5H2S + 4Cu(NO3)2 → 4CuSO4 + SO3 + 4N2 + 5H2O
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- Reaction of hydrogen sulfide and copper(II) nitrate
The reaction of hydrogen sulfide and copper(II) nitrate yields copper(II) sulfate, sulfur trioxide, , 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 copper(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 copper(II) nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| H2S | Hydrogen sulfide | 5 | Reducing | Reducing |
| Cu(NO3)2 | Copper(II) nitrate | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CuSO4 | Copper(II) sulfate | 4 | Oxidized | – |
| SO3 | Sulfur trioxide | 1 | Oxidized | – |
| 4 | Reduced | – | ||
| H2O | Water | 5 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and copper(II) nitrate
| 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 | −3640.9 | – | – | – |
per 1 mol of | −728.18 | – | – | – |
per 1 mol of | −910.23 | – | – | – |
per 1 mol of | −910.23 | – | – | – |
per 1 mol of | −3640.9 | – | – | – |
| −910.23 | – | – | – | |
per 1 mol of | −728.18 | – | – | – |
Changes in aqueous solution (1)
- Reaction of hydrogen sulfide and copper(II) nitrate◆
ΔrG −3561.35 kJ/mol K 8.35 × 10623 pK −623.92
| 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 | – | −3561.35 | – | – |
per 1 mol of | – | −712.270 | – | – |
per 1 mol of | – | −890.337 | – | – |
per 1 mol of | – | −890.337 | – | – |
per 1 mol of | – | −3561.35 | – | – |
| – | −890.337 | – | – | |
per 1 mol of | – | −712.270 | – | – |
Changes in aqueous solution (2)
- Reaction of hydrogen sulfide and copper(II) nitrate◆
ΔrG −3439.8 kJ/mol K 4.24 × 10602 pK −602.63
| 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 | −3370.8 | −3439.8 | 244 | – |
per 1 mol of | −674.16 | −687.96 | 48.8 | – |
per 1 mol of | −842.70 | −859.95 | 61.0 | – |
per 1 mol of | −842.70 | −859.95 | 61.0 | – |
per 1 mol of | −3370.8 | −3439.8 | 244 | – |
| −842.70 | −859.95 | 61.0 | – | |
per 1 mol of | −674.16 | −687.96 | 48.8 | – |
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] | – |
| Cu(NO3)2 (cr) | -302.9[1] | – | – | – |
| Cu(NO3)2 (ai) | -349.95[1] | -157.02[1] | 193.3[1] | – |
| Cu(NO3)2 (cr) 3 hydrate | -1217.1[1] | – | – | – |
| Cu(NO3)2 (cr) 6 hydrate | -2110.8[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 |
|---|---|---|---|---|
| CuSO4 (cr) | -771.36[1] | -661.8[1] | 109[1] | 100.0[1] |
| CuSO4 (ai) | -844.50[1] | -679.04[1] | -79.5[1] | – |
| CuSO4 (ao) | – | -692.18[1] | – | – |
| CuSO4 (cr) 1 hydrate | -1085.83[1] | -918.11[1] | 146.0[1] | 134[1] |
| CuSO4 (cr) 3 hydrate | -1684.31[1] | -1399.96[1] | 221.3[1] | 205[1] |
| CuSO4 (cr) 5 hydrate | -2279.65[1] | -1879.745[1] | 300.4[1] | 280[1] |
| SO3 (cr) β | -454.51[1] | -374.21[1] | 70.7[1] | – |
| SO3 (l) | -441.04[1] | -373.75[1] | 113.8[1] | – |
| SO3 (g) | -395.72[1] | -371.06[1] | 256.76[1] | 50.67[1] |
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[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, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas
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°, -302.9 kJ · mol−1
- ^ ΔfH°, -349.95 kJ · mol−1
- ^ ΔfG°, -157.02 kJ · mol−1
- ^ S°, 193.3 J · K−1 · mol−1
- ^ ΔfH°, -1217.1 kJ · mol−1
- ^ ΔfH°, -2110.8 kJ · mol−1
- ^ ΔfH°, -771.36 kJ · mol−1
- ^ ΔfG°, -661.8 kJ · mol−1
- ^ S°, 109. J · K−1 · mol−1
- ^ Cp°, 100.0 J · K−1 · mol−1
- ^ ΔfH°, -844.50 kJ · mol−1
- ^ ΔfG°, -679.04 kJ · mol−1
- ^ S°, -79.5 J · K−1 · mol−1
- ^ ΔfG°, -692.18 kJ · mol−1
- ^ ΔfH°, -1085.83 kJ · mol−1
- ^ ΔfG°, -918.11 kJ · mol−1
- ^ S°, 146.0 J · K−1 · mol−1
- ^ Cp°, 134. J · K−1 · mol−1
- ^ ΔfH°, -1684.31 kJ · mol−1
- ^ ΔfG°, -1399.96 kJ · mol−1
- ^ S°, 221.3 J · K−1 · mol−1
- ^ Cp°, 205. J · K−1 · mol−1
- ^ ΔfH°, -2279.65 kJ · mol−1
- ^ ΔfG°, -1879.745 kJ · mol−1
- ^ S°, 300.4 J · K−1 · mol−1
- ^ Cp°, 280. J · K−1 · mol−1
- ^ ΔfH°, -454.51 kJ · mol−1
- ^ ΔfG°, -374.21 kJ · mol−1
- ^ S°, 70.7 J · K−1 · mol−1
- ^ ΔfH°, -441.04 kJ · mol−1
- ^ ΔfG°, -373.75 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1
- ^ ΔfH°, -395.72 kJ · mol−1
- ^ ΔfG°, -371.06 kJ · mol−1
- ^ S°, 256.76 J · K−1 · mol−1
- ^ Cp°, 50.67 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 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