2CuCl + 2HNO3 🔥→ CuCl2 + Cu(NO3)2 + H2↑
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- Reaction of copper(I) chloride and nitric acid
The reaction of copper(I) chloride and nitric acid yields copper(II) chloride, copper(II) nitrate, and (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 copper(I) chloride and nitric acid
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of copper(I) chloride and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuCl | Copper(I) chloride | 2 | Reducing | Oxidizable |
| HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuCl2 | Copper(II) chloride | 1 | Oxidized | – |
| Cu(NO3)2 | Copper(II) nitrate | 1 | Oxidized | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of copper(I) chloride and nitric acid
| 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 | 99.6 | – | – | – |
per 1 mol of | 49.8 | – | – | – |
per 1 mol of | 49.8 | – | – | – |
per 1 mol of | 99.6 | – | – | – |
per 1 mol of | 99.6 | – | – | – |
| 99.6 | – | – | – |
Changes in aqueous solution (1)
- Reaction of copper(I) chloride and nitric acid◆
ΔrG 107.3 kJ/mol K 0.16 × 10−18 pK 18.80
| 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 | – | 107.3 | – | – |
per 1 mol of | – | 53.65 | – | – |
per 1 mol of | – | 53.65 | – | – |
per 1 mol of | – | 107.3 | – | – |
per 1 mol of | – | 107.3 | – | – |
| – | 107.3 | – | – |
Changes in aqueous solution (2)
- Reaction of copper(I) chloride and nitric acid◆
ΔrG 124.9 kJ/mol K 0.13 × 10−21 pK 21.88
| 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 | – | 124.9 | – | – |
per 1 mol of | – | 62.45 | – | – |
per 1 mol of | – | 62.45 | – | – |
per 1 mol of | – | 124.9 | – | – |
per 1 mol of | – | 124.9 | – | – |
| – | 124.9 | – | – |
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 |
|---|---|---|---|---|
| CuCl (cr) | -137.2[1] | -119.86[1] | 86.2[1] | 48.5[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] |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (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 |
|---|---|---|---|---|
| CuCl2 (cr) | -220.1[1] | -175.7[1] | 108.07[1] | 71.88[1] |
| CuCl2 (ao) | – | -197.9[1] | – | – |
| CuCl2 (cr) 2 hydrate | -821.3[1] | -655.9[1] | 167[1] | – |
| Cu(NO3)2 (cr) | -302.9[1] | – | – | – |
| Cu(NO3)2 (ai) | -349.95[1] | -157.02[1] | 193.3[1] | – |
| Cu(NO3)2 (cr) 3 hydrate | -1217.1[1] | – | – | – |
| Cu(NO3)2 (cr) 6 hydrate | -2110.8[1] | – | – | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (ai):Ionized aqueous solution, (g):Gas
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°, -137.2 kJ · mol−1
- ^ ΔfG°, -119.86 kJ · mol−1
- ^ S°, 86.2 J · K−1 · mol−1
- ^ Cp°, 48.5 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°, -220.1 kJ · mol−1
- ^ ΔfG°, -175.7 kJ · mol−1
- ^ S°, 108.07 J · K−1 · mol−1
- ^ Cp°, 71.88 J · K−1 · mol−1
- ^ ΔfG°, -197.9 kJ · mol−1
- ^ ΔfH°, -821.3 kJ · mol−1
- ^ ΔfG°, -655.9 kJ · mol−1
- ^ S°, 167. J · K−1 · mol−1
- ^ ΔfH°, -302.9 kJ · mol−1
- ^ ΔfH°, -349.95 kJ · mol−1
- ^ ΔfG°, -157.02 kJ · mol−1
- ^ S°, 193.3 J · K−1 · mol−1
- ^ ΔfH°, -1217.1 kJ · mol−1
- ^ ΔfH°, -2110.8 kJ · mol−1
- ^ 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