5H2S + 3Mg(NO3)2 → 2SO2 + 3N2O3 + 3MgS + 5H2O
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The reaction of hydrogen sulfide and magnesium nitrate yields sulfur dioxide, dinitrogen trioxide, magnesium sulfide, 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 magnesium nitrate
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 magnesium nitrate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 5 | Reducing | Reducing |
Mg(NO3)2 | Magnesium nitrate | 3 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
SO2 | Sulfur dioxide | 2 | Oxidized | – |
N2O3 | Dinitrogen trioxide | 3 | Reduced | – |
MgS | Magnesium sulfide | 3 | – | – |
H2O | Water | 5 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and magnesium nitrate◆
ΔrG −457.1 kJ/mol K 1.20 × 1080 pK −80.08
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 | −334.6 | −457.1 | 412.9 | 192.80 |
per 1 mol of | −66.92 | −91.42 | 82.58 | 38.560 |
per 1 mol of | −111.5 | −152.4 | 137.6 | 64.267 |
per 1 mol of | −167.3 | −228.6 | 206.4 | 96.400 |
per 1 mol of | −111.5 | −152.4 | 137.6 | 64.267 |
per 1 mol of | −111.5 | −152.4 | 137.6 | 64.267 |
per 1 mol of | −66.92 | −91.42 | 82.58 | 38.560 |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and magnesium nitrate◆
ΔrG −222.0 kJ/mol K 7.81 × 1038 pK −38.89
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 | 33.6 | −222.0 | 864 | – |
per 1 mol of | 6.72 | −44.40 | 173 | – |
per 1 mol of | 11.2 | −74.00 | 288 | – |
per 1 mol of | 16.8 | −111.0 | 432 | – |
per 1 mol of | 11.2 | −74.00 | 288 | – |
per 1 mol of | 11.2 | −74.00 | 288 | – |
per 1 mol of | 6.72 | −44.40 | 173 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and magnesium nitrate◆
ΔrG −223.0 kJ/mol K 1.17 × 1039 pK −39.07
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 | −18.7 | −223.0 | 692 | – |
per 1 mol of | −3.74 | −44.60 | 138 | – |
per 1 mol of | −6.23 | −74.33 | 231 | – |
per 1 mol of | −9.35 | −111.5 | 346 | – |
per 1 mol of | −6.23 | −74.33 | 231 | – |
per 1 mol of | −6.23 | −74.33 | 231 | – |
per 1 mol of | −3.74 | −44.60 | 138 | – |
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] | – |
Mg(NO3)2 (cr) | -790.65[1] | -589.4[1] | 164.0[1] | 141.92[1] |
Mg(NO3)2 (ai) | -881.57[1] | -677.3[1] | 154.8[1] | – |
Mg(NO3)2 (cr) 2 hydrate | -1409.2[1] | – | – | – |
Mg(NO3)2 (cr) 6 hydrate | -2613.28[1] | -2080.3[1] | 452[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 |
---|---|---|---|---|
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] | – |
N2O3 (l) | 50.29[1] | – | – | – |
N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[1] |
MgS (cr) | -346.0[1] | -341.8[1] | 50.33[1] | 45.56[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] |
* (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline 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°, -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°, -790.65 kJ · mol−1
- ^ ΔfG°, -589.4 kJ · mol−1
- ^ S°, 164.0 J · K−1 · mol−1
- ^ Cp°, 141.92 J · K−1 · mol−1
- ^ ΔfH°, -881.57 kJ · mol−1
- ^ ΔfG°, -677.3 kJ · mol−1
- ^ S°, 154.8 J · K−1 · mol−1
- ^ ΔfH°, -1409.2 kJ · mol−1
- ^ ΔfH°, -2613.28 kJ · mol−1
- ^ ΔfG°, -2080.3 kJ · mol−1
- ^ S°, 452. 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°, 50.29 kJ · mol−1
- ^ ΔfH°, 83.72 kJ · mol−1
- ^ ΔfG°, 139.46 kJ · mol−1
- ^ S°, 312.28 J · K−1 · mol−1
- ^ Cp°, 65.61 J · K−1 · mol−1
- ^ ΔfH°, -346.0 kJ · mol−1
- ^ ΔfG°, -341.8 kJ · mol−1
- ^ S°, 50.33 J · K−1 · mol−1
- ^ Cp°, 45.56 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