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5H2S + 3MgCO3 🔥→ 2SO2 + 3MgS + 5H2O + 3C

The reaction of hydrogen sulfide and magnesium carbonate yields sulfur dioxide, magnesium sulfide, water, 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

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 sulfide5
Reducing
Reducing
MgCO3Magnesium carbonate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SO2Sulfur dioxide2
Oxidized
MgSMagnesium sulfide3
H2OWater5
CCarbon3
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and magnesium carbonate
ΔrG392.7 kJ/mol
K0.16 × 10−68
pK68.80
5H2SGas + 3MgCO3Crystalline solid
🔥
2SO2Gas + 3MgSCrystalline solid + 5H2OLiquid + 3CCrystalline 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
329.7392.7−211.9220.75
per 1 mol of
65.9478.54−42.3844.150
109.9130.9−70.6373.583
per 1 mol of
164.8196.3−106.0110.38
per 1 mol of
109.9130.9−70.6373.583
per 1 mol of
65.9478.54−42.3844.150
per 1 mol of
109.9130.9−70.6373.583

Changes in standard condition (2)

Reaction of hydrogen sulfide and magnesium carbonate
ΔrG401.4 kJ/mol
K0.48 × 10−70
pK70.32
5H2SGas + 3MgCO3Crystalline solid
🔥
2SO2Gas + 3MgSCrystalline solid + 5H2OLiquid + 3CCrystalline 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
335.4401.4−221.9213.50
per 1 mol of
67.0880.28−44.3842.700
111.8133.8−73.9771.167
per 1 mol of
167.7200.7−111.0106.75
per 1 mol of
111.8133.8−73.9771.167
per 1 mol of
67.0880.28−44.3842.700
per 1 mol of
111.8133.8−73.9771.167

Changes in aqueous solution (1)

Reaction of hydrogen sulfide and magnesium carbonate
ΔrG364.0 kJ/mol
K0.17 × 10−63
pK63.77
5H2SUn-ionized aqueous solution + 3MgCO3Crystalline solid
🔥
2SO2Gas + 3MgSCrystalline solid + 5H2OLiquid + 3CCrystalline 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
425.1364.0212
per 1 mol of
85.0272.8042.4
141.7121.370.7
per 1 mol of
212.6182.0106
per 1 mol of
141.7121.370.7
per 1 mol of
85.0272.8042.4
per 1 mol of
141.7121.370.7

Changes in aqueous solution (2)

Reaction of hydrogen sulfide and magnesium carbonate
ΔrG363.1 kJ/mol
K0.24 × 10−63
pK63.61
5H2SUn-ionized aqueous solution + 3MgCO3Crystalline solid
🔥
2SO2Un-ionized aqueous solution + 3MgSCrystalline solid + 5H2OLiquid + 3CCrystalline 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
372.8363.139
per 1 mol of
74.5672.627.8
124.3121.013
per 1 mol of
186.4181.620
per 1 mol of
124.3121.013
per 1 mol of
74.5672.627.8
per 1 mol of
124.3121.013

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]
MgCO3 (cr)-1095.8[1]-1012.1[1]65.7[1]75.52[1]
MgCO3 (cr)
3 hydrate
-1726.1[1]
MgCO3 (cr)
5 hydrate
-2199.2[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
SO2 (l)-320.5[1]
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[1]
MgS (cr)-346.0[1]-341.8[1]50.33[1]45.56[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]
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]
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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)