Pb + 2N2O3 → PbO2 + 4NO
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- Reaction of and dinitrogen trioxide
The reaction of and dinitrogen trioxide yields lead(IV) oxide and nitrogen monoxide (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 dinitrogen trioxide
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and dinitrogen trioxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
1 | Reducing | Reducing | ||
N2O3 | Dinitrogen trioxide | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbO2 | Lead(IV) oxide | 1 | Oxidized | – |
NO | Nitrogen monoxide | 4 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and dinitrogen trioxide◆
ΔrG −150.05 kJ/mol K 1.94 × 1026 pK −26.29
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 | −83.8 | −150.05 | 222.3 | 26.36 |
−83.8 | −150.05 | 222.3 | 26.36 | |
per 1 mol of | −41.9 | −75.025 | 111.2 | 13.18 |
per 1 mol of | −83.8 | −150.05 | 222.3 | 26.36 |
per 1 mol of | −20.9 | −37.513 | 55.58 | 6.590 |
Changes in aqueous solution
- Reaction of and dinitrogen trioxide
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 | −17.0 | – | – | – |
−17.0 | – | – | – | |
per 1 mol of | −8.50 | – | – | – |
per 1 mol of | −17.0 | – | – | – |
per 1 mol of | −4.25 | – | – | – |
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] |
N2O3 (l) | 50.29[1] | – | – | – |
N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[1] |
* (cr):Crystalline solid, (g):Gas, (l):Liquid
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 |
---|---|---|---|---|
PbO2 (cr) | -277.4[1] | -217.33[1] | 68.6[1] | 64.64[1] |
NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[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°, 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°, 50.29 kJ · mol−1
- ^ ΔfH°, 83.72 kJ · mol−1
- ^ ΔfG°, 139.46 kJ · mol−1
- ^ S°, 312.28 J · K−1 · mol−1
- ^ Cp°, 65.61 J · K−1 · mol−1
- ^ ΔfH°, -277.4 kJ · mol−1
- ^ ΔfG°, -217.33 kJ · mol−1
- ^ S°, 68.6 J · K−1 · mol−1
- ^ Cp°, 64.64 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · mol−1