6Na + Pb(OH)2 → 2Na2O + 2NaH + Pb
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- Reaction of and lead(II) hydroxide
The reaction of and lead(II) hydroxide yields sodium oxide, sodium hydride, and (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 lead(II) hydroxide
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 lead(II) hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 6 | Reducing | Reducing | ||
| Pb(OH)2 | Lead(II) hydroxide | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2O | Sodium oxide | 2 | Oxidized | – |
| NaH | Sodium hydride | 2 | Redoxed product | – |
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and lead(II) hydroxide◆
ΔrG −365.6 kJ/mol K 1.12 × 1064 pK −64.05
| 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 | – | −365.6 | – | – |
| – | −60.93 | – | – | |
per 1 mol of | – | −365.6 | – | – |
per 1 mol of | – | −182.8 | – | – |
per 1 mol of | – | −182.8 | – | – |
| – | −365.6 | – | – |
Changes in standard condition (2)
- Reaction of and lead(II) hydroxide
| 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 | −425.1 | – | – | – |
| −70.85 | – | – | – | |
per 1 mol of | −425.1 | – | – | – |
per 1 mol of | −212.6 | – | – | – |
per 1 mol of | −212.6 | – | – | – |
| −425.1 | – | – | – |
Changes in aqueous solution
- Reaction of and lead(II) hydroxide◆
ΔrG −365.6 kJ/mol K 1.12 × 1064 pK −64.05
| 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 | – | −365.6 | – | – |
| – | −60.93 | – | – | |
per 1 mol of | – | −365.6 | – | – |
per 1 mol of | – | −182.8 | – | – |
per 1 mol of | – | −182.8 | – | – |
| – | −365.6 | – | – |
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] | 51.21[1] | 28.24[1] |
| (g) | 107.32[1] | 76.761[1] | 153.712[1] | 20.786[1] |
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[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 |
|---|---|---|---|---|
| Na2O (cr) | -414.22[1] | -375.46[1] | 75.06[1] | 69.12[1] |
| Na2O (g) | -35.6[1] | -52.3[1] | 261.2[1] | 55.2[1] |
| NaH (cr) | -56.275[1] | -33.46[1] | 40.016[1] | 36.401[1] |
| NaH (g) | 130.25[1] | 108.85[1] | 188.377[1] | 30.29[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] |
* (cr):Crystalline solid, (g):Gas
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°, 51.21 J · K−1 · mol−1
- ^ Cp°, 28.24 J · K−1 · mol−1
- ^ ΔfH°, 107.32 kJ · mol−1
- ^ ΔfG°, 76.761 kJ · mol−1
- ^ S°, 153.712 J · K−1 · mol−1
- ^ Cp°, 20.786 J · K−1 · mol−1
- ^ ΔfG°, -452.2 kJ · mol−1
- ^ ΔfH°, -515.9 kJ · mol−1
- ^ ΔfH°, -414.22 kJ · mol−1
- ^ ΔfG°, -375.46 kJ · mol−1
- ^ S°, 75.06 J · K−1 · mol−1
- ^ Cp°, 69.12 J · K−1 · mol−1
- ^ ΔfH°, -35.6 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 261.2 J · K−1 · mol−1
- ^ Cp°, 55.2 J · K−1 · mol−1
- ^ ΔfH°, -56.275 kJ · mol−1
- ^ ΔfG°, -33.46 kJ · mol−1
- ^ S°, 40.016 J · K−1 · mol−1
- ^ Cp°, 36.401 J · K−1 · mol−1
- ^ ΔfH°, 130.25 kJ · mol−1
- ^ ΔfG°, 108.85 kJ · mol−1
- ^ S°, 188.377 J · K−1 · mol−1
- ^ Cp°, 30.29 J · K−1 · mol−1
- ^ 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