2H2S + 3HgSO4 🔥→ 5SO2 + 3Hg + 2H2O
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- Reaction of hydrogen sulfide and mercury(II) sulfate
The reaction of hydrogen sulfide and mercury(II) sulfate yields sulfur dioxide, , and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen sulfide and mercury(II) sulfate
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen sulfide and mercury(II) sulfate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 2 | Reducing | Reducing |
HgSO4 | Mercury(II) sulfate | 3 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SO2 | Sulfur dioxide | 5 | Redoxed product | – |
3 | Reduced | – | ||
H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and mercury(II) sulfate
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 | 108.0 | – | – | – |
per 1 mol of | 54.00 | – | – | – |
per 1 mol of | 36.00 | – | – | – |
per 1 mol of | 21.60 | – | – | – |
36.00 | – | – | – | |
per 1 mol of | 54.00 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and mercury(II) sulfate◆
ΔrG −37.1 kJ/mol K 3.16 × 106 pK −6.50
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 | – | −37.1 | – | – |
per 1 mol of | – | −18.6 | – | – |
per 1 mol of | – | −12.4 | – | – |
per 1 mol of | – | −7.42 | – | – |
– | −12.4 | – | – | |
per 1 mol of | – | −18.6 | – | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and mercury(II) sulfate◆
ΔrG −39.5 kJ/mol K 8.32 × 106 pK −6.92
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 | – | −39.5 | – | – |
per 1 mol of | – | −19.8 | – | – |
per 1 mol of | – | −13.2 | – | – |
per 1 mol of | – | −7.90 | – | – |
– | −13.2 | – | – | |
per 1 mol of | – | −19.8 | – | – |
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 |
---|---|---|---|---|
H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
HgSO4 (cr) | -707.5[1] | – | – | – |
HgSO4 (ao) | – | -588.2[1] | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline 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 |
---|---|---|---|---|
SO2 (l) | -320.5[1] | – | – | – |
SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[1] | – |
(cr) | – | – | – | – |
(l) | 0[1] | 0[1] | 76.02[1] | 27.983[1] |
(g) | 61.317[1] | 31.820[1] | 174.96[1] | 20.786[1] |
(ao) | 37.7[1] | 39.3[1] | 71[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] |
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, -707.5 kJ · mol−1
- ^ ΔfG°, -588.2 kJ · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 76.02 J · K−1 · mol−1
- ^ Cp°, 27.983 J · K−1 · mol−1
- ^ ΔfH°, 61.317 kJ · mol−1
- ^ ΔfG°, 31.820 kJ · mol−1
- ^ S°, 174.96 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 37.7 kJ · mol−1
- ^ ΔfG°, 39.3 kJ · mol−1
- ^ S°, 71. 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