MnSO4 + NaHS 💧→ MnS↓ + NaHSO4
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The reaction of manganese(II) sulfate and sodium hydrogensulfide yields manganese(II) sulfide and sodium hydrogensulfate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of manganese(II) sulfate and sodium 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) sulfate and sodium hydrogensulfide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| MnSO4 | Manganese(II) sulfate | 1 | Lewis acid | Very soluble in water |
| NaHS | Sodium hydrogensulfide | 1 | 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 |
| NaHSO4 | Sodium hydrogensulfate | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of manganese(II) sulfate and sodium hydrogensulfide
| 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 | −37.2 | – | – | – |
per 1 mol of | −37.2 | – | – | – |
per 1 mol of | −37.2 | – | – | – |
per 1 mol of | −37.2 | – | – | – |
per 1 mol of | −37.2 | – | – | – |
Changes in standard condition (2)
- Reaction of manganese(II) sulfate and sodium hydrogensulfide
| 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 | −36.8 | – | – | – |
per 1 mol of | −36.8 | – | – | – |
per 1 mol of | −36.8 | – | – | – |
per 1 mol of | −36.8 | – | – | – |
per 1 mol of | −36.8 | – | – | – |
Changes in aqueous solution (1)
- Reaction of manganese(II) sulfate and sodium hydrogensulfide◆
ΔrG −0.7 kJ/mol K 1.33 × 100 pK −0.12
| 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 | 32.0 | −0.7 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
Changes in aqueous solution (2)
- Reaction of manganese(II) sulfate and sodium hydrogensulfide◆
ΔrG −13.7 kJ/mol K 2.51 × 102 pK −2.40
| 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 | 46.2 | −13.7 | 200.8 | – |
per 1 mol of | 46.2 | −13.7 | 200.8 | – |
per 1 mol of | 46.2 | −13.7 | 200.8 | – |
per 1 mol of | 46.2 | −13.7 | 200.8 | – |
per 1 mol of | 46.2 | −13.7 | 200.8 | – |
Changes in aqueous solution (3)
- Reaction of manganese(II) sulfate and sodium hydrogensulfide◆
ΔrG −0.7 kJ/mol K 1.33 × 100 pK −0.12
| 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 | 32.0 | −0.7 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
per 1 mol of | 32.0 | −0.70 | 110.8 | – |
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 |
|---|---|---|---|---|
| MnSO4 (cr) | -1065.25[1] | -957.36[1] | 112.1[1] | 100.50[1] |
| MnSO4 (ai) | -1130.1[1] | -972.7[1] | -53.6[1] | -243[1] |
| MnSO4 (ao) | -1115.9[1] | -985.7[1] | 36.4[1] | – |
| MnSO4 (cr) 1 hydrate α | -1376.5[1] | – | – | – |
| MnSO4 (cr) 1 hydrate β | -1348.1[1] | – | – | – |
| MnSO4 (cr) 4 hydrate | -2258.1[1] | – | – | – |
| MnSO4 (cr) 5 hydrate | -2553.1[1] | – | – | 326[1] |
| MnSO4 (cr) 7 hydrate | -3139.3[1] | – | – | – |
| NaHS (cr) | -237.23[1] | – | – | – |
| NaHS (ai) | -257.73[1] | -249.81[1] | 121.8[1] | – |
| NaHS (cr) 2 hydrate | -838.47[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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] | – | – | – |
| NaHSO4 (cr) | -1125.5[1] | -992.8[1] | 113.0[1] | – |
| NaHSO4 (ai) | -1127.46[1] | -1017.80[1] | 190.8[1] | -38[1] |
| NaHSO4 (cr) 1 hydrate | -1421.7[1] | -1231.6[1] | 155[1] | – |
* (cr):Crystalline solid, (am):Amorphous 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°, -1065.25 kJ · mol−1
- ^ ΔfG°, -957.36 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 100.50 J · K−1 · mol−1
- ^ ΔfH°, -1130.1 kJ · mol−1
- ^ ΔfG°, -972.7 kJ · mol−1
- ^ S°, -53.6 J · K−1 · mol−1
- ^ Cp°, -243. J · K−1 · mol−1
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfG°, -985.7 kJ · mol−1
- ^ S°, 36.4 J · K−1 · mol−1
- ^ ΔfH°, -1376.5 kJ · mol−1
- ^ ΔfH°, -1348.1 kJ · mol−1
- ^ ΔfH°, -2258.1 kJ · mol−1
- ^ ΔfH°, -2553.1 kJ · mol−1
- ^ Cp°, 326. J · K−1 · mol−1
- ^ ΔfH°, -3139.3 kJ · mol−1
- ^ ΔfH°, -237.23 kJ · mol−1
- ^ ΔfH°, -257.73 kJ · mol−1
- ^ ΔfG°, -249.81 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -838.47 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°, -1125.5 kJ · mol−1
- ^ ΔfG°, -992.8 kJ · mol−1
- ^ S°, 113.0 J · K−1 · mol−1
- ^ ΔfH°, -1127.46 kJ · mol−1
- ^ ΔfG°, -1017.80 kJ · mol−1
- ^ S°, 190.8 J · K−1 · mol−1
- ^ Cp°, -38. J · K−1 · mol−1
- ^ ΔfH°, -1421.7 kJ · mol−1
- ^ ΔfG°, -1231.6 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1