ZnSO4 + KHS 💧→ ZnS↓ + KHSO4
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The reaction of zinc sulfate and potassium hydrogensulfide yields zinc sulfide and potassium hydrogensulfate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of zinc sulfate 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 zinc sulfate and potassium hydrogensulfide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
ZnSO4 | Zinc sulfate | 1 | Lewis acid | Very soluble in water |
KHS | Potassium hydrogensulfide | 1 | Lewis base | Soluble in water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
ZnS | Zinc sulfide | 1 | Lewis conjugate | Insoluble in water |
KHSO4 | Potassium hydrogensulfate | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of zinc sulfate and potassium 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 | −118.7 | – | – | – |
per 1 mol of | −118.7 | – | – | – |
per 1 mol of | −118.7 | – | – | – |
per 1 mol of | −118.7 | – | – | – |
per 1 mol of | −118.7 | – | – | – |
Changes in aqueous solution (1)
- Reaction of zinc sulfate and potassium hydrogensulfide◆
ΔrG −64.4 kJ/mol K 1.92 × 1011 pK −11.28
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 | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
Changes in aqueous solution (2)
- Reaction of zinc sulfate and potassium hydrogensulfide◆
ΔrG −77.69 kJ/mol K 4.08 × 1013 pK −13.61
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 | −12.6 | −77.69 | 218.7 | – |
per 1 mol of | −12.6 | −77.69 | 218.7 | – |
per 1 mol of | −12.6 | −77.69 | 218.7 | – |
per 1 mol of | −12.6 | −77.69 | 218.7 | – |
per 1 mol of | −12.6 | −77.69 | 218.7 | – |
Changes in aqueous solution (3)
- Reaction of zinc sulfate and potassium hydrogensulfide◆
ΔrG −64.4 kJ/mol K 1.92 × 1011 pK −11.28
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 | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
per 1 mol of | −28.1 | −64.4 | 121.7 | – |
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 |
---|---|---|---|---|
ZnSO4 (cr) | -982.8[1] | -871.5[1] | 110.5[1] | 99.2[1] |
ZnSO4 (ai) | -1063.15[1] | -891.59[1] | -92.0[1] | -247[1] |
ZnSO4 (ao) | -1047.7[1] | -904.9[1] | 5.0[1] | – |
ZnSO4 (cr) 1 hydrate | -1304.49[1] | -1131.99[1] | 138.5[1] | – |
ZnSO4 (cr) 6 hydrate | -2777.46[1] | -2324.44[1] | 363.6[1] | 357.69[1] |
ZnSO4 (cr) 7 hydrate | -3077.75[1] | -2562.67[1] | 388.7[1] | 383.42[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, (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 |
---|---|---|---|---|
ZnS (cr) | -205.98[1] | -201.29[1] | 57.7[1] | 46.0[1] |
KHSO4 (cr) | -1160.6[1] | -1031.3[1] | 138.1[1] | – |
KHSO4 (ai) | -1139.72[1] | -1039.18[1] | 234.3[1] | -63[1] |
* (cr):Crystalline 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°, -982.8 kJ · mol−1
- ^ ΔfG°, -871.5 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, -1063.15 kJ · mol−1
- ^ ΔfG°, -891.59 kJ · mol−1
- ^ S°, -92.0 J · K−1 · mol−1
- ^ Cp°, -247. J · K−1 · mol−1
- ^ ΔfH°, -1047.7 kJ · mol−1
- ^ ΔfG°, -904.9 kJ · mol−1
- ^ S°, 5.0 J · K−1 · mol−1
- ^ ΔfH°, -1304.49 kJ · mol−1
- ^ ΔfG°, -1131.99 kJ · mol−1
- ^ S°, 138.5 J · K−1 · mol−1
- ^ ΔfH°, -2777.46 kJ · mol−1
- ^ ΔfG°, -2324.44 kJ · mol−1
- ^ S°, 363.6 J · K−1 · mol−1
- ^ Cp°, 357.69 J · K−1 · mol−1
- ^ ΔfH°, -3077.75 kJ · mol−1
- ^ ΔfG°, -2562.67 kJ · mol−1
- ^ S°, 388.7 J · K−1 · mol−1
- ^ Cp°, 383.42 J · K−1 · 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°, -205.98 kJ · mol−1
- ^ ΔfG°, -201.29 kJ · mol−1
- ^ S°, 57.7 J · K−1 · mol−1
- ^ Cp°, 46.0 J · K−1 · mol−1
- ^ ΔfH°, -1160.6 kJ · mol−1
- ^ ΔfG°, -1031.3 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1139.72 kJ · mol−1
- ^ ΔfG°, -1039.18 kJ · mol−1
- ^ S°, 234.3 J · K−1 · mol−1
- ^ Cp°, -63. J · K−1 · mol−1