3H2S + 6NaHCO3 🔥→ 2Na2SO3 + Na2S + 6CO + 6H2O
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The reaction of hydrogen sulfide and sodium hydrogencarbonate yields sodium sulfite, sodium sulfide, carbon monoxide, and water (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 | 3 | Reducing | Reducing |
NaHCO3 | Sodium hydrogencarbonate | 6 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SO3 | Sodium sulfite | 2 | Oxidized | – |
Na2S | Sodium sulfide | 1 | – | – |
CO | Carbon monoxide | 6 | Reduced | – |
H2O | Water | 6 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 586.1 kJ/mol K 0.21 × 10−102 pK 102.68
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 | 822.2 | 586.1 | 753.5 | – |
per 1 mol of | 274.1 | 195.4 | 251.2 | – |
per 1 mol of | 137.0 | 97.68 | 125.6 | – |
per 1 mol of | 411.1 | 293.1 | 376.8 | – |
per 1 mol of | 822.2 | 586.1 | 753.5 | – |
per 1 mol of | 137.0 | 97.68 | 125.6 | – |
per 1 mol of | 137.0 | 97.68 | 125.6 | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 470.8 kJ/mol K 0.33 × 10−82 pK 82.48
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 | 654.6 | 470.8 | 620 | – |
per 1 mol of | 218.2 | 156.9 | 207 | – |
per 1 mol of | 109.1 | 78.47 | 103 | – |
per 1 mol of | 327.3 | 235.4 | 310 | – |
per 1 mol of | 654.6 | 470.8 | 620 | – |
per 1 mol of | 109.1 | 78.47 | 103 | – |
per 1 mol of | 109.1 | 78.47 | 103 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 574.4 kJ/mol K 0.23 × 10−100 pK 100.63
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 | 592.0 | 574.4 | 62 | – |
per 1 mol of | 197.3 | 191.5 | 21 | – |
per 1 mol of | 98.67 | 95.73 | 10 | – |
per 1 mol of | 296.0 | 287.2 | 31 | – |
per 1 mol of | 592.0 | 574.4 | 62 | – |
per 1 mol of | 98.67 | 95.73 | 10 | – |
per 1 mol of | 98.67 | 95.73 | 10 | – |
Changes in aqueous solution (3)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 477.0 kJ/mol K 0.27 × 10−83 pK 83.57
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 | 725.3 | 477.0 | 839 | – |
per 1 mol of | 241.8 | 159.0 | 280 | – |
per 1 mol of | 120.9 | 79.50 | 140 | – |
per 1 mol of | 362.6 | 238.5 | 420 | – |
per 1 mol of | 725.3 | 477.0 | 839 | – |
per 1 mol of | 120.9 | 79.50 | 140 | – |
per 1 mol of | 120.9 | 79.50 | 140 | – |
Changes in aqueous solution (4)
- Reaction of hydrogen sulfide and sodium hydrogencarbonate◆
ΔrG 580.6 kJ/mol K 0.19 × 10−101 pK 101.72
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 | 662.7 | 580.6 | 280 | – |
per 1 mol of | 220.9 | 193.5 | 93.3 | – |
per 1 mol of | 110.5 | 96.77 | 46.7 | – |
per 1 mol of | 331.4 | 290.3 | 140 | – |
per 1 mol of | 662.7 | 580.6 | 280 | – |
per 1 mol of | 110.5 | 96.77 | 46.7 | – |
per 1 mol of | 110.5 | 96.77 | 46.7 | – |
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 |
---|---|---|---|---|
Na2SO3 (cr) | -1100.8[1] | -1012.5[1] | 145.94[1] | 120.25[1] |
Na2SO3 (ai) | -1115.87[1] | -1010.39[1] | 87.9[1] | – |
Na2SO3 (cr) 7 hydrate | -3162.3[1] | -2676.1[1] | 444[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] | – | – | – |
CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
CO (ao) | -120.96[1] | -119.90[1] | 104.6[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -1100.8 kJ · mol−1
- ^ ΔfG°, -1012.5 kJ · mol−1
- ^ S°, 145.94 J · K−1 · mol−1
- ^ Cp°, 120.25 J · K−1 · mol−1
- ^ ΔfH°, -1115.87 kJ · mol−1
- ^ ΔfG°, -1010.39 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -3162.3 kJ · mol−1
- ^ ΔfG°, -2676.1 kJ · mol−1
- ^ S°, 444. 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°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1