2H2S + PbO2 → S + PbS + 2H2O
Last updated:
- Reaction of hydrogen sulfide and lead(IV) oxide
The reaction of hydrogen sulfide and lead(IV) oxide yields , lead(II) sulfide, 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 lead(IV) oxide
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen sulfide and lead(IV) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 2 | Reducing | Reducing |
| PbO2 | Lead(IV) oxide | 1 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Oxidized | – | ||
| PbS | Lead(II) sulfide | 1 | Reduced | – |
| H2O | Water | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen sulfide and lead(IV) oxide◆
ΔrG −288.5 kJ/mol K 3.49 × 1050 pK −50.54
| 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 | −353.4 | −288.5 | −217.4 | 89.62 |
per 1 mol of | −176.7 | −144.3 | −108.7 | 44.81 |
per 1 mol of | −353.4 | −288.5 | −217.4 | 89.62 |
| −353.4 | −288.5 | −217.4 | 89.62 | |
per 1 mol of | −353.4 | −288.5 | −217.4 | 89.62 |
per 1 mol of | −176.7 | −144.3 | −108.7 | 44.81 |
Changes in standard condition (2)
- Reaction of hydrogen sulfide and lead(IV) oxide
| 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 | −353.1 | – | – | – |
per 1 mol of | −176.6 | – | – | – |
per 1 mol of | −353.1 | – | – | – |
| −353.1 | – | – | – | |
per 1 mol of | −353.1 | – | – | – |
per 1 mol of | −176.6 | – | – | – |
Changes in aqueous solution
- Reaction of hydrogen sulfide and lead(IV) oxide◆
ΔrG −300.0 kJ/mol K 3.61 × 1052 pK −52.56
| 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 | −315.3 | −300.0 | −48 | – |
per 1 mol of | −157.7 | −150.0 | −24 | – |
per 1 mol of | −315.3 | −300.0 | −48 | – |
| −315.3 | −300.0 | −48 | – | |
per 1 mol of | −315.3 | −300.0 | −48 | – |
per 1 mol of | −157.7 | −150.0 | −24 | – |
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] | – |
| PbO2 (cr) | -277.4[1] | -217.33[1] | 68.6[1] | 64.64[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 |
|---|---|---|---|---|
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| PbS (cr) | -100.4[1] | -98.7[1] | 91.2[1] | 49.50[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, (g):Gas, (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°, -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°, -277.4 kJ · mol−1
- ^ ΔfG°, -217.33 kJ · mol−1
- ^ S°, 68.6 J · K−1 · mol−1
- ^ Cp°, 64.64 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -100.4 kJ · mol−1
- ^ ΔfG°, -98.7 kJ · mol−1
- ^ S°, 91.2 J · K−1 · mol−1
- ^ Cp°, 49.50 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