HgSO4 🔥→ HgO + SO3
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- Decomposition of mercury(II) sulfate
Decomposition of mercury(II) sulfate yields mercury(II) oxide and sulfur trioxide (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
- Thermal decomposition without redox
- Thermal decomposition of oxoacid salt without redox
- Thermal decomposition of salt of oxoacid and hydroxide base
Table of contents
Reaction data
Chemical equation
- Decomposition of mercury(II) sulfate
General equation
- Thermal decomposition without redox
- Thermally decomposable substanceLewis conjugate🔥⟶ ProductLewis acid + ProductLewis base
- Thermal decomposition of oxoacid salt without redox
- Oxoacid saltLewis conjugate🔥⟶ Basic oxideLewis base + Acidic oxideLewis acid + (H2O)
- Thermal decomposition of salt of oxoacid and hydroxide base
- Salt of oxoacid and hydroxide baseLewis conjugate🔥⟶ Basic oxideLewis base + Acidic oxideLewis acid
Oxidation state of each atom
- Decomposition of mercury(II) sulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgSO4 | Mercury(II) sulfate | 1 | Lewis conjugate | Thermally decomposable Oxoacid salt Salt of oxoacid and hydroxide base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HgO | Mercury(II) oxide | 1 | Lewis acid Lewis base | – Basic oxide |
| SO3 | Sulfur trioxide | 1 | Lewis acid | – Acidic oxide |
Thermodynamic changes
Changes in standard condition (1)
- Decomposition of 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 | 175.6 | – | – | – |
per 1 mol of | 175.6 | – | – | – |
per 1 mol of | 175.6 | – | – | – |
per 1 mol of | 175.6 | – | – | – |
Changes in standard condition (2)
- Decomposition of 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 | 176.0 | – | – | – |
per 1 mol of | 176.0 | – | – | – |
per 1 mol of | 176.0 | – | – | – |
per 1 mol of | 176.0 | – | – | – |
Changes in standard condition (3)
- Decomposition of 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 | 177.0 | – | – | – |
per 1 mol of | 177.0 | – | – | – |
per 1 mol of | 177.0 | – | – | – |
per 1 mol of | 177.0 | – | – | – |
Changes in aqueous solution
- Decomposition of mercury(II) sulfate◆
ΔrG 155.5 kJ/mol K 0.57 × 10−27 pK 27.24
| 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 | – | 155.5 | – | – |
per 1 mol of | – | 155.5 | – | – |
per 1 mol of | – | 155.5 | – | – |
per 1 mol of | – | 155.5 | – | – |
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 |
|---|---|---|---|---|
| HgSO4 (cr) | -707.5[1] | – | – | – |
| HgSO4 (ao) | – | -588.2[1] | – | – |
* (cr):Crystalline solid, (ao):Un-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 |
|---|---|---|---|---|
| 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] |
| 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] |
* (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°, -707.5 kJ · mol−1
- ^ ΔfG°, -588.2 kJ · 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°, -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