9H2S + 3Ba3(PO4)2 → 5BaSO3 + 6P + 4BaS + 9H2O
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- Reaction of hydrogen sulfide and barium phosphate
The reaction of hydrogen sulfide and barium phosphate yields barium sulfite, , barium 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 barium phosphate
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 barium phosphate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 9 | Reducing | Reducing |
| Ba3(PO4)2 | Barium phosphate | 3 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaSO3 | Barium sulfite | 5 | Oxidized | – |
| 6 | Reduced | – | ||
| BaS | Barium sulfide | 4 | – | – |
| H2O | Water | 9 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen sulfide and barium phosphate
| 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 | 2152 | – | – | – |
per 1 mol of | 239.1 | – | – | – |
per 1 mol of | 717.3 | – | – | – |
per 1 mol of | 430.4 | – | – | – |
| 358.7 | – | – | – | |
per 1 mol of | 538.0 | – | – | – |
per 1 mol of | 239.1 | – | – | – |
Changes in standard condition (2)
- Reaction of hydrogen sulfide and barium phosphate
| 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 | 2046 | – | – | – |
per 1 mol of | 227.3 | – | – | – |
per 1 mol of | 682.0 | – | – | – |
per 1 mol of | 409.2 | – | – | – |
| 341.0 | – | – | – | |
per 1 mol of | 511.5 | – | – | – |
per 1 mol of | 227.3 | – | – | – |
Changes in standard condition (3)
- Reaction of hydrogen sulfide and barium phosphate
| 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 | 1916 | – | – | – |
per 1 mol of | 212.9 | – | – | – |
per 1 mol of | 638.7 | – | – | – |
per 1 mol of | 383.2 | – | – | – |
| 319.3 | – | – | – | |
per 1 mol of | 479.0 | – | – | – |
per 1 mol of | 212.9 | – | – | – |
Changes in standard condition (4)
- Reaction of hydrogen sulfide and barium phosphate
| 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 | 2107 | – | – | – |
per 1 mol of | 234.1 | – | – | – |
per 1 mol of | 702.3 | – | – | – |
per 1 mol of | 421.4 | – | – | – |
| 351.2 | – | – | – | |
per 1 mol of | 526.8 | – | – | – |
per 1 mol of | 234.1 | – | – | – |
Changes in aqueous solution
- Reaction of hydrogen sulfide and barium phosphate
| 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 | 2190 | – | – | – |
per 1 mol of | 243.3 | – | – | – |
per 1 mol of | 730.0 | – | – | – |
per 1 mol of | 438.0 | – | – | – |
| 365.0 | – | – | – | |
per 1 mol of | 547.5 | – | – | – |
per 1 mol of | 243.3 | – | – | – |
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] | – |
| Ba3(PO4)2 (cr) | -4092[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 |
|---|---|---|---|---|
| BaSO3 (cr) | -1179.5[1] | – | – | – |
| (cr) white | 0[1] | 0[1] | 41.09[1] | 23.84[1] |
| (cr) red, triclinic | -17.6[1] | -12.1[1] | 22.80[1] | 21.21[1] |
| (cr) black | -39.3[1] | – | – | – |
| (am) red | -7.5[1] | – | – | – |
| (g) | 314.64[1] | 278.25[1] | 163.193[1] | 20.786[1] |
| BaS (cr) | -460[1] | -456[1] | 78.2[1] | 49.37[1] |
| BaS (g) | 50[1] | – | – | – |
| BaS (aq) | -493.3[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, (am):Amorphous solid, (g):Gas, (aq):Aqueous solution, (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°, -4092. kJ · mol−1
- ^ ΔfH°, -1179.5 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 41.09 J · K−1 · mol−1
- ^ Cp°, 23.84 J · K−1 · mol−1
- ^ ΔfH°, -17.6 kJ · mol−1
- ^ ΔfG°, -12.1 kJ · mol−1
- ^ S°, 22.80 J · K−1 · mol−1
- ^ Cp°, 21.21 J · K−1 · mol−1
- ^ ΔfH°, -39.3 kJ · mol−1
- ^ ΔfH°, -7.5 kJ · mol−1
- ^ ΔfH°, 314.64 kJ · mol−1
- ^ ΔfG°, 278.25 kJ · mol−1
- ^ S°, 163.193 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, -460. kJ · mol−1
- ^ ΔfG°, -456. kJ · mol−1
- ^ S°, 78.2 J · K−1 · mol−1
- ^ Cp°, 49.37 J · K−1 · mol−1
- ^ ΔfH°, 50. kJ · mol−1
- ^ ΔfH°, -493.3 kJ · 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