |
|---|---|---|---|---|
| ZnI2 (cr) | -208.03[1] | -208.95[1] | 161.1[1] | – |
| ZnI2 (ai) | -264.26[1] | -250.20[1] | 110.5[1] | -238[1] |
| ZnI2 (ao) | – | -240.6[1] | – | – |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| Zn2+ (g) | 2782.78[1] | – | – | – |
| Zn2+ (ao) | -153.89[1] | -147.06[1] | -112.1[1] | 46[1] |
| (cr) | 0[1] | 0[1] | 116.135[1] | 54.438[1] |
| (g) | 62.438[1] | 19.327[1] | 260.69[1] | 36.90[1] |
| (ao) | 22.6[1] | 16.40[1] | 137.2[1] | – |
| NH4I (cr) | -201.42[1] | -112.5[1] | 117[1] | – |
| NH4I (ai) | -187.69[1] | -130.88[1] | 224.7[1] | -62.3[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] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):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°, -208.03 kJ · mol−1
- ^ ΔfG°, -208.95 kJ · mol−1
- ^ S°, 161.1 J · K−1 · mol−1
- ^ ΔfH°, -264.26 kJ · mol−1
- ^ ΔfG°, -250.20 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, -238. J · K−1 · mol−1
- ^ ΔfG°, -240.6 kJ · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, 2782.78 kJ · mol−1
- ^ ΔfH°, -153.89 kJ · mol−1
- ^ ΔfG°, -147.06 kJ · mol−1
- ^ S°, -112.1 J · K−1 · mol−1
- ^ Cp°, 46. J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 116.135 J · K−1 · mol−1
- ^ Cp°, 54.438 J · K−1 · mol−1
- ^ ΔfH°, 62.438 kJ · mol−1
- ^ ΔfG°, 19.327 kJ · mol−1
- ^ S°, 260.69 J · K−1 · mol−1
- ^ Cp°, 36.90 J · K−1 · mol−1
- ^ ΔfH°, 22.6 kJ · mol−1
- ^ ΔfG°, 16.40 kJ · mol−1
- ^ S°, 137.2 J · K−1 · mol−1
- ^ ΔfH°, -201.42 kJ · mol−1
- ^ ΔfG°, -112.5 kJ · mol−1
- ^ S°, 117. J · K−1 · mol−1
- ^ ΔfH°, -187.69 kJ · mol−1
- ^ ΔfG°, -130.88 kJ · mol−1
- ^ S°, 224.7 J · K−1 · mol−1
- ^ Cp°, -62.3 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