CaB4O7 + 2HI → CaI2 + 2B2O3 + H2O
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The reaction of calcium tetraborate and hydrogen iodide yields calcium iodide, diboron trioxide, and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of calcium tetraborate and hydrogen iodide
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of calcium tetraborate and hydrogen iodide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaB4O7 | Calcium tetraborate | 1 | Brønsted base | Salt of weak acid |
| HI | Hydrogen iodide | 2 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaI2 | Calcium iodide | 1 | Conjugate base | Salt of strong acid |
| B2O3 | Diboron trioxide | 2 | – | Acidic oxide |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of calcium tetraborate and hydrogen iodide◆
ΔrG 10.3 kJ/mol K 0.16 × 10−1 pK 1.80
| 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 | −57.6 | 10.3 | −228 | – |
per 1 mol of | −57.6 | 10.3 | −228 | – |
per 1 mol of | −28.8 | 5.15 | −114 | – |
per 1 mol of | −57.6 | 10.3 | −228 | – |
per 1 mol of | −28.8 | 5.15 | −114 | – |
per 1 mol of | −57.6 | 10.3 | −228 | – |
Changes in standard condition (2)
- Reaction of calcium tetraborate and hydrogen iodide◆
ΔrG 33.0 kJ/mol K 0.17 × 10−5 pK 5.78
| 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 | −21.1 | 33.0 | −180 | – |
per 1 mol of | −21.1 | 33.0 | −180 | – |
per 1 mol of | −10.6 | 16.5 | −90.0 | – |
per 1 mol of | −21.1 | 33.0 | −180 | – |
per 1 mol of | −10.6 | 16.5 | −90.0 | – |
per 1 mol of | −21.1 | 33.0 | −180 | – |
Changes in aqueous solution
- Reaction of calcium tetraborate and hydrogen iodide◆
ΔrG −11.00 kJ/mol K 8.46 × 101 pK −1.93
| 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 | −13.95 | −11.00 | −9.9 | – |
per 1 mol of | −13.95 | −11.00 | −9.9 | – |
per 1 mol of | −6.975 | −5.500 | −5.0 | – |
per 1 mol of | −13.95 | −11.00 | −9.9 | – |
per 1 mol of | −6.975 | −5.500 | −5.0 | – |
per 1 mol of | −13.95 | −11.00 | −9.9 | – |
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 |
|---|---|---|---|---|
| CaB4O7 (cr) | -3360.25[1] | -3167.01[1] | 134.7[1] | 157.95[1] |
| CaB4O7 (vit) | -3307.37[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, (vit):Vitreous 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 |
|---|---|---|---|---|
| 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] | – | – | – |
| B2O3 (cr) | -1272.77[1] | -1193.65[1] | 53.97[1] | 62.93[1] |
| B2O3 (am) | -1254.53[1] | -1182.3[1] | 77.8[1] | 61.1[1] |
| B2O3 (g) | -843.79[1] | -831.97[1] | 279.81[1] | 66.86[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] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (am):Amorphous solid, (l):Liquid
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°, -3360.25 kJ · mol−1
- ^ ΔfG°, -3167.01 kJ · mol−1
- ^ S°, 134.7 J · K−1 · mol−1
- ^ Cp°, 157.95 J · K−1 · mol−1
- ^ ΔfH°, -3307.37 kJ · 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
- ^ 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°, -1272.77 kJ · mol−1
- ^ ΔfG°, -1193.65 kJ · mol−1
- ^ S°, 53.97 J · K−1 · mol−1
- ^ Cp°, 62.93 J · K−1 · mol−1
- ^ ΔfH°, -1254.53 kJ · mol−1
- ^ ΔfG°, -1182.3 kJ · mol−1
- ^ S°, 77.8 J · K−1 · mol−1
- ^ Cp°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -843.79 kJ · mol−1
- ^ ΔfG°, -831.97 kJ · mol−1
- ^ S°, 279.81 J · K−1 · mol−1
- ^ Cp°, 66.86 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