Pb + F2 → PbF2
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The reaction of and yields lead(II) fluoride. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
- Reducing agent + Oxidizing agent ⟶ Binary compoundOxidation reduction product
Oxidation state of each atom
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing Metal | ||
| 1 | Oxidizing | Oxidizing Nonmetal |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbF2 | Lead(II) fluoride | 1 | Redoxed product | – Binary compound |
Thermodynamic changes
Changes in standard condition
| 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 | −664.0 | −617.1 | −157.1 | – |
| −664.0 | −617.1 | −157.1 | – | |
| −664.0 | −617.1 | −157.1 | – | |
per 1 mol of | −664.0 | −617.1 | −157.1 | – |
Changes in aqueous solution (1)
| 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 | – | −596.6 | – | – |
| – | −596.6 | – | – | |
| – | −596.6 | – | – | |
per 1 mol of | – | −596.6 | – | – |
Changes in aqueous solution (2)
| 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 | −664.0 | −617.1 | −157.1 | – |
| −664.0 | −617.1 | −157.1 | – | |
| −664.0 | −617.1 | −157.1 | – | |
per 1 mol of | −664.0 | −617.1 | −157.1 | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 64.81[1] | 26.44[1] |
| (g) | 195.0[1] | 161.9[1] | 175.373[1] | 20.786[1] |
| (g) | 0[1] | 0[1] | 202.78[1] | 31.30[1] |
* (cr):Crystalline solid, (g):Gas
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 |
|---|---|---|---|---|
| PbF2 (cr) | -664.0[1] | -617.1[1] | 110.5[1] | – |
| PbF2 (ai) | -666.9[1] | -582.00[1] | -17.2[1] | – |
| PbF2 (ao) | – | -596.6[1] | – | – |
* (cr):Crystalline solid, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 64.81 J · K−1 · mol−1
- ^ Cp°, 26.44 J · K−1 · mol−1
- ^ ΔfH°, 195.0 kJ · mol−1
- ^ ΔfG°, 161.9 kJ · mol−1
- ^ S°, 175.373 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 202.78 J · K−1 · mol−1
- ^ Cp°, 31.30 J · K−1 · mol−1
- ^ ΔfH°, -664.0 kJ · mol−1
- ^ ΔfG°, -617.1 kJ · mol−1
- ^ S°, 110.5 J · K−1 · mol−1
- ^ ΔfH°, -666.9 kJ · mol−1
- ^ ΔfG°, -582.00 kJ · mol−1
- ^ S°, -17.2 J · K−1 · mol−1
- ^ ΔfG°, -596.6 kJ · mol−1