CaI2 + 2HClO4 → Ca(ClO4)2 + 2HI↑
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The reaction of calcium iodide and perchloric acid yields calcium perchlorate and hydrogen iodide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of calcium iodide and perchloric acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of calcium iodide and perchloric acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
CaI2 | Calcium iodide | 1 | Brønsted base | Salt of volatile acid |
HClO4 | Perchloric acid | 2 | Brønsted acid | Nonvolatile acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Ca(ClO4)2 | Calcium perchlorate | 1 | Conjugate base | Salt of non volatile acid |
HI | Hydrogen iodide | 2 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of calcium iodide and perchloric 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 | −69.1 | – | – | – |
per 1 mol of | −69.1 | – | – | – |
per 1 mol of | −34.5 | – | – | – |
per 1 mol of | −69.1 | – | – | – |
per 1 mol of | −34.5 | – | – | – |
Changes in aqueous solution (1)
- Reaction of calcium iodide and perchloric acid◆
ΔrG 106.54 kJ/mol K 0.22 × 10−18 pK 18.67
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 | 163.34 | 106.54 | 190.6 | – |
per 1 mol of | 163.34 | 106.54 | 190.6 | – |
per 1 mol of | 81.670 | 53.270 | 95.30 | – |
per 1 mol of | 163.34 | 106.54 | 190.6 | – |
per 1 mol of | 81.670 | 53.270 | 95.30 | – |
Changes in aqueous solution (2)
- Reaction of calcium iodide and perchloric acid◆
ΔrG 0.00 kJ/mol K 1.00 × 100 pK 0.00
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 | 0.00 | 0.00 | 0.0 | – |
per 1 mol of | 0.00 | 0.00 | 0.0 | – |
per 1 mol of | 0.00 | 0.00 | 0.0 | – |
per 1 mol of | 0.00 | 0.00 | 0.0 | – |
per 1 mol of | 0.00 | 0.00 | 0.0 | – |
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 |
---|---|---|---|---|
CaI2 (cr) | -533.5[1] | -528.9[1] | 142[1] | – |
CaI2 (g) | -272[1] | – | – | – |
CaI2 (ai) | -653.21[1] | -656.72[1] | 169.5[1] | – |
CaI2 (cr) 8 hydrate | -2929.6[1] | – | – | – |
HClO4 (l) | -40.58[1] | – | – | – |
HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
HClO4 (l) 2 hydrate | -677.98[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid
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 |
---|---|---|---|---|
Ca(ClO4)2 (cr) | -736.76[1] | – | – | – |
Ca(ClO4)2 (ai) | -801.49[1] | -570.62[1] | 310.9[1] | – |
Ca(ClO4)2 (cr) 4 hydrate | -1948.9[1] | -1476.47[1] | 433.5[1] | – |
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] |
* (cr):Crystalline solid, (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°, -533.5 kJ · mol−1
- ^ ΔfG°, -528.9 kJ · mol−1
- ^ S°, 142. J · K−1 · mol−1
- ^ ΔfH°, -272. kJ · mol−1
- ^ ΔfH°, -653.21 kJ · mol−1
- ^ ΔfG°, -656.72 kJ · mol−1
- ^ S°, 169.5 J · K−1 · mol−1
- ^ ΔfH°, -2929.6 kJ · mol−1
- ^ ΔfH°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · mol−1
- ^ ΔfH°, -736.76 kJ · mol−1
- ^ ΔfH°, -801.49 kJ · mol−1
- ^ ΔfG°, -570.62 kJ · mol−1
- ^ S°, 310.9 J · K−1 · mol−1
- ^ ΔfH°, -1948.9 kJ · mol−1
- ^ ΔfG°, -1476.47 kJ · mol−1
- ^ S°, 433.5 J · K−1 · mol−1
- ^ 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