Mn(CH3COO)2 + 2KHS 💧→ MnS↓ + 2CH3COOH + K2S
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The reaction of manganese(II) acetate and potassium hydrogensulfide yields manganese(II) sulfide, acetic acid, and potassium sulfide (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 manganese(II) acetate and potassium hydrogensulfide
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 manganese(II) acetate and potassium hydrogensulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Mn(CH3COO)2 | Manganese(II) acetate | 1 | Lewis acid | Very soluble in water |
| KHS | Potassium hydrogensulfide | 2 | Lewis base | Soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnS | Manganese(II) sulfide | 1 | Lewis conjugate | Insoluble in water |
| CH3COOH | Acetic acid | 2 | Non-redox product | – |
| K2S | Potassium sulfide | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of manganese(II) acetate and potassium hydrogensulfide
- Mn(CH3COO)2Crystalline solid + 2KHSCrystalline solidMnS↓Crystalline solidgreen + 2CH3COOHLiquid + K2SCrystalline solid💧⟶
| 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 | 114.4 | – | – | – |
per 1 mol of | 114.4 | – | – | – |
per 1 mol of | 57.20 | – | – | – |
per 1 mol of | 114.4 | – | – | – |
per 1 mol of | 57.20 | – | – | – |
per 1 mol of | 114.4 | – | – | – |
Changes in standard condition (2)
- Reaction of manganese(II) acetate and potassium hydrogensulfide
- Mn(CH3COO)2Crystalline solid + 2KHSCrystalline solidMnS↓Amorphous solidprecipitated, pink + 2CH3COOHLiquid + K2SCrystalline solid💧⟶
| 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 | 114.8 | – | – | – |
per 1 mol of | 114.8 | – | – | – |
per 1 mol of | 57.40 | – | – | – |
per 1 mol of | 114.8 | – | – | – |
per 1 mol of | 57.40 | – | – | – |
per 1 mol of | 114.8 | – | – | – |
Changes in aqueous solution (1)
- Reaction of manganese(II) acetate and potassium hydrogensulfide
- Mn(CH3COO)2Aqueous solution + 2KHSIonized aqueous solutionMnS↓Crystalline solidgreen + 2CH3COOHUn-ionized aqueous solution + K2SIonized 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 | 81.7 | – | – | – |
per 1 mol of | 81.7 | – | – | – |
per 1 mol of | 40.9 | – | – | – |
per 1 mol of | 81.7 | – | – | – |
per 1 mol of | 40.9 | – | – | – |
per 1 mol of | 81.7 | – | – | – |
Changes in aqueous solution (2)
- Reaction of manganese(II) acetate and potassium hydrogensulfide
- Mn(CH3COO)2Aqueous solution + 2KHSIonized aqueous solutionMnS↓Crystalline solidgreen + 2CH3COOHIonized aqueous solution + K2SIonized 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 | 81.2 | – | – | – |
per 1 mol of | 81.2 | – | – | – |
per 1 mol of | 40.6 | – | – | – |
per 1 mol of | 81.2 | – | – | – |
per 1 mol of | 40.6 | – | – | – |
per 1 mol of | 81.2 | – | – | – |
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 |
|---|---|---|---|---|
| Mn(CH3COO)2 (cr) | -1148.1[1] | – | – | – |
| Mn(CH3COO)2 (aq) | -1199.1[1] | – | – | – |
| Mn(CH3COO)2 (cr) 4 hydrate | -2338.0[1] | – | – | – |
| KHS (cr) | -265.10[1] | – | – | 75.31[1] |
| KHS (ai) | -269.9[1] | -271.19[1] | 165.3[1] | – |
| KHS (cr) 0.25 hydrate | -337.2[1] | – | – | – |
* (cr):Crystalline solid, (aq):Aqueous solution, (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 |
|---|---|---|---|---|
| MnS (cr) green | -214.2[1] | -218.4[1] | 78.2[1] | 49.96[1] |
| MnS (am) precipitated, pink | -213.8[1] | – | – | – |
| CH3COOH (l) | -484.5[1] | -389.9[1] | 159.8[1] | 124.3[1] |
| CH3COOH (g) | -432.25[1] | -374.0[1] | 282.5[1] | 66.5[1] |
| CH3COOH (ai) | -486.01[1] | -369.31[1] | 86.6[1] | -6.3[1] |
| CH3COOH (ao) | -485.76[1] | -396.46[1] | 178.7[1] | – |
| K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
| K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
| K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
| K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
* (cr):Crystalline solid, (am):Amorphous solid, (l):Liquid, (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°, -1148.1 kJ · mol−1
- ^ ΔfH°, -1199.1 kJ · mol−1
- ^ ΔfH°, -2338.0 kJ · mol−1
- ^ ΔfH°, -265.10 kJ · mol−1
- ^ Cp°, 75.31 J · K−1 · mol−1
- ^ ΔfH°, -269.9 kJ · mol−1
- ^ ΔfG°, -271.19 kJ · mol−1
- ^ S°, 165.3 J · K−1 · mol−1
- ^ ΔfH°, -337.2 kJ · mol−1
- ^ ΔfH°, -214.2 kJ · mol−1
- ^ ΔfG°, -218.4 kJ · mol−1
- ^ S°, 78.2 J · K−1 · mol−1
- ^ Cp°, 49.96 J · K−1 · mol−1
- ^ ΔfH°, -213.8 kJ · mol−1
- ^ ΔfH°, -484.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 159.8 J · K−1 · mol−1
- ^ Cp°, 124.3 J · K−1 · mol−1
- ^ ΔfH°, -432.25 kJ · mol−1
- ^ ΔfG°, -374.0 kJ · mol−1
- ^ S°, 282.5 J · K−1 · mol−1
- ^ Cp°, 66.5 J · K−1 · mol−1
- ^ ΔfH°, -486.01 kJ · mol−1
- ^ ΔfG°, -369.31 kJ · mol−1
- ^ S°, 86.6 J · K−1 · mol−1
- ^ Cp°, -6.3 J · K−1 · mol−1
- ^ ΔfH°, -485.76 kJ · mol−1
- ^ ΔfG°, -396.46 kJ · mol−1
- ^ S°, 178.7 J · K−1 · mol−1
- ^ ΔfH°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1