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HgS + 2H[AuCl4] → HgCl2 + 2AuCl3 + H2S↑

The reaction of mercury(II) sulfide and tetrachloridoauric(III) acid yields mercury(II) chloride, gold(III) chloride, and hydrogen sulfide. This reaction is an acid-base 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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HgSMercury(II) sulfide1
Brønsted base
Salt of weak acid
H[AuCl4]Tetrachloridoauric(III) acid2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
HgCl2Mercury(II) chloride1
Conjugate base
Salt of strong acid
AuCl3Gold(III) chloride2
Conjugate base
Salt of strong acid
H2SHydrogen sulfide1
Conjugate acid
Weak acid

Thermodynamic changes

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
HgS (cr)
red
-58.2[1]-50.6[1]82.4[1]48.41[1]
HgS (cr)
black
-53.6[1]-47.7[1]88.3[1]
HgS (g)254.75[1]
H[AuCl4]
* (cr):Crystalline solid, (g):Gas

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
HgCl2 (cr)-224.3[1]-178.6[1]146.0[1]
HgCl2 (ao)-216.3[1]-173.2[1]155[1]
AuCl3 (cr)-117.6[1]
AuCl3 (cr)
2 hydrate
-715.0[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]
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (g):Gas

References

List of references

  1. 1