FeI2 + Ca(HCO3)2 💧→ FeCO3↓ + CaI2 + H2CO3
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The reaction of iron(II) iodide and calcium hydrogencarbonate yields iron(II) carbonate, calcium iodide, and carbonic acid. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of iron(II) iodide and calcium hydrogencarbonate
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of iron(II) iodide and calcium hydrogencarbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeI2 | Iron(II) iodide | 1 | Lewis acid | Soluble in water |
| Ca(HCO3)2 | Calcium hydrogencarbonate | 1 | Lewis base | Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| FeCO3 | Iron(II) carbonate | 1 | Lewis conjugate | Very slightly soluble in water |
| CaI2 | Calcium iodide | 1 | Non-redox product | – |
| H2CO3 | Carbonic acid | 1 | Non-redox product | – |
Thermodynamic changes
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 |
|---|---|---|---|---|
| FeI2 (cr) | -113.0[1] | – | – | – |
| FeI2 (g) | 60.7[1] | – | – | – |
| FeI2 (ai) | -199.6[1] | -182.05[1] | 84.9[1] | – |
| Ca(HCO3)2 | – | – | – | – |
* (cr):Crystalline 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 |
|---|---|---|---|---|
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[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] | – | – | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (cr):Crystalline solid, (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°, -113.0 kJ · mol−1
- ^ ΔfH°, 60.7 kJ · mol−1
- ^ ΔfH°, -199.6 kJ · mol−1
- ^ ΔfG°, -182.05 kJ · mol−1
- ^ S°, 84.9 J · K−1 · mol−1
- ^ ΔfH°, -740.57 kJ · mol−1
- ^ ΔfG°, -666.67 kJ · mol−1
- ^ S°, 92.9 J · K−1 · mol−1
- ^ Cp°, 82.13 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°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1