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3H2S + 2Au(OH)3 → 3S + 2Au + 6H2O

The reaction of hydrogen sulfide and gold(III) hydroxide yields sulfur, gold, and water. 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 categories

Reaction data

Chemical equation

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide3
Reducing
Reducing
Au(OH)3Gold(III) hydroxide2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SSulfur3
Oxidized
AuGold2
Reduced
H2OWater6

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and gold(III) hydroxide
ΔrG−688.25 kJ/mol
K3.77 × 10120
pK−120.58
3H2SGas + 2Au(OH)3Crystalline solidprecipitated
3SCrystalline solidrhombic + 2AuCrystalline solid + 6H2OLiquid
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
−803.7−688.25−386.7
per 1 mol of
−267.9−229.42−128.9
−401.9−344.13−193.3
per 1 mol of
−267.9−229.42−128.9
per 1 mol of
−401.9−344.13−193.3
per 1 mol of
−134.0−114.71−64.45

Changes in standard condition (2)

Reaction of hydrogen sulfide and gold(III) hydroxide
3H2SGas + 2Au(OH)3Crystalline solidprecipitated
3SCrystalline solidmonoclinic + 2AuCrystalline solid + 6H2OLiquid
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
−802.7
per 1 mol of
−267.6
−401.4
per 1 mol of
−267.6
per 1 mol of
−401.4
per 1 mol of
−133.8

Changes in aqueous solution

Reaction of hydrogen sulfide and gold(III) hydroxide
ΔrG−772.54 kJ/mol
K2.20 × 10135
pK−135.34
3H2SUn-ionized aqueous solution + 2Au(OH)3Un-ionized aqueous solution
3SCrystalline solidrhombic + 2AuCrystalline solid + 6H2OLiquid
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
−772.54
per 1 mol of
−257.51
−386.27
per 1 mol of
−257.51
per 1 mol of
−386.27
per 1 mol of
−128.76

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]
Au(OH)3 (cr)
precipitated
-424.7[1]-316.92[1]189.5[1]
Au(OH)3 (ao)-283.37[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
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
Au (cr)0[1]0[1]47.40[1]25.418[1]
Au (g)366.1[1]326.3[1]180.503[1]20.786[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

  1. 1