ZnI2 + 2HNO3 + 2H+ 🔥→ Zn2+ + HIO3 + 2NO↑ + H2O + HI↑
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- Reaction of zinc iodide and nitric acid under acidic condition
- ZnI2Zinc iodide + 2HNO3Nitric acid + 2H+Hydrogen ionZn2+Zinc ion + HIO3Iodic acid + 2NO↑Nitrogen monoxide + H2OWater + HI↑Hydrogen iodide🔥⟶
The reaction of zinc iodide, nitric acid, and hydrogen ion yields zinc ion, iodic acid, nitrogen monoxide, water, and hydrogen iodide (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
- ZnI2Zinc iodide + 2HNO3Nitric acid + 2H+Hydrogen ionZn2+Zinc ion + HIO3Iodic acid + 2NO↑Nitrogen monoxide + H2OWater + HI↑Hydrogen iodide🔥⟶
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 | 1 | Reducing | Oxidizable |
| HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 2 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn2+ | Zinc ion | 1 | – | – |
| HIO3 | Iodic acid | 1 | Oxidized | – |
| NO | Nitrogen monoxide | 2 | Reduced | – |
| H2O | Water | 1 | – | Water |
| HI | Hydrogen iodide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of zinc iodide and nitric acid under acidic condition◆
ΔrG 130.7 kJ/mol K 0.13 × 10−22 pK 22.90
| 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 | 234.9 | 130.7 | 349.5 | – |
per 1 mol of | 234.9 | 130.7 | 349.5 | – |
per 1 mol of | 117.5 | 65.35 | 174.8 | – |
per 1 mol of Hydrogen ion | 117.5 | 65.35 | 174.8 | – |
per 1 mol of Zinc ion | 234.9 | 130.7 | 349.5 | – |
per 1 mol of | 234.9 | 130.7 | 349.5 | – |
per 1 mol of | 117.5 | 65.35 | 174.8 | – |
per 1 mol of | 234.9 | 130.7 | 349.5 | – |
per 1 mol of | 234.9 | 130.7 | 349.5 | – |
Changes in standard condition (2)
- Reaction of zinc iodide and nitric acid under acidic condition◆
ΔrG 77.4 kJ/mol K 0.28 × 10−13 pK 13.56
| 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 | 153.3 | 77.4 | 254.2 | – |
per 1 mol of | 153.3 | 77.4 | 254.2 | – |
per 1 mol of | 76.65 | 38.7 | 127.1 | – |
per 1 mol of Hydrogen ion | 76.65 | 38.7 | 127.1 | – |
per 1 mol of Zinc ion | 153.3 | 77.4 | 254.2 | – |
per 1 mol of | 153.3 | 77.4 | 254.2 | – |
per 1 mol of | 76.65 | 38.7 | 127.1 | – |
per 1 mol of | 153.3 | 77.4 | 254.2 | – |
per 1 mol of | 153.3 | 77.4 | 254.2 | – |
Changes in standard condition (3)
- Reaction of zinc iodide and nitric acid under acidic condition◆
ΔrG 121.1 kJ/mol K 0.61 × 10−21 pK 21.22
| 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 | – | 121.1 | – | – |
per 1 mol of | – | 121.1 | – | – |
per 1 mol of | – | 60.55 | – | – |
per 1 mol of Hydrogen ion | – | 60.55 | – | – |
per 1 mol of Zinc ion | – | 121.1 | – | – |
per 1 mol of | – | 121.1 | – | – |
per 1 mol of | – | 60.55 | – | – |
per 1 mol of | – | 121.1 | – | – |
per 1 mol of | – | 121.1 | – | – |
Changes in standard condition (4)
- Reaction of zinc iodide and nitric acid under acidic condition◆
ΔrG 67.8 kJ/mol K 0.13 × 10−11 pK 11.88
| 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 | – | 67.8 | – | – |
per 1 mol of | – | 67.8 | – | – |
per 1 mol of | – | 33.9 | – | – |
per 1 mol of Hydrogen ion | – | 33.9 | – | – |
per 1 mol of Zinc ion | – | 67.8 | – | – |
per 1 mol of | – | 67.8 | – | – |
per 1 mol of | – | 33.9 | – | – |
per 1 mol of | – | 67.8 | – | – |
per 1 mol of | – | 67.8 | – | – |
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] |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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] |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (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°, -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°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 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
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1