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11H2S + 6NaHCO3 🔥→ 2H2SO3 + 6SO2 + 3Na2S + 6CH4

The reaction of hydrogen sulfide and sodium hydrogencarbonate yields sulfurous acid, sulfur dioxide, sodium sulfide, and methane (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 sulfide11
Reducing
Reducing
NaHCO3Sodium hydrogencarbonate6
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
H2SO3Sulfurous acid2
Oxidized
SO2Sulfur dioxide6
Oxidized
Na2SSodium sulfide3
CH4Methane6
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG902.7 kJ/mol
K0.71 × 10−158
pK158.15
11H2SUn-ionized aqueous solution + 6NaHCO3Ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Gas + 3Na2SIonized aqueous solution + 6CH4Gas
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
1240.0902.71149
per 1 mol of
112.7382.06104.5
206.67150.5191.5
per 1 mol of
620.00451.4574.5
per 1 mol of
206.67150.5191.5
per 1 mol of
413.33300.9383.0
per 1 mol of
206.67150.5191.5

Changes in standard condition (2)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG1001.0 kJ/mol
K0.43 × 10−175
pK175.37
11H2SUn-ionized aqueous solution + 6NaHCO3Ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Gas + 3Na2SIonized aqueous solution + 6CH4Un-ionized aqueous solution
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
1154.61001.0534
per 1 mol of
104.9691.00048.5
192.43166.8389.0
per 1 mol of
577.30500.50267
per 1 mol of
192.43166.8389.0
per 1 mol of
384.87333.67178
per 1 mol of
192.43166.8389.0

Changes in standard condition (3)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG899.8 kJ/mol
K0.23 × 10−157
pK157.64
11H2SUn-ionized aqueous solution + 6NaHCO3Ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Un-ionized aqueous solution + 3Na2SIonized aqueous solution + 6CH4Gas
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
1083.1899.8631
per 1 mol of
98.46481.8057.4
180.52150.0105
per 1 mol of
541.55449.9316
per 1 mol of
180.52150.0105
per 1 mol of
361.03299.9210
per 1 mol of
180.52150.0105

Changes in standard condition (4)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG998.1 kJ/mol
K0.14 × 10−174
pK174.86
11H2SUn-ionized aqueous solution + 6NaHCO3Ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Un-ionized aqueous solution + 3Na2SIonized aqueous solution + 6CH4Un-ionized aqueous solution
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
997.7998.116
per 1 mol of
90.7090.741.5
166.3166.32.7
per 1 mol of
498.9499.18.0
per 1 mol of
166.3166.32.7
per 1 mol of
332.6332.75.3
per 1 mol of
166.3166.32.7

Changes in standard condition (5)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG908.9 kJ/mol
K0.59 × 10−159
pK159.23
11H2SUn-ionized aqueous solution + 6NaHCO3Un-ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Gas + 3Na2SIonized aqueous solution + 6CH4Gas
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
1310.7908.91367
per 1 mol of
119.1582.63124.3
218.45151.5227.8
per 1 mol of
655.35454.4683.5
per 1 mol of
218.45151.5227.8
per 1 mol of
436.90303.0455.7
per 1 mol of
218.45151.5227.8

Changes in standard condition (6)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG1007.3 kJ/mol
K0.34 × 10−176
pK176.47
11H2SUn-ionized aqueous solution + 6NaHCO3Un-ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Gas + 3Na2SIonized aqueous solution + 6CH4Un-ionized aqueous solution
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
1225.41007.3752
per 1 mol of
111.4091.57368.4
204.23167.88125
per 1 mol of
612.70503.65376
per 1 mol of
204.23167.88125
per 1 mol of
408.47335.77251
per 1 mol of
204.23167.88125

Changes in standard condition (7)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG906.0 kJ/mol
K0.19 × 10−158
pK158.72
11H2SUn-ionized aqueous solution + 6NaHCO3Un-ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Un-ionized aqueous solution + 3Na2SIonized aqueous solution + 6CH4Gas
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
1153.8906.0849
per 1 mol of
104.8982.3677.2
192.30151.0142
per 1 mol of
576.90453.0425
per 1 mol of
192.30151.0142
per 1 mol of
384.60302.0283
per 1 mol of
192.30151.0142

Changes in standard condition (8)

Reaction of hydrogen sulfide and sodium hydrogencarbonate
ΔrG1004.4 kJ/mol
K0.11 × 10−175
pK175.96
11H2SUn-ionized aqueous solution + 6NaHCO3Un-ionized aqueous solution
🔥
2H2SO3Un-ionized aqueous solution + 6SO2Un-ionized aqueous solution + 3Na2SIonized aqueous solution + 6CH4Un-ionized aqueous solution
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
1068.51004.4234
per 1 mol of
97.13691.30921.3
178.08167.4039.0
per 1 mol of
534.25502.20117
per 1 mol of
178.08167.4039.0
per 1 mol of
356.17334.8078.0
per 1 mol of
178.08167.4039.0

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]
NaHCO3 (cr)-950.81[1]-851.0[1]101.7[1]87.61[1]
NaHCO3 (ai)-932.11[1]-848.66[1]150.2[1]
NaHCO3 (ao)-943.9[1]-849.7[1]113.8[1]
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized 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
H2SO3 (ao)-608.81[1]-537.81[1]232.2[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]
Na2S (cr)-364.8[1]-349.8[1]83.7[1]
Na2S (ai)-447.3[1]-438.1[1]103.3[1]
Na2S (cr)
4.5 hydrate
-1725.9[1]
Na2S (cr)
5 hydrate
-1886.6[1]
Na2S (cr)
9 hydrate
-3074.0[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]
* (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas, (cr):Crystalline solid, (ai):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)