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14H2S + 3Ba3(PO4)2 → 5H2SO3 + 6P + 9BaS + 9H2O

The reaction of hydrogen sulfide and barium phosphate yields sulfurous acid, phosphorus, barium sulfide, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide14
Reducing
Reducing
Ba3(PO4)2Barium phosphate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2SO3Sulfurous acid5
Oxidized
PPhosphorus6
Reduced
BaSBarium sulfide9
H2OWater9

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen sulfide and barium phosphate
14H2SUn-ionized aqueous solution + 3Ba3(PO4)2Crystalline solid
5H2SO3Un-ionized aqueous solution + 6PCrystalline solidwhite + 9BaSAqueous solution + 9H2OLiquid
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
2776
per 1 mol of
198.3
per 1 mol of
925.3
per 1 mol of
555.2
per 1 mol of
462.7
per 1 mol of
308.4
per 1 mol of
308.4

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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
H2SO3 (ao)-608.81[1]-537.81[1]232.2[1]
P (cr)
white
0[1]0[1]41.09[1]23.84[1]
P (cr)
red, triclinic
-17.6[1]-12.1[1]22.80[1]21.21[1]
P (cr)
black
-39.3[1]
P (am)
red
-7.5[1]
P (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]
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (aq):Aqueous solution, (l):Liquid

References

List of references

  1. 1