CdSO4 + Li2CO3 💧→ CdCO3↓ + Li2SO4
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The reaction of cadmium sulfate and lithium carbonate yields cadmium carbonate and lithium sulfate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of cadmium sulfate and lithium carbonate
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 cadmium sulfate and lithium carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CdSO4 | Cadmium sulfate | 1 | Lewis acid | Very soluble in water |
| Li2CO3 | Lithium carbonate | 1 | Lewis base | Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CdCO3 | Cadmium carbonate | 1 | Lewis conjugate | Insoluble in water |
| Li2SO4 | Lithium sulfate | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of cadmium sulfate and lithium carbonate◆
ΔrG −36.3 kJ/mol K 2.29 × 106 pK −6.36
| 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 | −37.9 | −36.3 | −5.8 | – |
per 1 mol of | −37.9 | −36.3 | −5.8 | – |
per 1 mol of | −37.9 | −36.3 | −5.8 | – |
per 1 mol of | −37.9 | −36.3 | −5.8 | – |
per 1 mol of | −37.9 | −36.3 | −5.8 | – |
Changes in aqueous solution
- Reaction of cadmium sulfate and lithium carbonate◆
ΔrG −45.8 kJ/mol K 1.06 × 108 pK −8.02
| 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 | −67.7 | −45.8 | −73.6 | – |
per 1 mol of | −67.7 | −45.8 | −73.6 | – |
per 1 mol of | −67.7 | −45.8 | −73.6 | – |
per 1 mol of | −67.7 | −45.8 | −73.6 | – |
per 1 mol of | −67.7 | −45.8 | −73.6 | – |
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 |
|---|---|---|---|---|
| CdSO4 (cr) | -933.28[1] | -822.72[1] | 123.039[1] | 99.58[1] |
| CdSO4 (ai) | -985.16[1] | -822.13[1] | -53.1[1] | – |
| CdSO4 (cr) 1 hydrate | -1239.55[1] | -1068.73[1] | 154.030[1] | 134.56[1] |
| CdSO4 (cr) 8/3 hydrate | -1729.4[1] | -1465.141[1] | 229.630[1] | 213.26[1] |
| Li2CO3 (cr) | -1215.9[1] | -1132.06[1] | 90.37[1] | 99.12[1] |
| Li2CO3 (ai) | -1234.11[1] | -1114.6[1] | -29.7[1] | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| CdCO3 (cr) | -750.6[1] | -669.4[1] | 92.5[1] | – |
| Li2SO4 (cr) | -1436.49[1] | -1321.70[1] | 115.1[1] | 117.57[1] |
| Li2SO4 (ai) | -1466.24[1] | -1331.20[1] | 47.3[1] | -155.6[1] |
| Li2SO4 (cr) 1 hydrate | -1735.5[1] | -1565.5[1] | 163.6[1] | 151.08[1] |
* (cr):Crystalline solid, (ai):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°, -933.28 kJ · mol−1
- ^ ΔfG°, -822.72 kJ · mol−1
- ^ S°, 123.039 J · K−1 · mol−1
- ^ Cp°, 99.58 J · K−1 · mol−1
- ^ ΔfH°, -985.16 kJ · mol−1
- ^ ΔfG°, -822.13 kJ · mol−1
- ^ S°, -53.1 J · K−1 · mol−1
- ^ ΔfH°, -1239.55 kJ · mol−1
- ^ ΔfG°, -1068.73 kJ · mol−1
- ^ S°, 154.030 J · K−1 · mol−1
- ^ Cp°, 134.56 J · K−1 · mol−1
- ^ ΔfH°, -1729.4 kJ · mol−1
- ^ ΔfG°, -1465.141 kJ · mol−1
- ^ S°, 229.630 J · K−1 · mol−1
- ^ Cp°, 213.26 J · K−1 · mol−1
- ^ ΔfH°, -1215.9 kJ · mol−1
- ^ ΔfG°, -1132.06 kJ · mol−1
- ^ S°, 90.37 J · K−1 · mol−1
- ^ Cp°, 99.12 J · K−1 · mol−1
- ^ ΔfH°, -1234.11 kJ · mol−1
- ^ ΔfG°, -1114.6 kJ · mol−1
- ^ S°, -29.7 J · K−1 · mol−1
- ^ ΔfH°, -750.6 kJ · mol−1
- ^ ΔfG°, -669.4 kJ · mol−1
- ^ S°, 92.5 J · K−1 · mol−1
- ^ ΔfH°, -1436.49 kJ · mol−1
- ^ ΔfG°, -1321.70 kJ · mol−1
- ^ S°, 115.1 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -1466.24 kJ · mol−1
- ^ ΔfG°, -1331.20 kJ · mol−1
- ^ S°, 47.3 J · K−1 · mol−1
- ^ Cp°, -155.6 J · K−1 · mol−1
- ^ ΔfH°, -1735.5 kJ · mol−1
- ^ ΔfG°, -1565.5 kJ · mol−1
- ^ S°, 163.6 J · K−1 · mol−1
- ^ Cp°, 151.08 J · K−1 · mol−1