2CH3COONH4 + Mn(OH)2 🔥→ Mn(CH3COO)2 + 2NH3↑ + 2H2O
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The reaction of ammonium acetate and manganese(II) hydroxide yields manganese(II) acetate, ammonia, and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium acetate and manganese(II) hydroxide
General equation
- Reaction of volatile acid and non volatile base
- Salt of volatile baseBrønsted acid + Nonvolatile baseBrønsted base ⟶ Salt of non volatile baseConjugate acid + Volatile baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of ammonium acetate and manganese(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COONH4 | Ammonium acetate | 2 | Brønsted acid | Salt of volatile base |
| Mn(OH)2 | Manganese(II) hydroxide | 1 | Brønsted base | Nonvolatile base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(CH3COO)2 | Manganese(II) acetate | 1 | Conjugate acid | Salt of non volatile base |
| NH3 | Ammonia | 2 | Conjugate base | Volatile base |
| H2O | Water | 2 | – | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium acetate and manganese(II) hydroxide
- 2CH3COONH4Crystalline solid + Mn(OH)2Amorphous solidprecipitatedMn(CH3COO)2Crystalline solid + 2NH3↑Gas + 2H2OLiquid🔥⟶
| 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 | 115.7 | – | – | – |
per 1 mol of | 57.85 | – | – | – |
per 1 mol of | 115.7 | – | – | – |
per 1 mol of | 115.7 | – | – | – |
per 1 mol of | 57.85 | – | – | – |
per 1 mol of | 57.85 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium acetate and manganese(II) hydroxide
- 2CH3COONH4Ionized aqueous solution + Mn(OH)2Amorphous solidprecipitatedMn(CH3COO)2Aqueous solution + 2NH3↑Gas + 2H2OLiquid🔥⟶
| 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 | 69.5 | – | – | – |
per 1 mol of | 34.8 | – | – | – |
per 1 mol of | 69.5 | – | – | – |
per 1 mol of | 69.5 | – | – | – |
per 1 mol of | 34.8 | – | – | – |
per 1 mol of | 34.8 | – | – | – |
Changes in aqueous solution (2)
- Reaction of ammonium acetate and manganese(II) hydroxide
- 2CH3COONH4Ionized aqueous solution + Mn(OH)2Amorphous solidprecipitatedMn(CH3COO)2Aqueous solution + 2NH3↑Un-ionized aqueous solution + 2H2OLiquid🔥⟶
| 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 | 1.1 | – | – | – |
per 1 mol of | 0.55 | – | – | – |
per 1 mol of | 1.1 | – | – | – |
per 1 mol of | 1.1 | – | – | – |
per 1 mol of | 0.55 | – | – | – |
per 1 mol of | 0.55 | – | – | – |
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 |
|---|---|---|---|---|
| CH3COONH4 (cr) | -616.14[1] | – | – | – |
| CH3COONH4 (ai) | -618.52[1] | -448.61[1] | 200.0[1] | 73.6[1] |
| Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid
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 |
|---|---|---|---|---|
| Mn(CH3COO)2 (cr) | -1148.1[1] | – | – | – |
| Mn(CH3COO)2 (aq) | -1199.1[1] | – | – | – |
| Mn(CH3COO)2 (cr) 4 hydrate | -2338.0[1] | – | – | – |
| NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
| NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[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, (aq):Aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -616.14 kJ · mol−1
- ^ ΔfH°, -618.52 kJ · mol−1
- ^ ΔfG°, -448.61 kJ · mol−1
- ^ S°, 200.0 J · K−1 · mol−1
- ^ Cp°, 73.6 J · K−1 · mol−1
- ^ ΔfH°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, -1148.1 kJ · mol−1
- ^ ΔfH°, -1199.1 kJ · mol−1
- ^ ΔfH°, -2338.0 kJ · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 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