2HCl + 3Zn(NO3)2 + 6H+ 🔥→ Cl2O + 2HNO2 + 3Zn2+ + 4HNO3 + H2O
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- Reaction of hydrogen chloride and zinc nitrate under acidic condition
- 2HClHydrogen chloride + 3Zn(NO3)2Zinc nitrate + 6H+Hydrogen ionCl2ODichlorine monoxide + 2HNO2Nitrous acid + 3Zn2+Zinc ion + 4HNO3Nitric acid + H2OWater🔥⟶
The reaction of hydrogen chloride, zinc nitrate, and hydrogen ion yields dichlorine monoxide, nitrous acid, zinc ion, nitric acid, 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
- 2HClHydrogen chloride + 3Zn(NO3)2Zinc nitrate + 6H+Hydrogen ionCl2ODichlorine monoxide + 2HNO2Nitrous acid + 3Zn2+Zinc ion + 4HNO3Nitric acid + H2OWater🔥⟶
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 | 2 | Reducing | Hardly oxidizable |
| Zn(NO3)2 | Zinc nitrate | 3 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 6 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cl2O | Dichlorine monoxide | 1 | Oxidized | – |
| HNO2 | Nitrous acid | 2 | Reduced | – |
| Zn2+ | Zinc ion | 3 | – | – |
| HNO3 | Nitric acid | 4 | – | – |
| H2O | Water | 1 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen chloride and zinc nitrate under acidic condition◆
ΔrG 244.6 kJ/mol K 0.14 × 10−42 pK 42.85
| 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 | 305.1 | 244.6 | 201.5 | – |
per 1 mol of | 152.6 | 122.3 | 100.8 | – |
per 1 mol of | 101.7 | 81.53 | 67.17 | – |
per 1 mol of Hydrogen ion | 50.85 | 40.77 | 33.58 | – |
per 1 mol of | 305.1 | 244.6 | 201.5 | – |
per 1 mol of | 152.6 | 122.3 | 100.8 | – |
per 1 mol of Zinc ion | 101.7 | 81.53 | 67.17 | – |
per 1 mol of | 76.28 | 61.15 | 50.38 | – |
per 1 mol of | 305.1 | 244.6 | 201.5 | – |
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 |
|---|---|---|---|---|
| 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 |
|---|---|---|---|---|
| Cl2O (g) | 80.3[1] | 97.9[1] | 266.21[1] | 45.40[1] |
| HNO2 (g) cis | -77.99[1] | -42.94[1] | 248.76[1] | 44.77[1] |
| HNO2 (g) trans | -80.12[1] | -45.24[1] | 249.22[1] | 46.07[1] |
| HNO2 (g) | -79.5[1] | -46.0[1] | 254.1[1] | 45.6[1] |
| HNO2 (ao) | -119.2[1] | -50.6[1] | 135.6[1] | – |
| Zn2+ (g) | 2782.78[1] | – | – | – |
| Zn2+ (ao) | -153.89[1] | -147.06[1] | -112.1[1] | 46[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] |
| 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, (l):Liquid, (ai):Ionized aqueous solution, (cr):Crystalline solid
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°, 80.3 kJ · mol−1
- ^ ΔfG°, 97.9 kJ · mol−1
- ^ S°, 266.21 J · K−1 · mol−1
- ^ Cp°, 45.40 J · K−1 · mol−1
- ^ ΔfH°, -77.99 kJ · mol−1
- ^ ΔfG°, -42.94 kJ · mol−1
- ^ S°, 248.76 J · K−1 · mol−1
- ^ Cp°, 44.77 J · K−1 · mol−1
- ^ ΔfH°, -80.12 kJ · mol−1
- ^ ΔfG°, -45.24 kJ · mol−1
- ^ S°, 249.22 J · K−1 · mol−1
- ^ Cp°, 46.07 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -46.0 kJ · mol−1
- ^ S°, 254.1 J · K−1 · mol−1
- ^ Cp°, 45.6 J · K−1 · mol−1
- ^ ΔfH°, -119.2 kJ · mol−1
- ^ ΔfG°, -50.6 kJ · mol−1
- ^ S°, 135.6 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°, -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°, -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