3H2 + HgSO4 → S + HgO + 3H2O
Last updated:
- Reaction of and mercury(II) sulfate
The reaction of and mercury(II) sulfate yields , mercury(II) oxide, 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 and mercury(II) sulfate
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 and mercury(II) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 3 | Reducing | Reducing | ||
| HgSO4 | Mercury(II) sulfate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reduced | – | ||
| HgO | Mercury(II) oxide | 1 | – | – |
| H2O | Water | 3 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and mercury(II) sulfate
| 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 | −240.8 | – | – | – |
| −80.27 | – | – | – | |
per 1 mol of | −240.8 | – | – | – |
| −240.8 | – | – | – | |
per 1 mol of | −240.8 | – | – | – |
per 1 mol of | −80.27 | – | – | – |
Changes in standard condition (2)
- Reaction of and mercury(II) sulfate
| 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 | −240.5 | – | – | – |
| −80.17 | – | – | – | |
per 1 mol of | −240.5 | – | – | – |
| −240.5 | – | – | – | |
per 1 mol of | −240.5 | – | – | – |
per 1 mol of | −80.17 | – | – | – |
Changes in standard condition (3)
- Reaction of and mercury(II) sulfate
| 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 | −239.5 | – | – | – |
| −79.83 | – | – | – | |
per 1 mol of | −239.5 | – | – | – |
| −239.5 | – | – | – | |
per 1 mol of | −239.5 | – | – | – |
per 1 mol of | −79.83 | – | – | – |
Changes in standard condition (4)
- Reaction of and mercury(II) sulfate
| 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 | −240.5 | – | – | – |
| −80.17 | – | – | – | |
per 1 mol of | −240.5 | – | – | – |
| −240.5 | – | – | – | |
per 1 mol of | −240.5 | – | – | – |
per 1 mol of | −80.17 | – | – | – |
Changes in standard condition (5)
- Reaction of and mercury(II) sulfate
| 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 | −240.1 | – | – | – |
| −80.03 | – | – | – | |
per 1 mol of | −240.1 | – | – | – |
| −240.1 | – | – | – | |
per 1 mol of | −240.1 | – | – | – |
per 1 mol of | −80.03 | – | – | – |
Changes in standard condition (6)
- Reaction of and mercury(II) sulfate
| 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 | −239.2 | – | – | – |
| −79.73 | – | – | – | |
per 1 mol of | −239.2 | – | – | – |
| −239.2 | – | – | – | |
per 1 mol of | −239.2 | – | – | – |
per 1 mol of | −79.73 | – | – | – |
Changes in aqueous solution
- Reaction of and mercury(II) sulfate◆
ΔrG −234.5 kJ/mol K 1.21 × 1041 pK −41.08
| 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 | – | −234.5 | – | – |
| – | −78.17 | – | – | |
per 1 mol of | – | −234.5 | – | – |
| – | −234.5 | – | – | |
per 1 mol of | – | −234.5 | – | – |
per 1 mol of | – | −78.17 | – | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
| HgSO4 (cr) | -707.5[1] | – | – | – |
| HgSO4 (ao) | – | -588.2[1] | – | – |
* (g):Gas, (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 |
|---|---|---|---|---|
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[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] |
| 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, (g):Gas, (l):Liquid
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°, 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
- ^ ΔfH°, -707.5 kJ · mol−1
- ^ ΔfG°, -588.2 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 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°, -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