6NaHS + 6MnO2 → 2Na2SO3 + Na2S + 3Mn(OH)2 + 3MnS
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The reaction of sodium hydrogensulfide and manganese(IV) oxide yields sodium sulfite, sodium sulfide, manganese(II) hydroxide, and manganese(II) sulfide (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 sodium hydrogensulfide and manganese(IV) oxide
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 sodium hydrogensulfide and manganese(IV) oxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NaHS | Sodium hydrogensulfide | 6 | Reducing | Reducing |
MnO2 | Manganese(IV) oxide | 6 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na2SO3 | Sodium sulfite | 2 | Oxidized | – |
Na2S | Sodium sulfide | 1 | – | – |
Mn(OH)2 | Manganese(II) hydroxide | 3 | Reduced | – |
MnS | Manganese(II) sulfide | 3 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of sodium hydrogensulfide and manganese(IV) oxide
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 | −751.6 | – | – | – |
per 1 mol of | −125.3 | – | – | – |
per 1 mol of | −125.3 | – | – | – |
per 1 mol of | −375.8 | – | – | – |
per 1 mol of | −751.6 | – | – | – |
per 1 mol of | −250.5 | – | – | – |
per 1 mol of | −250.5 | – | – | – |
Changes in standard condition (2)
- Reaction of sodium hydrogensulfide and manganese(IV) oxide
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 | −750.4 | – | – | – |
per 1 mol of | −125.1 | – | – | – |
per 1 mol of | −125.1 | – | – | – |
per 1 mol of | −375.2 | – | – | – |
per 1 mol of | −750.4 | – | – | – |
per 1 mol of | −250.1 | – | – | – |
per 1 mol of | −250.1 | – | – | – |
Changes in standard condition (3)
- Reaction of sodium hydrogensulfide and manganese(IV) oxide
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 | −856.8 | – | – | – |
per 1 mol of | −142.8 | – | – | – |
per 1 mol of | −142.8 | – | – | – |
per 1 mol of | −428.4 | – | – | – |
per 1 mol of | −856.8 | – | – | – |
per 1 mol of | −285.6 | – | – | – |
per 1 mol of | −285.6 | – | – | – |
Changes in standard condition (4)
- Reaction of sodium hydrogensulfide and manganese(IV) oxide
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 | −855.6 | – | – | – |
per 1 mol of | −142.6 | – | – | – |
per 1 mol of | −142.6 | – | – | – |
per 1 mol of | −427.8 | – | – | – |
per 1 mol of | −855.6 | – | – | – |
per 1 mol of | −285.2 | – | – | – |
per 1 mol of | −285.2 | – | – | – |
Changes in aqueous solution
- Reaction of sodium hydrogensulfide and manganese(IV) oxide◆
ΔrG −669.4 kJ/mol K 1.88 × 10117 pK −117.27
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 | −741.3 | −669.4 | −237.8 | – |
per 1 mol of | −123.5 | −111.6 | −39.63 | – |
per 1 mol of | −123.5 | −111.6 | −39.63 | – |
per 1 mol of | −370.6 | −334.7 | −118.9 | – |
per 1 mol of | −741.3 | −669.4 | −237.8 | – |
per 1 mol of | −247.1 | −223.1 | −79.27 | – |
per 1 mol of | −247.1 | −223.1 | −79.27 | – |
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 |
---|---|---|---|---|
NaHS (cr) | -237.23[1] | – | – | – |
NaHS (ai) | -257.73[1] | -249.81[1] | 121.8[1] | – |
NaHS (cr) 2 hydrate | -838.47[1] | – | – | – |
MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
MnO2 (am) precipitated | -502.5[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid
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] | – | – | – |
Mn(OH)2 (am) precipitated | -695.4[1] | -615.0[1] | 99.2[1] | – |
MnS (cr) green | -214.2[1] | -218.4[1] | 78.2[1] | 49.96[1] |
MnS (am) precipitated, pink | -213.8[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous solid
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°, -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
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · 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°, -695.4 kJ · mol−1
- ^ ΔfG°, -615.0 kJ · mol−1
- ^ S°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, -214.2 kJ · mol−1
- ^ ΔfG°, -218.4 kJ · mol−1
- ^ S°, 78.2 J · K−1 · mol−1
- ^ Cp°, 49.96 J · K−1 · mol−1
- ^ ΔfH°, -213.8 kJ · mol−1