12H2S + 3Pb(NO3)2 → 2(NH4)2SO3 + 6SO2 + (NH4)2S + 3PbS
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The reaction of hydrogen sulfide and lead(II) nitrate yields ammonium sulfite, sulfur dioxide, ammonium sulfide, and lead(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 hydrogen sulfide and lead(II) 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 lead(II) nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 12 | Reducing | Reducing |
| Pb(NO3)2 | Lead(II) nitrate | 3 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)2SO3 | Ammonium sulfite | 2 | Redoxed product | – |
| SO2 | Sulfur dioxide | 6 | Oxidized | – |
| (NH4)2S | Ammonium sulfide | 1 | Reduced | – |
| PbS | Lead(II) sulfide | 3 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and lead(II) nitrate◆
ΔrG −2385.1 kJ/mol K 7.10 × 10417 pK −417.85
| 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 | −2389.5 | −2385.1 | 8 | – |
per 1 mol of | −199.13 | −198.76 | 0.7 | – |
per 1 mol of | −796.50 | −795.03 | 3 | – |
per 1 mol of | −1194.8 | −1192.5 | 4 | – |
per 1 mol of | −398.25 | −397.52 | 1 | – |
per 1 mol of | −2389.5 | −2385.1 | 8 | – |
per 1 mol of | −796.50 | −795.03 | 3 | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and lead(II) nitrate◆
ΔrG −2388.0 kJ/mol K 2.29 × 10418 pK −418.36
| 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 | −2546.4 | −2388.0 | −510 | – |
per 1 mol of | −212.20 | −199.00 | −42.5 | – |
per 1 mol of | −848.80 | −796.00 | −170 | – |
per 1 mol of | −1273.2 | −1194.0 | −255 | – |
per 1 mol of | −424.40 | −398.00 | −85.0 | – |
per 1 mol of | −2546.4 | −2388.0 | −510 | – |
per 1 mol of | −848.80 | −796.00 | −170 | – |
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] | – |
| Pb(NO3)2 (cr) | -451.9[1] | – | – | – |
| Pb(NO3)2 (ai) | -416.3[1] | -246.93[1] | 303.3[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 |
|---|---|---|---|---|
| (NH4)2SO3 (cr) | -885.3[1] | – | – | – |
| (NH4)2SO3 (ai) | -900.4[1] | -645.0[1] | 197.5[1] | – |
| (NH4)2SO3 (cr) 1 hydrate | -1187.4[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] | – |
| (NH4)2S (ai) | -231.8[1] | -72.6[1] | 212.1[1] | – |
| PbS (cr) | -100.4[1] | -98.7[1] | 91.2[1] | 49.50[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (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°, -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°, -451.9 kJ · mol−1
- ^ ΔfH°, -416.3 kJ · mol−1
- ^ ΔfG°, -246.93 kJ · mol−1
- ^ S°, 303.3 J · K−1 · mol−1
- ^ ΔfH°, -885.3 kJ · mol−1
- ^ ΔfH°, -900.4 kJ · mol−1
- ^ ΔfG°, -645.0 kJ · mol−1
- ^ S°, 197.5 J · K−1 · mol−1
- ^ ΔfH°, -1187.4 kJ · 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°, -231.8 kJ · mol−1
- ^ ΔfG°, -72.6 kJ · mol−1
- ^ S°, 212.1 J · K−1 · mol−1
- ^ ΔfH°, -100.4 kJ · mol−1
- ^ ΔfG°, -98.7 kJ · mol−1
- ^ S°, 91.2 J · K−1 · mol−1
- ^ Cp°, 49.50 J · K−1 · mol−1