11H2S + 6NaHCO3 🔥→ 2H2SO3 + 6SO2 + 3Na2S + 6CH4
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- Reaction of hydrogen sulfide and sodium hydrogencarbonate
The reaction of hydrogen sulfide and sodium hydrogencarbonate yields sulfurous acid, sulfur dioxide, sodium sulfide, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen sulfide and sodium hydrogencarbonate
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 sodium hydrogencarbonate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 11 | Reducing | Reducing |
NaHCO3 | Sodium hydrogencarbonate | 6 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2SO3 | Sulfurous acid | 2 | Oxidized | – |
SO2 | Sulfur dioxide | 6 | Oxidized | – |
Na2S | Sodium sulfide | 3 | – | – |
6 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 902.7 kJ/mol K 0.71 × 10−158 pK 158.15
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 | 1240.0 | 902.7 | 1149 | – |
per 1 mol of | 112.73 | 82.06 | 104.5 | – |
per 1 mol of | 206.67 | 150.5 | 191.5 | – |
per 1 mol of | 620.00 | 451.4 | 574.5 | – |
per 1 mol of | 206.67 | 150.5 | 191.5 | – |
per 1 mol of | 413.33 | 300.9 | 383.0 | – |
206.67 | 150.5 | 191.5 | – |
Changes in standard condition (2)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 1001.0 kJ/mol K 0.43 × 10−175 pK 175.37
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 | 1154.6 | 1001.0 | 534 | – |
per 1 mol of | 104.96 | 91.000 | 48.5 | – |
per 1 mol of | 192.43 | 166.83 | 89.0 | – |
per 1 mol of | 577.30 | 500.50 | 267 | – |
per 1 mol of | 192.43 | 166.83 | 89.0 | – |
per 1 mol of | 384.87 | 333.67 | 178 | – |
192.43 | 166.83 | 89.0 | – |
Changes in standard condition (3)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 899.8 kJ/mol K 0.23 × 10−157 pK 157.64
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 | 1083.1 | 899.8 | 631 | – |
per 1 mol of | 98.464 | 81.80 | 57.4 | – |
per 1 mol of | 180.52 | 150.0 | 105 | – |
per 1 mol of | 541.55 | 449.9 | 316 | – |
per 1 mol of | 180.52 | 150.0 | 105 | – |
per 1 mol of | 361.03 | 299.9 | 210 | – |
180.52 | 150.0 | 105 | – |
Changes in standard condition (4)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 998.1 kJ/mol K 0.14 × 10−174 pK 174.86
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 | 997.7 | 998.1 | 16 | – |
per 1 mol of | 90.70 | 90.74 | 1.5 | – |
per 1 mol of | 166.3 | 166.3 | 2.7 | – |
per 1 mol of | 498.9 | 499.1 | 8.0 | – |
per 1 mol of | 166.3 | 166.3 | 2.7 | – |
per 1 mol of | 332.6 | 332.7 | 5.3 | – |
166.3 | 166.3 | 2.7 | – |
Changes in standard condition (5)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 908.9 kJ/mol K 0.59 × 10−159 pK 159.23
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 | 1310.7 | 908.9 | 1367 | – |
per 1 mol of | 119.15 | 82.63 | 124.3 | – |
per 1 mol of | 218.45 | 151.5 | 227.8 | – |
per 1 mol of | 655.35 | 454.4 | 683.5 | – |
per 1 mol of | 218.45 | 151.5 | 227.8 | – |
per 1 mol of | 436.90 | 303.0 | 455.7 | – |
218.45 | 151.5 | 227.8 | – |
Changes in standard condition (6)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 1007.3 kJ/mol K 0.34 × 10−176 pK 176.47
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 | 1225.4 | 1007.3 | 752 | – |
per 1 mol of | 111.40 | 91.573 | 68.4 | – |
per 1 mol of | 204.23 | 167.88 | 125 | – |
per 1 mol of | 612.70 | 503.65 | 376 | – |
per 1 mol of | 204.23 | 167.88 | 125 | – |
per 1 mol of | 408.47 | 335.77 | 251 | – |
204.23 | 167.88 | 125 | – |
Changes in standard condition (7)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 906.0 kJ/mol K 0.19 × 10−158 pK 158.72
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 | 1153.8 | 906.0 | 849 | – |
per 1 mol of | 104.89 | 82.36 | 77.2 | – |
per 1 mol of | 192.30 | 151.0 | 142 | – |
per 1 mol of | 576.90 | 453.0 | 425 | – |
per 1 mol of | 192.30 | 151.0 | 142 | – |
per 1 mol of | 384.60 | 302.0 | 283 | – |
192.30 | 151.0 | 142 | – |
Changes in standard condition (8)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 1004.4 kJ/mol K 0.11 × 10−175 pK 175.96
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 | 1068.5 | 1004.4 | 234 | – |
per 1 mol of | 97.136 | 91.309 | 21.3 | – |
per 1 mol of | 178.08 | 167.40 | 39.0 | – |
per 1 mol of | 534.25 | 502.20 | 117 | – |
per 1 mol of | 178.08 | 167.40 | 39.0 | – |
per 1 mol of | 356.17 | 334.80 | 78.0 | – |
178.08 | 167.40 | 39.0 | – |
Thermodynamic data of reactants
Chemical formula | Standard 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 formula | Standard 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] | – | – | – |
(g) | -74.81[1] | -50.72[1] | 186.264[1] | 35.309[1] |
(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
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, -950.81 kJ · mol−1
- ^ ΔfG°, -851.0 kJ · mol−1
- ^ S°, 101.7 J · K−1 · mol−1
- ^ Cp°, 87.61 J · K−1 · mol−1
- ^ ΔfH°, -932.11 kJ · mol−1
- ^ ΔfG°, -848.66 kJ · mol−1
- ^ S°, 150.2 J · K−1 · mol−1
- ^ ΔfH°, -943.9 kJ · mol−1
- ^ ΔfG°, -849.7 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1
- ^ ΔfH°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1
- ^ ΔfH°, -364.8 kJ · mol−1
- ^ ΔfG°, -349.8 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1
- ^ ΔfH°, -447.3 kJ · mol−1
- ^ ΔfG°, -438.1 kJ · mol−1
- ^ S°, 103.3 J · K−1 · mol−1
- ^ ΔfH°, -1725.9 kJ · mol−1
- ^ ΔfH°, -1886.6 kJ · mol−1
- ^ ΔfH°, -3074.0 kJ · mol−1
- ^ ΔfH°, -74.81 kJ · mol−1
- ^ ΔfG°, -50.72 kJ · mol−1
- ^ S°, 186.264 J · K−1 · mol−1
- ^ Cp°, 35.309 J · K−1 · mol−1
- ^ ΔfH°, -89.04 kJ · mol−1
- ^ ΔfG°, -34.33 kJ · mol−1
- ^ S°, 83.7 J · K−1 · mol−1