Zn(SCN)2 + 11Fe2O3 → ZnSO4 + FeSO4 + N2↑ + 2FeCO3 + 19FeO
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- Reaction of zinc thiocyanate and iron(III) oxide
The reaction of zinc thiocyanate and iron(III) oxide yields zinc sulfate, iron(II) sulfate, , iron(II) carbonate, and iron(II) oxide (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 thiocyanate and iron(III) oxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of zinc thiocyanate and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn(SCN)2 | Zinc thiocyanate | 1 | Reducing | Reducing |
| Fe2O3 | Iron(III) oxide | 11 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| ZnSO4 | Zinc sulfate | 1 | Oxidized | – |
| FeSO4 | Iron(II) sulfate | 1 | Redoxed product | – |
| 1 | Oxidized | – | ||
| FeCO3 | Iron(II) carbonate | 2 | Reduced | – |
| FeO | Iron(II) oxide | 19 | Reduced | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of zinc thiocyanate and iron(III) oxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (2)
- Reaction of zinc thiocyanate and iron(III) oxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (3)
- Reaction of zinc thiocyanate and iron(III) oxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
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 |
|---|---|---|---|---|
| Zn(SCN)2 (ao) | – | 33.1[1] | – | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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] |
| FeSO4 (cr) | -928.4[1] | -820.8[1] | 107.5[1] | 100.58[1] |
| FeSO4 (ai) | -998.3[1] | -823.43[1] | -117.6[1] | – |
| FeSO4 (cr) 1 hydrate | -1243.69[1] | – | – | – |
| FeSO4 (cr) 4 hydrate | -2129.2[1] | – | – | – |
| FeSO4 (cr) 7 hydrate | -3014.57[1] | -2509.87[1] | 409.2[1] | 394.47[1] |
| (g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
| FeCO3 (cr) siderite | -740.57[1] | -666.67[1] | 92.9[1] | 82.13[1] |
| FeO (cr) | -272.0[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)
- ^ ΔfG°, 33.1 kJ · mol−1
- ^ ΔfH°, -824.2 kJ · mol−1
- ^ ΔfG°, -742.2 kJ · mol−1
- ^ S°, 87.40 J · K−1 · mol−1
- ^ Cp°, 103.85 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°, -928.4 kJ · mol−1
- ^ ΔfG°, -820.8 kJ · mol−1
- ^ S°, 107.5 J · K−1 · mol−1
- ^ Cp°, 100.58 J · K−1 · mol−1
- ^ ΔfH°, -998.3 kJ · mol−1
- ^ ΔfG°, -823.43 kJ · mol−1
- ^ S°, -117.6 J · K−1 · mol−1
- ^ ΔfH°, -1243.69 kJ · mol−1
- ^ ΔfH°, -2129.2 kJ · mol−1
- ^ ΔfH°, -3014.57 kJ · mol−1
- ^ ΔfG°, -2509.87 kJ · mol−1
- ^ S°, 409.2 J · K−1 · mol−1
- ^ Cp°, 394.47 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°, -740.57 kJ · mol−1
- ^ ΔfG°, -666.67 kJ · mol−1
- ^ S°, 92.9 J · K−1 · mol−1
- ^ Cp°, 82.13 J · K−1 · mol−1
- ^ ΔfH°, -272.0 kJ · mol−1