CuF + HI → CuI + HF
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The reaction of copper(I) fluoride and hydrogen iodide yields copper(I) iodide 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 iodide
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 iodide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CuF | Copper(I) fluoride | 1 | Brønsted base | Salt of weak acid |
HI | Hydrogen iodide | 1 | Brønsted acid | Strong acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CuI | Copper(I) iodide | 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 iodide◆
ΔrG −84 kJ/mol K 5.20 × 1014 pK −14.72
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 | −85 | −84 | −1.0 | – |
per 1 mol of | −85 | −84 | −1.0 | – |
per 1 mol of | −85 | −84 | −1.0 | – |
per 1 mol of | −85 | −84 | −1.0 | – |
per 1 mol of | −85 | −84 | −1.0 | – |
Changes in aqueous solution (1)
- Reaction of copper(I) fluoride and hydrogen iodide◆
ΔrG −31 kJ/mol K 2.70 × 105 pK −5.43
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 | −4 | −31 | 94.3 | – |
per 1 mol of | −4 | −31 | 94.3 | – |
per 1 mol of | −4 | −31 | 94.3 | – |
per 1 mol of | −4 | −31 | 94.3 | – |
per 1 mol of | −4 | −31 | 94.3 | – |
Changes in aqueous solution (2)
- Reaction of copper(I) fluoride and hydrogen iodide◆
ΔrG −55 kJ/mol K 4.32 × 109 pK −9.64
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 | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
Changes in aqueous solution (3)
- Reaction of copper(I) fluoride and hydrogen iodide◆
ΔrG −55 kJ/mol K 4.32 × 109 pK −9.64
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 | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
per 1 mol of | −53 | −55 | 9.2 | – |
Changes in aqueous solution (4)
- Reaction of copper(I) fluoride and hydrogen iodide◆
ΔrG −37 kJ/mol K 3.03 × 106 pK −6.48
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 | −65 | −37 | −93.3 | – |
per 1 mol of | −65 | −37 | −93.3 | – |
per 1 mol of | −65 | −37 | −93.3 | – |
per 1 mol of | −65 | −37 | −93.3 | – |
per 1 mol of | −65 | −37 | −93.3 | – |
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 | – |
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] |
* (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 |
---|---|---|---|---|
CuI (cr) | -67.8[1] | -69.5[1] | 96.7[1] | 54.06[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°, 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
- ^ ΔfH°, -67.8 kJ · mol−1
- ^ ΔfG°, -69.5 kJ · mol−1
- ^ S°, 96.7 J · K−1 · mol−1
- ^ Cp°, 54.06 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