Na2CO3 + H2S → NaHCO3 + NaHS
Last updated:
The reaction of sodium carbonate and hydrogen sulfide yields sodium hydrogencarbonate and sodium hydrogensulfide (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium carbonate and hydrogen sulfide
General equation
Oxidation state of each atom
- Reaction of sodium carbonate and hydrogen sulfide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2CO3 | Sodium carbonate | 1 | Brønsted base | Salt |
H2S | Hydrogen sulfide | 1 | Brønsted acid | Acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NaHCO3 | Sodium hydrogencarbonate | 1 | Conjugate acid base | Acid salt |
NaHS | Sodium hydrogensulfide | 1 | Conjugate acid base | Acid salt |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium carbonate and hydrogen sulfide
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 | −36.73 | – | – | – |
per 1 mol of | −36.73 | – | – | – |
per 1 mol of | −36.73 | – | – | – |
per 1 mol of | −36.73 | – | – | – |
per 1 mol of | −36.73 | – | – | – |
Changes in aqueous solution (1)
- Reaction of sodium carbonate and hydrogen sulfide◆
ΔrG −19.00 kJ/mol K 2.13 × 103 pK −3.33
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 | 7.2 | −19.00 | 90 | – |
per 1 mol of | 7.2 | −19.00 | 90 | – |
per 1 mol of | 7.2 | −19.00 | 90 | – |
per 1 mol of | 7.2 | −19.00 | 90 | – |
per 1 mol of | 7.2 | −19.00 | 90 | – |
Changes in aqueous solution (2)
- Reaction of sodium carbonate and hydrogen sulfide◆
ΔrG −20.0 kJ/mol K 3.19 × 103 pK −3.50
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 | −4.5 | −20.0 | 54 | – |
per 1 mol of | −4.5 | −20.0 | 54 | – |
per 1 mol of | −4.5 | −20.0 | 54 | – |
per 1 mol of | −4.5 | −20.0 | 54 | – |
per 1 mol of | −4.5 | −20.0 | 54 | – |
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 |
---|---|---|---|---|
Na2CO3 (cr) | -1130.68[1] | -1044.44[1] | 134.98[1] | 112.30[1] |
Na2CO3 (ai) | -1157.38[1] | -1051.64[1] | 61.1[1] | – |
Na2CO3 (cr) 1 hydrate | -1431.26[1] | -1285.31[1] | 168.11[1] | 145.60[1] |
Na2CO3 (cr) 7 hydrate | -3199.96[1] | -2714.2[1] | 422.2[1] | – |
Na2CO3 (cr) 10 hydrate | -4081.32[1] | -3427.66[1] | 562.7[1] | 550.32[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] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-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 |
---|---|---|---|---|
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] | – |
NaHS (cr) | -237.23[1] | – | – | – |
NaHS (ai) | -257.73[1] | -249.81[1] | 121.8[1] | – |
NaHS (cr) 2 hydrate | -838.47[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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°, -1130.68 kJ · mol−1
- ^ ΔfG°, -1044.44 kJ · mol−1
- ^ S°, 134.98 J · K−1 · mol−1
- ^ Cp°, 112.30 J · K−1 · mol−1
- ^ ΔfH°, -1157.38 kJ · mol−1
- ^ ΔfG°, -1051.64 kJ · mol−1
- ^ S°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -1431.26 kJ · mol−1
- ^ ΔfG°, -1285.31 kJ · mol−1
- ^ S°, 168.11 J · K−1 · mol−1
- ^ Cp°, 145.60 J · K−1 · mol−1
- ^ ΔfH°, -3199.96 kJ · mol−1
- ^ ΔfG°, -2714.2 kJ · mol−1
- ^ S°, 422.2 J · K−1 · mol−1
- ^ ΔfH°, -4081.32 kJ · mol−1
- ^ ΔfG°, -3427.66 kJ · mol−1
- ^ S°, 562.7 J · K−1 · mol−1
- ^ Cp°, 550.32 J · K−1 · mol−1
- ^ 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°, -237.23 kJ · mol−1
- ^ ΔfH°, -257.73 kJ · mol−1
- ^ ΔfG°, -249.81 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -838.47 kJ · mol−1