CdCO3 + Ca(OH)2 → CaCO3 + Cd(OH)2
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The reaction of cadmium carbonate and calcium hydroxide yields calcium carbonate and cadmium hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of cadmium carbonate and calcium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of cadmium carbonate and calcium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CdCO3 | Cadmium carbonate | 1 | Brønsted acid | Salt of weak base |
| Ca(OH)2 | Calcium hydroxide | 1 | Brønsted base | Strong base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaCO3 | Calcium carbonate | 1 | Conjugate acid | Salt of strong base |
| Cd(OH)2 | Cadmium hydroxide | 1 | Conjugate base | Weak base |
Thermodynamic changes
Changes in standard condition
- Reaction of cadmium carbonate and calcium hydroxide◆
ΔrG −33.5 kJ/mol K 7.40 × 105 pK −5.87
| 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 | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
Changes in aqueous solution (1)
- Reaction of cadmium carbonate and calcium hydroxide◆
ΔrG −2.5 kJ/mol K 2.74 × 100 pK −0.44
| 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 | – | −2.5 | – | – |
per 1 mol of | – | −2.5 | – | – |
per 1 mol of | – | −2.5 | – | – |
per 1 mol of | – | −2.5 | – | – |
per 1 mol of | – | −2.5 | – | – |
Changes in aqueous solution (2)
- Reaction of cadmium carbonate and calcium hydroxide◆
ΔrG −33.5 kJ/mol K 7.40 × 105 pK −5.87
| 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 | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 9 | – |
per 1 mol of | −31.1 | −33.5 | 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 |
|---|---|---|---|---|
| CdCO3 (cr) | -750.6[1] | -669.4[1] | 92.5[1] | – |
| Ca(OH)2 (cr) | -986.09[1] | -898.49[1] | 83.39[1] | 87.49[1] |
| Ca(OH)2 (g) | -544[1] | – | – | – |
| Ca(OH)2 (ai) | -1002.82[1] | -868.07[1] | -74.5[1] | – |
| Ca(OH)2 (cr) 2 hydrate | -1218.4[1] | – | – | – |
* (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 |
|---|---|---|---|---|
| CaCO3 (cr) | -1207.13[1] | -1127.75[1] | 88.7[1] | 81.25[1] |
| CaCO3 (ai) | -1219.97[1] | -1081.39[1] | -110.0[1] | – |
| Cd(OH)2 (cr) precipitated | -560.7[1] | -473.6[1] | 96[1] | – |
| Cd(OH)2 (ai) | -535.89[1] | -392.10[1] | -94.6[1] | – |
| Cd(OH)2 (ao) | – | -442.6[1] | – | – |
* (cr):Crystalline solid, (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°, -750.6 kJ · mol−1
- ^ ΔfG°, -669.4 kJ · mol−1
- ^ S°, 92.5 J · K−1 · mol−1
- ^ ΔfH°, -986.09 kJ · mol−1
- ^ ΔfG°, -898.49 kJ · mol−1
- ^ S°, 83.39 J · K−1 · mol−1
- ^ Cp°, 87.49 J · K−1 · mol−1
- ^ ΔfH°, -544. kJ · mol−1
- ^ ΔfH°, -1002.82 kJ · mol−1
- ^ ΔfG°, -868.07 kJ · mol−1
- ^ S°, -74.5 J · K−1 · mol−1
- ^ ΔfH°, -1218.4 kJ · mol−1
- ^ ΔfH°, -1207.13 kJ · mol−1
- ^ ΔfG°, -1127.75 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1
- ^ Cp°, 81.25 J · K−1 · mol−1
- ^ ΔfH°, -1219.97 kJ · mol−1
- ^ ΔfG°, -1081.39 kJ · mol−1
- ^ S°, -110.0 J · K−1 · mol−1
- ^ ΔfH°, -560.7 kJ · mol−1
- ^ ΔfG°, -473.6 kJ · mol−1
- ^ S°, 96. J · K−1 · mol−1
- ^ ΔfH°, -535.89 kJ · mol−1
- ^ ΔfG°, -392.10 kJ · mol−1
- ^ S°, -94.6 J · K−1 · mol−1
- ^ ΔfG°, -442.6 kJ · mol−1