3H2S + NaIO3 → 3S + NaI + 3H2O
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- Reaction of hydrogen sulfide and sodium iodate
The reaction of hydrogen sulfide and sodium iodate yields , sodium iodide, 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 iodate
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen sulfide and sodium iodate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 3 | Reducing | Reducing |
NaIO3 | Sodium iodate | 1 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
3 | Oxidized | – | ||
NaI | Sodium iodide | 1 | Reduced | – |
H2O | Water | 3 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of hydrogen sulfide and sodium iodate
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 | −601.59 | – | – | 151.2 |
per 1 mol of | −200.53 | – | – | 50.40 |
per 1 mol of | −601.59 | – | – | 151.2 |
−200.53 | – | – | 50.40 | |
per 1 mol of | −601.59 | – | – | 151.2 |
per 1 mol of | −200.53 | – | – | 50.40 |
Changes in standard condition (2)
- Reaction of hydrogen sulfide and sodium iodate
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 | −600.60 | – | – | – |
per 1 mol of | −200.20 | – | – | – |
per 1 mol of | −600.60 | – | – | – |
−200.20 | – | – | – | |
per 1 mol of | −600.60 | – | – | – |
per 1 mol of | −200.20 | – | – | – |
Changes in aqueous solution
- Reaction of hydrogen sulfide and sodium iodate◆
ΔrG −551.5 kJ/mol K 4.16 × 1096 pK −96.62
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 | −572.2 | −551.5 | −65 | – |
per 1 mol of | −190.7 | −183.8 | −22 | – |
per 1 mol of | −572.2 | −551.5 | −65 | – |
−190.7 | −183.8 | −22 | – | |
per 1 mol of | −572.2 | −551.5 | −65 | – |
per 1 mol of | −190.7 | −183.8 | −22 | – |
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] | – |
NaIO3 (cr) | -481.788[1] | – | – | 92.0[1] |
NaIO3 (ai) | -461.5[1] | -389.9[1] | 177.4[1] | – |
NaIO3 (cr) 1 hydrate | -779.48[1] | -634.03[1] | 162.3[1] | – |
NaIO3 (cr) 5 hydrate | -1952.25[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 |
---|---|---|---|---|
(cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
(cr) monoclinic | 0.33[1] | – | – | – |
(g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
NaI (cr) | -287.78[1] | -286.06[1] | 98.53[1] | 52.09[1] |
NaI (g) | -79.5[1] | -121.0[1] | 248.978[1] | 36.65[1] |
NaI (ai) | -295.31[1] | -313.47[1] | 170.3[1] | -95.8[1] |
NaI (cr) 1 hydrate | -883.096[1] | -771.10[1] | 196.2[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, (g):Gas, (ai):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°, -481.788 kJ · mol−1
- ^ Cp°, 92.0 J · K−1 · mol−1
- ^ ΔfH°, -461.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 177.4 J · K−1 · mol−1
- ^ ΔfH°, -779.48 kJ · mol−1
- ^ ΔfG°, -634.03 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1
- ^ ΔfH°, -1952.25 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -287.78 kJ · mol−1
- ^ ΔfG°, -286.06 kJ · mol−1
- ^ S°, 98.53 J · K−1 · mol−1
- ^ Cp°, 52.09 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -121.0 kJ · mol−1
- ^ S°, 248.978 J · K−1 · mol−1
- ^ Cp°, 36.65 J · K−1 · mol−1
- ^ ΔfH°, -295.31 kJ · mol−1
- ^ ΔfG°, -313.47 kJ · mol−1
- ^ S°, 170.3 J · K−1 · mol−1
- ^ Cp°, -95.8 J · K−1 · mol−1
- ^ ΔfH°, -883.096 kJ · mol−1
- ^ ΔfG°, -771.10 kJ · mol−1
- ^ S°, 196.2 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