3ZnS + 4HNO3 → 3ZnSO4 + 2N2↑ + 2H2↑
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- Reaction of zinc sulfide and nitric acid
The reaction of zinc sulfide and nitric acid yields zinc sulfate, , and (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 zinc sulfide and nitric acid
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 zinc sulfide and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnS | Zinc sulfide | 3 | Reducing | Reducing |
| HNO3 | Nitric acid | 4 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnSO4 | Zinc sulfate | 3 | Oxidized | – |
| 2 | Reduced | – | ||
| 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1687.8 kJ/mol K 4.90 × 10295 pK −295.69
| 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 | −1634.1 | −1687.8 | 180.6 | −164.0 |
per 1 mol of | −544.70 | −562.60 | 60.20 | −54.67 |
per 1 mol of | −408.52 | −421.95 | 45.15 | −41.00 |
per 1 mol of | −544.70 | −562.60 | 60.20 | −54.67 |
| −817.05 | −843.90 | 90.30 | −82.00 | |
| −817.05 | −843.90 | 90.30 | −82.00 |
Changes in aqueous solution (1)
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1665.8 kJ/mol K 6.85 × 10291 pK −291.84
| 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 | −1695.7 | −1665.8 | −99.1 | – |
per 1 mol of | −565.23 | −555.27 | −33.0 | – |
per 1 mol of | −423.93 | −416.45 | −24.8 | – |
per 1 mol of | −565.23 | −555.27 | −33.0 | – |
| −847.85 | −832.90 | −49.5 | – | |
| −847.85 | −832.90 | −49.5 | – |
Changes in aqueous solution (2)
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1630.6 kJ/mol K 4.66 × 10285 pK −285.67
| 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 | −1704.1 | −1630.6 | 794 | – |
per 1 mol of | −568.03 | −543.53 | 265 | – |
per 1 mol of | −426.02 | −407.65 | 199 | – |
per 1 mol of | −568.03 | −543.53 | 265 | – |
| −852.05 | −815.30 | 397 | – | |
| −852.05 | −815.30 | 397 | – |
Changes in aqueous solution (3)
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1625.90 kJ/mol K 7.00 × 10284 pK −284.85
| 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 | −1742.07 | −1625.90 | −390.1 | −417 |
per 1 mol of | −580.690 | −541.967 | −130.0 | −139 |
per 1 mol of | −435.517 | −406.475 | −97.53 | −104 |
per 1 mol of | −580.690 | −541.967 | −130.0 | −139 |
| −871.035 | −812.950 | −195.1 | −209 | |
| −871.035 | −812.950 | −195.1 | −209 |
Changes in aqueous solution (4)
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1590.7 kJ/mol K 4.77 × 10278 pK −278.68
| 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 | −1750.5 | −1590.7 | 503 | – |
per 1 mol of | −583.50 | −530.23 | 168 | – |
per 1 mol of | −437.63 | −397.68 | 126 | – |
per 1 mol of | −583.50 | −530.23 | 168 | – |
| −875.25 | −795.35 | 252 | – | |
| −875.25 | −795.35 | 252 | – |
Changes in aqueous solution (5)
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1665.8 kJ/mol K 6.85 × 10291 pK −291.84
| 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 | −1695.7 | −1665.8 | −99.1 | – |
per 1 mol of | −565.23 | −555.27 | −33.0 | – |
per 1 mol of | −423.93 | −416.45 | −24.8 | – |
per 1 mol of | −565.23 | −555.27 | −33.0 | – |
| −847.85 | −832.90 | −49.5 | – | |
| −847.85 | −832.90 | −49.5 | – |
Changes in aqueous solution (6)
- Reaction of zinc sulfide and nitric acid◆
ΔrG −1630.6 kJ/mol K 4.66 × 10285 pK −285.67
| 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 | −1704.1 | −1630.6 | 794 | – |
per 1 mol of | −568.03 | −543.53 | 265 | – |
per 1 mol of | −426.02 | −407.65 | 199 | – |
per 1 mol of | −568.03 | −543.53 | 265 | – |
| −852.05 | −815.30 | 397 | – | |
| −852.05 | −815.30 | 397 | – |
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 |
|---|---|---|---|---|
| ZnS (cr) | -205.98[1] | -201.29[1] | 57.7[1] | 46.0[1] |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (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 |
|---|---|---|---|---|
| ZnSO4 (cr) | -982.8[1] | -871.5[1] | 110.5[1] | 99.2[1] |
| ZnSO4 (ai) | -1063.15[1] | -891.59[1] | -92.0[1] | -247[1] |
| ZnSO4 (ao) | -1047.7[1] | -904.9[1] | 5.0[1] | – |
| ZnSO4 (cr) 1 hydrate | -1304.49[1] | -1131.99[1] | 138.5[1] | – |
| ZnSO4 (cr) 6 hydrate | -2777.46[1] | -2324.44[1] | 363.6[1] | 357.69[1] |
| ZnSO4 (cr) 7 hydrate | -3077.75[1] | -2562.67[1] | 388.7[1] | 383.42[1] |
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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°, -205.98 kJ · mol−1
- ^ ΔfG°, -201.29 kJ · mol−1
- ^ S°, 57.7 J · K−1 · mol−1
- ^ Cp°, 46.0 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -982.8 kJ · mol−1
- ^ ΔfG°, -871.5 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ Cp°, 99.2 J · K−1 · mol−1
- ^ ΔfH°, -1063.15 kJ · mol−1
- ^ ΔfG°, -891.59 kJ · mol−1
- ^ S°, -92.0 J · K−1 · mol−1
- ^ Cp°, -247. J · K−1 · mol−1
- ^ ΔfH°, -1047.7 kJ · mol−1
- ^ ΔfG°, -904.9 kJ · mol−1
- ^ S°, 5.0 J · K−1 · mol−1
- ^ ΔfH°, -1304.49 kJ · mol−1
- ^ ΔfG°, -1131.99 kJ · mol−1
- ^ S°, 138.5 J · K−1 · mol−1
- ^ ΔfH°, -2777.46 kJ · mol−1
- ^ ΔfG°, -2324.44 kJ · mol−1
- ^ S°, 363.6 J · K−1 · mol−1
- ^ Cp°, 357.69 J · K−1 · mol−1
- ^ ΔfH°, -3077.75 kJ · mol−1
- ^ ΔfG°, -2562.67 kJ · mol−1
- ^ S°, 388.7 J · K−1 · mol−1
- ^ Cp°, 383.42 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1