HgS + I2 → HgI2 + S
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- Reaction of mercury(II) sulfide and
The reaction of mercury(II) sulfide and yields mercury(II) iodide and . This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of mercury(II) sulfide and
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 mercury(II) sulfide and
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
HgS | Mercury(II) sulfide | 1 | Reducing | Reducing |
1 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
HgI2 | Mercury(II) iodide | 1 | Reduced | – |
1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of mercury(II) sulfide and ◆
ΔrG −51.1 kJ/mol K 8.96 × 108 pK −8.95
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 | −47.2 | −51.1 | 13 | – |
per 1 mol of | −47.2 | −51.1 | 13 | – |
−47.2 | −51.1 | 13 | – | |
per 1 mol of | −47.2 | −51.1 | 13 | – |
−47.2 | −51.1 | 13 | – |
Changes in standard condition (2)
- Reaction of mercury(II) sulfide and
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 | −46.9 | – | – | – |
per 1 mol of | −46.9 | – | – | – |
−46.9 | – | – | – | |
per 1 mol of | −46.9 | – | – | – |
−46.9 | – | – | – |
Changes in standard condition (3)
- Reaction of mercury(II) sulfide and
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 | −44.7 | – | – | – |
per 1 mol of | −44.7 | – | – | – |
−44.7 | – | – | – | |
per 1 mol of | −44.7 | – | – | – |
−44.7 | – | – | – |
Changes in standard condition (4)
- Reaction of mercury(II) sulfide and
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 | −44.4 | – | – | – |
per 1 mol of | −44.4 | – | – | – |
−44.4 | – | – | – | |
per 1 mol of | −44.4 | – | – | – |
−44.4 | – | – | – |
Changes in standard condition (5)
- Reaction of mercury(II) sulfide and ◆
ΔrG −54.0 kJ/mol K 2.89 × 109 pK −9.46
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 | −51.8 | −54.0 | 7 | – |
per 1 mol of | −51.8 | −54.0 | 7 | – |
−51.8 | −54.0 | 7 | – | |
per 1 mol of | −51.8 | −54.0 | 7 | – |
−51.8 | −54.0 | 7 | – |
Changes in standard condition (6)
- Reaction of mercury(II) sulfide and
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 | −51.5 | – | – | – |
per 1 mol of | −51.5 | – | – | – |
−51.5 | – | – | – | |
per 1 mol of | −51.5 | – | – | – |
−51.5 | – | – | – |
Changes in standard condition (7)
- Reaction of mercury(II) sulfide and
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 | −49.3 | – | – | – |
per 1 mol of | −49.3 | – | – | – |
−49.3 | – | – | – | |
per 1 mol of | −49.3 | – | – | – |
−49.3 | – | – | – |
Changes in standard condition (8)
- Reaction of mercury(II) sulfide and
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 | −49.0 | – | – | – |
per 1 mol of | −49.0 | – | – | – |
−49.0 | – | – | – | |
per 1 mol of | −49.0 | – | – | – |
−49.0 | – | – | – |
Changes in aqueous solution
- Reaction of mercury(II) sulfide and ◆
ΔrG −41.1 kJ/mol K 1.59 × 107 pK −7.20
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 | −43.9 | −41.1 | −12 | – |
per 1 mol of | −43.9 | −41.1 | −12 | – |
−43.9 | −41.1 | −12 | – | |
per 1 mol of | −43.9 | −41.1 | −12 | – |
−43.9 | −41.1 | −12 | – |
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 |
---|---|---|---|---|
HgS (cr) red | -58.2[1] | -50.6[1] | 82.4[1] | 48.41[1] |
HgS (cr) black | -53.6[1] | -47.7[1] | 88.3[1] | – |
HgS (g) | – | – | 254.75[1] | – |
(cr) | 0[1] | 0[1] | 116.135[1] | 54.438[1] |
(g) | 62.438[1] | 19.327[1] | 260.69[1] | 36.90[1] |
(ao) | 22.6[1] | 16.40[1] | 137.2[1] | – |
* (cr):Crystalline solid, (g):Gas, (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 |
---|---|---|---|---|
HgI2 (cr) red | -105.4[1] | -101.7[1] | 180[1] | – |
HgI2 (cr) yellow | -102.9[1] | – | – | – |
HgI2 (g) | -17.2[1] | -59.9[1] | 336.13[1] | 61.09[1] |
HgI2 (ao) | -79.5[1] | -75.3[1] | 176[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] |
* (cr):Crystalline solid, (g):Gas, (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°, -58.2 kJ · mol−1
- ^ ΔfG°, -50.6 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, 48.41 J · K−1 · mol−1
- ^ ΔfH°, -53.6 kJ · mol−1
- ^ ΔfG°, -47.7 kJ · mol−1
- ^ S°, 88.3 J · K−1 · mol−1
- ^ S°, 254.75 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 116.135 J · K−1 · mol−1
- ^ Cp°, 54.438 J · K−1 · mol−1
- ^ ΔfH°, 62.438 kJ · mol−1
- ^ ΔfG°, 19.327 kJ · mol−1
- ^ S°, 260.69 J · K−1 · mol−1
- ^ Cp°, 36.90 J · K−1 · mol−1
- ^ ΔfH°, 22.6 kJ · mol−1
- ^ ΔfG°, 16.40 kJ · mol−1
- ^ S°, 137.2 J · K−1 · mol−1
- ^ ΔfH°, -105.4 kJ · mol−1
- ^ ΔfG°, -101.7 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ ΔfH°, -102.9 kJ · mol−1
- ^ ΔfH°, -17.2 kJ · mol−1
- ^ ΔfG°, -59.9 kJ · mol−1
- ^ S°, 336.13 J · K−1 · mol−1
- ^ Cp°, 61.09 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -75.3 kJ · mol−1
- ^ S°, 176. J · K−1 · 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