3Hg2Cl2 + 10Fe2O3 🔥→ 6HgO + 6Fe3O4 + 2FeCl3
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The reaction of mercury(I) chloride and iron(III) oxide yields mercury(II) oxide, iron(II,III) oxide, and iron(III) chloride (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 mercury(I) chloride and iron(III) oxide
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of mercury(I) chloride and iron(III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Hg2Cl2 | Mercury(I) chloride | 3 | Reducing | Oxidizable |
| Fe2O3 | Iron(III) oxide | 10 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgO | Mercury(II) oxide | 6 | Oxidized | – |
| Fe3O4 | Iron(II,III) oxide | 6 | Reduced | – |
| FeCl3 | Iron(III) chloride | 2 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of mercury(I) chloride and iron(III) oxide◆
ΔrG 942.6 kJ/mol K 0.73 × 10−165 pK 165.14
| 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 | 983.3 | 942.6 | 133.2 | – |
per 1 mol of | 327.8 | 314.2 | 44.40 | – |
per 1 mol of | 98.33 | 94.26 | 13.32 | – |
per 1 mol of | 163.9 | 157.1 | 22.20 | – |
per 1 mol of | 163.9 | 157.1 | 22.20 | – |
per 1 mol of | 491.6 | 471.3 | 66.60 | – |
Changes in standard condition (2)
- Reaction of mercury(I) chloride and iron(III) oxide◆
ΔrG 943.4 kJ/mol K 0.53 × 10−165 pK 165.28
| 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 | 985.5 | 943.4 | 138.1 | – |
per 1 mol of | 328.5 | 314.5 | 46.03 | – |
per 1 mol of | 98.55 | 94.34 | 13.81 | – |
per 1 mol of | 164.3 | 157.2 | 23.02 | – |
per 1 mol of | 164.3 | 157.2 | 23.02 | – |
per 1 mol of | 492.8 | 471.7 | 69.05 | – |
Changes in standard condition (3)
- Reaction of mercury(I) chloride and iron(III) oxide◆
ΔrG 944.5 kJ/mol K 0.34 × 10−165 pK 165.47
| 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 | 991.3 | 944.5 | 153.1 | – |
per 1 mol of | 330.4 | 314.8 | 51.03 | – |
per 1 mol of | 99.13 | 94.45 | 15.31 | – |
per 1 mol of | 165.2 | 157.4 | 25.52 | – |
per 1 mol of | 165.2 | 157.4 | 25.52 | – |
per 1 mol of | 495.6 | 472.3 | 76.55 | – |
Changes in aqueous solution (1)
- Reaction of mercury(I) chloride and iron(III) oxide◆
ΔrG 801.6 kJ/mol K 0.37 × 10−140 pK 140.43
| 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 | – | 801.6 | – | – |
per 1 mol of | – | 267.2 | – | – |
per 1 mol of | – | 80.16 | – | – |
per 1 mol of | – | 133.6 | – | – |
per 1 mol of | – | 133.6 | – | – |
per 1 mol of | – | 400.8 | – | – |
Changes in aqueous solution (2)
- Reaction of mercury(I) chloride and iron(III) oxide◆
ΔrG 814.0 kJ/mol K 0.25 × 10−142 pK 142.61
| 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 | 681.9 | 814.0 | −444.2 | – |
per 1 mol of | 227.3 | 271.3 | −148.1 | – |
per 1 mol of | 68.19 | 81.40 | −44.42 | – |
per 1 mol of | 113.6 | 135.7 | −74.03 | – |
per 1 mol of | 113.6 | 135.7 | −74.03 | – |
per 1 mol of | 340.9 | 407.0 | −222.1 | – |
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 |
|---|---|---|---|---|
| Hg2Cl2 (cr) | -265.22[1] | -210.745[1] | 192.5[1] | – |
| Fe2O3 (cr) | -824.2[1] | -742.2[1] | 87.40[1] | 103.85[1] |
* (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 |
|---|---|---|---|---|
| HgO (cr) red, orthorhombic | -90.83[1] | -58.539[1] | 70.29[1] | 44.06[1] |
| HgO (cr) yellow | -90.46[1] | -58.409[1] | 71.1[1] | – |
| HgO (cr) hexagonal | -89.5[1] | -58.22[1] | 73.6[1] | – |
| HgO (g) | – | – | 241.9[1] | 34.10[1] |
| Fe3O4 (cr) | -1118.4[1] | -1015.4[1] | 146.4[1] | 143.43[1] |
| FeCl3 (cr) | -399.49[1] | -334.00[1] | 142.3[1] | 96.65[1] |
| FeCl3 (g) | -254.0[1] | – | – | – |
| FeCl3 (ai) | -550.2[1] | -398.3[1] | -146.4[1] | – |
| FeCl3 (ao) | – | -404.5[1] | – | – |
| FeCl3 (cr) 6 hydrate | -2223.8[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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°, -265.22 kJ · mol−1
- ^ ΔfG°, -210.745 kJ · mol−1
- ^ S°, 192.5 J · K−1 · 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°, -90.83 kJ · mol−1
- ^ ΔfG°, -58.539 kJ · mol−1
- ^ S°, 70.29 J · K−1 · mol−1
- ^ Cp°, 44.06 J · K−1 · mol−1
- ^ ΔfH°, -90.46 kJ · mol−1
- ^ ΔfG°, -58.409 kJ · mol−1
- ^ S°, 71.1 J · K−1 · mol−1
- ^ ΔfH°, -89.5 kJ · mol−1
- ^ ΔfG°, -58.22 kJ · mol−1
- ^ S°, 73.6 J · K−1 · mol−1
- ^ S°, 241.9 J · K−1 · mol−1
- ^ Cp°, 34.10 J · K−1 · mol−1
- ^ ΔfH°, -1118.4 kJ · mol−1
- ^ ΔfG°, -1015.4 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, 143.43 J · K−1 · mol−1
- ^ ΔfH°, -399.49 kJ · mol−1
- ^ ΔfG°, -334.00 kJ · mol−1
- ^ S°, 142.3 J · K−1 · mol−1
- ^ Cp°, 96.65 J · K−1 · mol−1
- ^ ΔfH°, -254.0 kJ · mol−1
- ^ ΔfH°, -550.2 kJ · mol−1
- ^ ΔfG°, -398.3 kJ · mol−1
- ^ S°, -146.4 J · K−1 · mol−1
- ^ ΔfG°, -404.5 kJ · mol−1
- ^ ΔfH°, -2223.8 kJ · mol−1