You-iggy
  1. Home
  2. Chemical reactions
  3. H2S + Sr(CH3COO)2 → SrSO4 + 2CH4 + 2C

H2S + Sr(CH3COO)2 → SrSO4 + 2CH4 + 2C

Last updated:
Reaction of hydrogen sulfide and strontium acetate
H2SHydrogen sulfide + Sr(CH3COO)2Strontium acetate
⟶
SrSO4Strontium sulfate + 2CH4Methane + 2CCarbon

The reaction of hydrogen sulfide and strontium acetate yields strontium sulfate, methane, and carbon (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

Reaction of hydrogen sulfide and strontium acetate
H2SHydrogen sulfide + Sr(CH3COO)2Strontium acetate
⟶
SrSO4Strontium sulfate + 2CH4Methane + 2CCarbon

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 strontium acetate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2SHydrogen sulfide1
Reducing
Reducing
Sr(CH3COO)2Strontium acetate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SrSO4Strontium sulfate1
Oxidized
–
CH4Methane2
Reduced
–
CCarbon2
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and strontium acetate
H2SGas + Sr(CH3COO)2Crystalline solid
⟶
SrSO4Crystalline solid + 2CH4Gas + 2CCrystalline solidgraphite
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
−94.7–––
per 1 mol of
−94.7–––
per 1 mol of
−94.7–––
per 1 mol of
−94.7–––
per 1 mol of
−47.4–––
per 1 mol of
−47.4–––

Changes in standard condition (2)

Reaction of hydrogen sulfide and strontium acetate
H2SGas + Sr(CH3COO)2Crystalline solid
⟶
SrSO4Crystalline solid + 2CH4Gas + 2CCrystalline soliddiamond
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
−90.9–––
per 1 mol of
−90.9–––
per 1 mol of
−90.9–––
per 1 mol of
−90.9–––
per 1 mol of
−45.5–––
per 1 mol of
−45.5–––

Changes in standard condition (3)

Reaction of hydrogen sulfide and strontium acetate
H2SGas + Sr(CH3COO)2Crystalline solid
⟶
SrSO4Crystalline solidprecipitated + 2CH4Gas + 2CCrystalline solidgraphite
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
−91.4–––
per 1 mol of
−91.4–––
per 1 mol of
−91.4–––
per 1 mol of
−91.4–––
per 1 mol of
−45.7–––
per 1 mol of
−45.7–––

Changes in standard condition (4)

Reaction of hydrogen sulfide and strontium acetate
H2SGas + Sr(CH3COO)2Crystalline solid
⟶
SrSO4Crystalline solidprecipitated + 2CH4Gas + 2CCrystalline soliddiamond
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
−87.6–––
per 1 mol of
−87.6–––
per 1 mol of
−87.6–––
per 1 mol of
−87.6–––
per 1 mol of
−43.8–––
per 1 mol of
−43.8–––

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and strontium acetate
H2SUn-ionized aqueous solution + Sr(CH3COO)2Aqueous solution
⟶
SrSO4Crystalline solid + 2CH4Gas + 2CCrystalline solidgraphite
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
−50.9–––
per 1 mol of
−50.9–––
per 1 mol of
−50.9–––
per 1 mol of
−50.9–––
per 1 mol of
−25.4–––
per 1 mol of
−25.4–––

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and strontium acetate
H2SUn-ionized aqueous solution + Sr(CH3COO)2Aqueous solution
⟶
SrSO4Crystalline solid + 2CH4Un-ionized aqueous solution + 2CCrystalline solidgraphite
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
−79.4–––
per 1 mol of
−79.4–––
per 1 mol of
−79.4–––
per 1 mol of
−79.4–––
per 1 mol of
−39.7–––
per 1 mol of
−39.7–––

Changes in aqueous solution (3)

Reaction of hydrogen sulfide and strontium acetate
H2SUn-ionized aqueous solution + Sr(CH3COO)2Aqueous solution
⟶
SrSO4Crystalline solidprecipitated + 2CH4Gas + 2CCrystalline solidgraphite
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
−47.6–––
per 1 mol of
−47.6–––
per 1 mol of
−47.6–––
per 1 mol of
−47.6–––
per 1 mol of
−23.8–––
per 1 mol of
−23.8–––

Changes in aqueous solution (4)

Reaction of hydrogen sulfide and strontium acetate
H2SUn-ionized aqueous solution + Sr(CH3COO)2Aqueous solution
⟶
SrSO4Crystalline solidprecipitated + 2CH4Un-ionized aqueous solution + 2CCrystalline solidgraphite
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
−76.1–––
per 1 mol of
−76.1–––
per 1 mol of
−76.1–––
per 1 mol of
−76.1–––
per 1 mol of
−38.0–––
per 1 mol of
−38.0–––

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]–
Sr(CH3COO)2 (cr)-1487.4[1]–––
Sr(CH3COO)2 (aq)-1512.1[1]–––
Sr(CH3COO)2 (cr)
0.5 hydrate
-1631.8[1]–––
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (aq):Aqueous solution

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
SrSO4 (cr)-1453.1[1]-1340.9[1]117[1]–
SrSO4 (cr)
precipitated
-1449.8[1]–––
SrSO4 (ai)-1455.07[1]-1304.00[1]-12.6[1]–
CH4 (g)-74.81[1]-50.72[1]186.264[1]35.309[1]
CH4 (ao)-89.04[1]-34.33[1]83.7[1]–
C (cr)
graphite
0[1]0[1]5.740[1]8.527[1]
C (cr)
diamond
1.895[1]2.900[1]2.377[1]6.113[1]
C (g)716.682[1]671.257[1]158.096[1]20.838[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)