3HCl + 2Zn(NO3)2 + 4H+ 🔥→ 3HClO2 + 4NO + 2Zn2+ + 2H2O
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- Reaction of hydrogen chloride and zinc nitrate under acidic condition
- 3HClHydrogen chloride + 2Zn(NO3)2Zinc nitrate + 4H+Hydrogen ion3HClO2Chlorous acid + 4NONitrogen monoxide + 2Zn2+Zinc ion + 2H2OWater🔥⟶
The reaction of hydrogen chloride, zinc nitrate, and hydrogen ion yields chlorous acid, nitrogen monoxide, zinc ion, 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 zinc nitrate under acidic condition
- 3HClHydrogen chloride + 2Zn(NO3)2Zinc nitrate + 4H+Hydrogen ion3HClO2Chlorous acid + 4NONitrogen monoxide + 2Zn2+Zinc ion + 2H2OWater🔥⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species under acidic condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of hydrogen chloride and zinc nitrate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HCl | Hydrogen chloride | 3 | Reducing | Hardly oxidizable |
| Zn(NO3)2 | Zinc nitrate | 2 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 4 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HClO2 | Chlorous acid | 3 | Oxidized | – |
| NO | Nitrogen monoxide | 4 | Reduced | – |
| Zn2+ | Zinc ion | 2 | – | – |
| H2O | Water | 2 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and zinc nitrate under acidic condition◆
ΔrG 728.3 kJ/mol K 0.26 × 10−127 pK 127.59
| 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 | 964.6 | 728.3 | 792.7 | – |
per 1 mol of | 321.5 | 242.8 | 264.2 | – |
per 1 mol of | 482.3 | 364.1 | 396.4 | – |
per 1 mol of Hydrogen ion | 241.2 | 182.1 | 198.2 | – |
per 1 mol of | 321.5 | 242.8 | 264.2 | – |
per 1 mol of | 241.2 | 182.1 | 198.2 | – |
per 1 mol of Zinc ion | 482.3 | 364.1 | 396.4 | – |
per 1 mol of | 482.3 | 364.1 | 396.4 | – |
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] |
| 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] |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (g):Gas, (ai):Ionized aqueous solution, (cr):Crystalline solid, (ao):Un-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 |
|---|---|---|---|---|
| HClO2 (ao) | -51.9[1] | 5.9[1] | 188.3[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| Zn2+ (g) | 2782.78[1] | – | – | – |
| Zn2+ (ao) | -153.89[1] | -147.06[1] | -112.1[1] | 46[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] |
* (ao):Un-ionized aqueous solution, (g):Gas, (cr):Crystalline solid, (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°, -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°, -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°, 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°, -51.9 kJ · mol−1
- ^ ΔfG°, 5.9 kJ · mol−1
- ^ S°, 188.3 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°, 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°, -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