Pb(OH)2 + N2O5 → Pb(NO3)2 + H2O
Last updated:
The reaction of lead(II) hydroxide and dinitrogen pentaoxide yields lead(II) nitrate and water. This reaction is an acid-base reaction and is classified as follows:
- Reaction of base and acidic oxide
- Reaction of hydroxide base and acidic oxide
- Reaction of weak hydroxide base and strongly acidic oxide
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) hydroxide and dinitrogen pentaoxide
General equation
- Reaction of base and acidic oxide
- BaseLewis base + Acidic oxideLewis acid + H2O ⟶ Oxoacid saltLewis conjugate + (H2O)
- Reaction of hydroxide base and acidic oxide
- Hydroxide baseLewis base + Acidic oxideLewis acid ⟶ Oxoacid saltLewis conjugate + H2O
- Reaction of weak hydroxide base and strongly acidic oxide
- Weak hydroxide baseLewis base + Strongly acidic oxideLewis acid ⟶ Salt of strong acid and weak baseLewis conjugate + H2O
Oxidation state of each atom
- Reaction of lead(II) hydroxide and dinitrogen pentaoxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(OH)2 | Lead(II) hydroxide | 1 | Lewis base | Base Hydroxide base Weak hydroxide base |
| N2O5 | Dinitrogen pentaoxide | 1 | Lewis acid | Acidic oxide Strongly acidic oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Pb(NO3)2 | Lead(II) nitrate | 1 | Lewis conjugate | Oxoacid salt Salt of strong acid and weak base |
| H2O | Water | 1 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of lead(II) hydroxide and dinitrogen pentaoxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (2)
- Reaction of lead(II) hydroxide and dinitrogen pentaoxide
| 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 | −178.7 | – | – | – |
per 1 mol of | −178.7 | – | – | – |
per 1 mol of | −178.7 | – | – | – |
per 1 mol of | −178.7 | – | – | – |
per 1 mol of | −178.7 | – | – | – |
Changes in aqueous solution
- Reaction of lead(II) hydroxide and dinitrogen pentaoxide◆
ΔrG −145.8 kJ/mol K 3.49 × 1025 pK −25.54
| 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 | – | −145.8 | – | – |
per 1 mol of | – | −145.8 | – | – |
per 1 mol of | – | −145.8 | – | – |
per 1 mol of | – | −145.8 | – | – |
per 1 mol of | – | −145.8 | – | – |
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 |
|---|---|---|---|---|
| Pb(OH)2 (cr) | – | -452.2[1] | – | – |
| Pb(OH)2 (cr) precipitated | -515.9[1] | – | – | – |
| N2O5 (cr) | -43.1[1] | 113.9[1] | 178.2[1] | 143.1[1] |
| N2O5 (g) | 11.3[1] | 115.1[1] | 355.7[1] | 84.5[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 |
|---|---|---|---|---|
| Pb(NO3)2 (cr) | -451.9[1] | – | – | – |
| Pb(NO3)2 (ai) | -416.3[1] | -246.93[1] | 303.3[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, (ai):Ionized aqueous solution, (l):Liquid, (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)
- ^ ΔfG°, -452.2 kJ · mol−1
- ^ ΔfH°, -515.9 kJ · mol−1
- ^ ΔfH°, -43.1 kJ · mol−1
- ^ ΔfG°, 113.9 kJ · mol−1
- ^ S°, 178.2 J · K−1 · mol−1
- ^ Cp°, 143.1 J · K−1 · mol−1
- ^ ΔfH°, 11.3 kJ · mol−1
- ^ ΔfG°, 115.1 kJ · mol−1
- ^ S°, 355.7 J · K−1 · mol−1
- ^ Cp°, 84.5 J · K−1 · mol−1
- ^ ΔfH°, -451.9 kJ · mol−1
- ^ ΔfH°, -416.3 kJ · mol−1
- ^ ΔfG°, -246.93 kJ · mol−1
- ^ S°, 303.3 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