3ZnCO3 + 2H3AsO4 → Zn3(AsO4)2 + 3H2CO3
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- Reaction of zinc carbonate and arsenic acid
The reaction of zinc carbonate and arsenic acid yields zinc arsenate and carbonic acid (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of zinc carbonate and arsenic 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 zinc carbonate and arsenic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnCO3 | Zinc carbonate | 3 | Brønsted base | Salt of volatile acid |
| H3AsO4 | Arsenic acid | 2 | Brønsted acid | Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn3(AsO4)2 | Zinc arsenate | 1 | Conjugate base | Salt of non volatile acid |
| H2CO3 | Carbonic acid | 3 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of zinc carbonate and arsenic acid◆
ΔrG −38 kJ/mol K 4.54 × 106 pK −6.66 - 3ZnCO3Crystalline solid + 2H3AsO4Un-ionized aqueous solutionZn3(AsO4)2Crystalline solid + 3H2CO3Un-ionized aqueous solution⟶
| 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 | – | −38 | – | – |
per 1 mol of | – | −13 | – | – |
per 1 mol of | – | −19 | – | – |
per 1 mol of | – | −38 | – | – |
per 1 mol of | – | −13 | – | – |
Changes in standard condition (2)
- Reaction of zinc carbonate and arsenic acid
- 3ZnCO3Crystalline solid + 2H3AsO4Aqueous solutionZn3(AsO4)2Crystalline solid + 3H2CO3Un-ionized aqueous solution⟶
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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 |
|---|---|---|---|---|
| ZnCO3 (cr) | -812.78[1] | -731.52[1] | 82.4[1] | 79.71[1] |
| ZnCO3 (cr) 1 hydrate | – | -970.6[1] | – | – |
| H3AsO4 (cr) | -906.3[1] | – | – | – |
| H3AsO4 (ao) | -902.5[1] | -766.0[1] | 184[1] | – |
| H3AsO4 (aq) | -904.6[1] | – | – | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (aq):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 |
|---|---|---|---|---|
| Zn3(AsO4)2 (cr) | – | -1895[1] | – | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (cr):Crystalline solid, (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°, -812.78 kJ · mol−1
- ^ ΔfG°, -731.52 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, 79.71 J · K−1 · mol−1
- ^ ΔfG°, -970.6 kJ · mol−1
- ^ ΔfH°, -906.3 kJ · mol−1
- ^ ΔfH°, -902.5 kJ · mol−1
- ^ ΔfG°, -766.0 kJ · mol−1
- ^ S°, 184. J · K−1 · mol−1
- ^ ΔfH°, -904.6 kJ · mol−1
- ^ ΔfG°, -1895. kJ · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1