CuF + HCl → CuCl + HF
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The reaction of copper(I) fluoride and hydrogen chloride yields copper(I) chloride and hydrogen fluoride. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of copper(I) fluoride and hydrogen chloride
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
Oxidation state of each atom
- Reaction of copper(I) fluoride and hydrogen chloride
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuF | Copper(I) fluoride | 1 | Brønsted base | Salt of weak acid |
| HCl | Hydrogen chloride | 1 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuCl | Copper(I) chloride | 1 | Conjugate base | Salt of strong acid |
| HF | Hydrogen fluoride | 1 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in standard condition
- Reaction of copper(I) fluoride and hydrogen chloride◆
ΔrG −38 kJ/mol K 4.54 × 106 pK −6.66
| 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 | −36 | −38 | 8.2 | – |
per 1 mol of | −36 | −38 | 8.2 | – |
per 1 mol of | −36 | −38 | 8.2 | – |
per 1 mol of | −36 | −38 | 8.2 | – |
per 1 mol of | −36 | −38 | 8.2 | – |
Changes in aqueous solution (1)
- Reaction of copper(I) fluoride and hydrogen chloride◆
ΔrG −2 kJ/mol K 2.24 × 100 pK −0.35
| 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 | 39 | −2 | 138.6 | – |
per 1 mol of | 39 | −2 | 138.6 | – |
per 1 mol of | 39 | −2 | 138.6 | – |
per 1 mol of | 39 | −2 | 138.6 | – |
per 1 mol of | 39 | −2 | 138.6 | – |
Changes in aqueous solution (2)
- Reaction of copper(I) fluoride and hydrogen chloride◆
ΔrG −25 kJ/mol K 2.40 × 104 pK −4.38
| 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 | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
Changes in aqueous solution (3)
- Reaction of copper(I) fluoride and hydrogen chloride◆
ΔrG −25 kJ/mol K 2.40 × 104 pK −4.38
| 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 | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
per 1 mol of | −10 | −25 | 53.5 | – |
Changes in aqueous solution (4)
- Reaction of copper(I) fluoride and hydrogen chloride◆
ΔrG −7 kJ/mol K 1.68 × 101 pK −1.23
| 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 | −23 | −7 | −49.0 | – |
per 1 mol of | −23 | −7 | −49.0 | – |
per 1 mol of | −23 | −7 | −49.0 | – |
per 1 mol of | −23 | −7 | −49.0 | – |
per 1 mol of | −23 | −7 | −49.0 | – |
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 |
|---|---|---|---|---|
| CuF (s) | -280 | -260 | 64.9 | – |
| 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] |
* (s):Solid, (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 |
|---|---|---|---|---|
| CuCl (cr) | -137.2[1] | -119.86[1] | 86.2[1] | 48.5[1] |
| HF (l) x denotes undetermined zero point entropy | -299.78[1] | – | 75.40+x[1] | – |
| HF (g) | -271.1[1] | -273.2[1] | 173.779[1] | 29.133[1] |
| HF (ai) | -332.63[1] | -278.79[1] | -13.8[1] | -106.7[1] |
| HF (ao) | -320.08[1] | -296.82[1] | 88.7[1] | – |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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°, -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°, -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°, -299.78 kJ · mol−1
- ^ S°, 75.40+x J · K−1 · mol−1
- ^ ΔfH°, -271.1 kJ · mol−1
- ^ ΔfG°, -273.2 kJ · mol−1
- ^ S°, 173.779 J · K−1 · mol−1
- ^ Cp°, 29.133 J · K−1 · mol−1
- ^ ΔfH°, -332.63 kJ · mol−1
- ^ ΔfG°, -278.79 kJ · mol−1
- ^ S°, -13.8 J · K−1 · mol−1
- ^ Cp°, -106.7 J · K−1 · mol−1
- ^ ΔfH°, -320.08 kJ · mol−1
- ^ ΔfG°, -296.82 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1